SAME BASIC CONCEPT OF CHEMISTRY PDF

QUESTION If the atomic weight of an element is 23 times that of the lightest element and it has 11 protons, then it contains A 11 protons, 23 neutrons, 11 electrons B 11 protons, 11 neutrons, 11 electrons C 11 protons, 12 neutrons, 11 electrons D 11 protons, 11 neutrons, 23 electrons Q...

QUESTION If the atomic weight of an element is 23 times that of the lightest element and it has 11 protons, then it contains A 11 protons, 23 neutrons, 11 electrons B 11 protons, 11 neutrons, 11 electrons C 11 protons, 12 neutrons, 11 electrons D 11 protons, 11 neutrons, 23 electrons QUESTION The number of electrons in the atom which has 20 protons in the nucleus is A 20 B 10 C 30 D 40 QUESTION An atom which has lost one electron would be A Negatively charged B Positively charged C Electrically neutral D Carry double positive charge QUESTION Positive ions are formed from the neutral atom by the A Increase of nuclear charge B Gain of protons C Loss of electrons D Loss of protons QUESTION The nucleus of the atom consists of A Proton and neutron B Proton and electron C Neutron and electron D Proton, neutron and electron QUESTION The number of electrons in [19K40] is A 19 B 20 C 18 D 40 QUESTION In the nucleus of 20Ca40 there are A 40 protons and 20 electrons B 20 protons and 40 electrons C 20 protons and 20 neutrons D 20 protons and 40 neutrons QUESTION Nitrogen atom has an atomic number of 7 and oxygen has an atomic number 8. The total number of electrons in a nitrate ion (NO3–) will be A 8 B 16 C 32 D 64 QUESTION The number of protons, neutrons and electrons in 175Lu71 respectively, are: [NEET-2020] A 71, 104 and 71 B 104, 71 and 71 C 71, 71 and 104 D 175, 104 and 71 QUESTION Chlorine atom differs from chloride ions in the number of A Proton B Neutron C Electrons D Protons and electrons QUESTION The number of neutrons in tripositive aluminum ion with mass number 27 is A 14 B 16 C 18 D 20 QUESTION Atomic number and mass number of an element M are 25 and 52 respectively. The number of electrons, protons and neutrons in M2+ ion are respectively. A 25, 25 and 27 B 25, 27 and 25 C 27, 25 and 27 D 23, 25 and 27 QUESTION Chlorine atom differs from chloride ions in the number of A Proton B Neutron C Electrons D Protons and electrons QUESTION In the nucleus of 20Ca40 there are A 40 protons and 20 electrons B 20 protons and 40 electrons C 20 protons and 20 neutrons D 20 protons and 40 neutrons QUESTION The number of neutrons in tripositive aluminum ion with mass number 27 is A 14 B 16 C 18 D 20 QUESTION Sodium atom differs from sodium ion in the number of A Electron B Protons C Neutrons D Does not differ QUESTION The number of electrons in one molecule of CO2 are A 22 B 44 C 66 D 88 QUESTION 30 atoms of H is present in A 10 molecules of CH4 B 20 molecules of C2H6 C 3 molecules of C4H10 D 5 molecules of C3H8 QUESTION Atomic weight of chlorine is 35.5. It has two isotopes of atomic weight 35 and 37. What is the percentage of the heavier isotope in the sample? A 5 B 10 C 25 D 20 QUESTION B has two isotopes 10B (19%) and 11B (81%). The atomic mass of B is A 10.81 B 11.5 C 11 D 10.5 QUESTION Which of the following statements is/are true? A An element of a substance contains only one kind of atoms. B A compound can be decomposed into its components. C All homogeneous mixtures are called as solutions. D All of these QUESTION Assertion : Solids have definite volume and shape. Reason : In solids, the constituent particles are very close to each other and there is not much freedom of movement. A If both assertion and reason are true and reason is the correct explanation of assertion. B If both assertion and reason are true but reason is not the correct explanation of assertion. C If assertion is true but reason is false. D If both assertion and reason are false. QUESTION Assertion : On heating, a solid usually changes to a liquid and the liquid on further heating changes to the gaseous state. Reason : Arrangement of constituent particles is different in solid, liquid and gaseous state. A If both assertion and reason are true and reason is the correct explanation of assertion. B If both assertion and reason are true but reason is not the correct explanation of assertion. C If assertion is true but reason is false. D If both assertion and reason are false. QUESTION Assertion : Elements and compounds are the examples of pure substances. Reason : The properties of a compound are different from those of its constituent elements. A If both assertion and reason are true and reason is the correct explanation of assertion. B If both assertion and reason are true but reason is not the correct explanation of assertion. C If assertion is true but reason is false. D If both assertion and reason are false. QUESTION Select the correct Statements from the following: A. Atoms of all elements are composed of two fundamental particles. B. The mass of the electron is 9.10939 10–31 kg. C. All the isotopes of a given elements show same chemical properties. D. Protons and electron are collectively known as nucleons. E. Dalton’s atomic theory, regarded the atom as an ultimate particle of matter. Choose the correct answer form the options give below: [NEET-2023] A C, D and E only B A and E only C B, C and E only D A, B and C only QUESTION Average atomic mass of magnesium is 24.31 amu. This magnesium is composed of 79 % of 24Mg and remaining 21% of 25Mg and 26Mg. Calculate % of 26Mg. A 10 B 11 C 15 D 16 QUESTION Chemistry was not studied for its own sake, rather it came up as a result of search for A Philosopher's stone B Elexir of life C Paras D All of the above QUESTION Which of the following environmentally hazardous refrigerant responsible for ozone depletion in the stratosphere? A CFCs (Chlorofluorocarbons) B CFM (Chlorofluoromethane) C CC (Chloroiodocarbons) D CIM (Chloroiodomethane) QUESTION Matter can be classified as mixtures or pure substances. These can be further sub-divided as shown. Matter Mixture Pure substances Homogeneous A mixtures B Compounds The missing terms A and B respectively are A A → microscopic level, B → heterogeneous mixtures B A → heterogeneous mixtures, B → elements C A → homogeneous mixtures, B → elements D A → elements, B → heterogeneous mixtures QUESTION A bivalent metal has an atomic mass of 64u. The molecular mass of the metal nitrate is A 182 B 168 C 192 D 188 QUESTION Total number of atoms represented by the compound CuSO4.5H2O is A 27 B 21 C 5 D 8 QUESTION The two effective drugs which act as life saving drugs for cancer therapy and AIDS victims respectively are A AZT (azidothymidine) and taxol. B taxol and cisplatin. C taxol and AZT (azidothymidine). D AZT (azidothymidine) and cisplatin. QUESTION 1 amu is equal to: A 1/12 of mass of C-12 B 1/14 of mass of O-16 C 1 g of H2 D 1.66  10–24 kg QUESTION The actual molecular mass of chlorine is: A 58.93  10–24 g B 118.57  10–24 g C 58.93  10–24 kg D 118.57  10–24 kg QUESTION The modern atomic weight scale is based on: A C12 B O16 C H1 D C13 QUESTION Molecular weight of SO2 is: A 64 g B 64 amu C 32 g D 32 amu QUESTION What is the mass of a molecule of CH4: A 16 g B 26.6  1022 g C 2.66  10–23 g D 16 NA g QUESTION Twenty molecules of SO3 will weigh as much as...molecules of oxygen A 100 B 50 C 15 D 8 QUESTION The weight of one molecule of a compound C60H122 is A 1.3 × 10–20 g B 5.01 × 10–21 g C 3.72 × 1023 g D 1.4 × 10–21 g QUESTION Calculate total number of electrons in 88g of CO2? A NA B 32 NA C 44 NA D 22 NA QUESTION How many moles of magnesium phosphate, Mg3(PO4)2 will contain 0.25 mole of oxygen atoms? A 2.5 × 102 B 3.125 × 10–2 C 0.02 D 1.25 × 10–2 QUESTION What is the mass of 0.5 moles of O3 molecules? A 16 gm B 20 gm C 40 gm D 24 gm QUESTION Number of atoms present in 49 g of H2SO4? A NA/7 B 7NA C 7NA/2 D 14NA QUESTION The number of oxygen atoms in 4.4 g of CO2 is A 6 × 1023 B 11 × 1023 C 12 × 1023 D 1.2 × 1023 QUESTION Find the number of atoms present in 0.016 g of methane. A 0.5 N0 B 0.005 N0 C N0 D 1.6 N0 QUESTION The number of atoms present in 0.05g of water is A 1.67 × 1023 B 1.67 × 1022 C 5.02 × 1021 D 1.67 × 1021 QUESTION Which has maximum number of oxygen atoms? A 1 gm of O B 1 gm of O2 C 1 gm of O3 D All have same no. of O-atoms QUESTION Which of the following contains the greatest number of atoms? A 1.0 g of butane (C4H10) B 1.0 g of nitrogen (N2) C 1.0 g of silver (Ag) D 1.0 g of water (H2O) QUESTION Find mass of 18.066 × 1023 molecules of NH3? (If atomic mass of N and H are 14 and 1) A 51 g B 34 g C 17 g D None of these QUESTION Find mass of CO2 which have same molecules as present in 68 g of NH3? A 88 g B 176 g C 44 g D 132 g QUESTION Which one of the following pairs of gases contains the same number of molecules A 16 g of O2 and 14 g of N2 B 8 g of O2 and 22 g of CO2 C 28 g of N2 and 22 g of CO2 D 32 g of O2 and 32 g of N2 QUESTION A gaseous mixture contains O2 and N2 in the ratio 1 : 4 by weight. Then the ratio of their number of molecules in the mixture is A 3 : 32 B 7 : 32 C 1:4 D 3 : 16 QUESTION The volume occupied by 4.4 g of CO2 at STP is A 22.4 L B 2.24 L C 0.224 L D 0.1 L QUESTION 11.35 L of a gas at STP weighs 14 g. The gas could be: A N2O B N2 C CO D Both B and C QUESTION 2g of O2 at NTP occupies the volume A 1.4 L B 2.8 L C 11.4 L D 3.2 L QUESTION The maximum number of molecules is present in A 15 L of H2 gas at STP B 5 L of N2 gas at STP C 1.5 g of H2 gas D 5g of O2 gas QUESTION One mole of CH4 contains A 4.0 g atoms of hydrogen B 3.0 g atoms of carbon C 6.02 × 1023 atoms of hydrogen D 1.81 × 1023 molecules of CH4 QUESTION A balanced chemical equation is in accordance with- A Avogadro’s law B Law of constant proportions C Law of conservation of mass D Law of gaseous volumes QUESTION Percentage of copper and oxygen in sample of CuO obtained by different methods were found to be same. This proves the law of- A Constant proportion B Multiple proportion C Reciprocal proportion D None of these QUESTION Two gaseous samples were analyzed. One contained 1.2 g of carbon and 3.2 g of oxygen. The other contained 27.3% carbon and 72.7% oxygen. The experimental data are in accordance with A Law of conservation of mass B Law of definite proportions C Law of reciprocal proportion D Law of multiple proportion QUESTION A sample of calcium carbonate (CaCO3) has the following percentage composition: Ca = 40%, C = 12%, O = 48%. If the law of constant proportions is true, then the weight of calcium in 4 g of a sample of calcium carbonate obtained from another source will be: A 0.016 g B 0.16 g C 1.6 g D 16 g QUESTION The percentage of hydrogen in water and hydrogen peroxide is 11.1 and 5.9% respectively. These figures illustrate- A Law of multiple proportions B Law of conservation of mass C Law of reciprocal proportions D Law of combining volumes QUESTION Nitrogen forms five stable oxides with oxygen of the formula, N2O, NO, N2O3, N2O4, N2O5. The formation of these oxides explains fully the- A Law of definite proportions B Law of partial pressures C Law of multiple proportions D Law of reciprocal proportions QUESTION The law of multiple proportions is illustrated by- A Carbon monoxide and carbon dioxide B Potassium bromide and potassium chloride C Water and heavy water D Calcium hydroxide and barium hydroxide QUESTION 1L of N2 combines with 3L of H2 to form 2L of NH3 under the same conditions. This illustrates the- A Law of constant composition B Law of multiple proportions C Law of reciprocal proportions D Gay Lussac’s law of gaseous volumes QUESTION 6g of carbon combines with 32g of sulphur to form CS2. 12g of C also combine with 32g of oxygen to form carbon dioxide. 10g of sulphur combines with 20g of oxygen to form sulphur dioxide. Which law is illustrated by the above example- A Law of multiple proportions B Law of constant composition C Law of reciprocal proportions D Gay Lussac's law QUESTION Which one of the following represents Avogadro’s hypothesis? A Gases react together in volumes which bear a simple ratio to one another B Equal volumes of all gases under same conditions of temperature and pressure contain equal number of molecules C Equal volumes of all gases under same conditions of temperature and pressure contain equal number of atoms D The rates of diffusion of gases are inversely proportional to the square root of their densities QUESTION 1 mole of atom X has mass, 0.444 times the mass of 1 mole of atom Y. Atomic mass of X is 2.96 times the mass of one atom of C-12. What is the atomic weight of Y. A 15.77 amu B 80 amu C 46.66 amu D 40 amu QUESTION The number of atoms in 0.1 mole of a triatomic gas is A 6.025  1022 B 1.806  1023 C 3.600  1023 D 1.800  1022 QUESTION Which one of the followings has maximum number of atoms? A 1 g of Ag (s) [Atomic mass of Ag = 108] B 1 g of Mg (s) [Atomic mass of Mg = 24] C 1 g of O2 (g) [Atomic mass of O = 16] D 1 g of Li (s) [Atomic mass of Li = 7] QUESTION The number of water molecules in 1 L of water is A 18 B 18 × 1000 C NA D 55.55 NA QUESTION Volume occupied by one molecule of water (density = 1g cm–3) is A 9.0  10-23 cm3 B 6.023  10-23 cm3 C 3  10-23 cm3 D 5.5  10-23 cm3 QUESTION Calculate the mass of 6.022 × 1023 molecules of calcium carbonate. A 50 g B 100 g C 200 g D None of these QUESTION The weight of a molecule of the compound C6H12O6, is about: A 180 g B 3 × 10–22 g C 22 × 10–22 g D 132 g QUESTION What is the charge of 96 amu of S2–? A 2C B 3.2 × 10–19 C C 9.6 × 10 –19 C D 6C QUESTION Calculate number of oxygen atoms in 126 g of HNO3? A 6NA B 2NA C 3NA D 14NA QUESTION The number of atoms present in 16 g of oxygen gas is: A 6.02  1011.5 B 3.01  1023 C 3.01  1011.5 D 6.02  1023 QUESTION The least number of molecules are contained in: A 2 g hydrogen B 8 g oxygen C 4 g nitrogen D 16 g CO2 QUESTION The number of atoms in 4.25 g of 𝐍𝐇𝟑 is approximately A 6  1023 B 2  1023 C 1.5  1023 D 1  1023 QUESTION 16 g of oxygen has same number of molecules as in A 16 g of CO B 28 g of N2 C 24 g of C2 D 1.0 g of H2 QUESTION The number of molecules in 89.6 liters of a gas at NTP are A 6.02 × 1023 B 2 × 6.02 × 1023 C 3 × 6.02 × 10 23 D 4 × 6.02 × 1023 QUESTION 44.8 L of SO2(g) weigh how much gram at STP? A 128 g B 95 g C 24 g D 50 g QUESTION 11.2 L of O3(g) contains how many numbers of molecules? A NA molecules B NA/2 molecules C 2NA molecules D 3NA molecules QUESTION Calculate weight occupied by 12.04 × 1024 molecules of N2(g)? A 280 g B 560 g C 112 g D 200 g QUESTION Number of atoms in 560 g of Fe (atomic mas 56 g mol–1) is A Twice that of 70 g N2 B Half that of 20 g H2 C Both are correct D None of these QUESTION How many H-atoms are present in 0.046 g of ethanol? A 6  1020 B 1.2  1021 C 3  10 21 D 6  1021 QUESTION Number of atoms of oxygen present in 10.6 g of Na2CO3 will be A 6.02  1023 B 12.04  1022 C 1.806  1023 D 31.80  1028 QUESTION Find total number of neutrons in 56 g of CO? 𝟏𝟐 If 𝟔 𝐂 𝐚𝐧𝐝 𝟏𝟔 𝟖 𝐎 if Avogadro’s No. = NA A 28 NA B 22 NA C 11 NA D None of these QUESTION A sample of aluminium has a mass of 54.0 g. What is the mass of the same number of magnesium atoms? (At. wt. Al = 27, Mg = 24) A 12 g B 24 g C 48 g D 96 g QUESTION 5.6 litre of oxygen at STP contains A 6.02 × 1023 atoms B 3.01 × 1023 atoms C 1.505 × 10 23 atoms D 0.7525 × 1023 atoms QUESTION A person adds 1.71 gram of sugar (C12H22O11) in order to sweeten his tea. The number of carbon atoms added are (mol. mass of sugar = 342) A 3.6 × 1022 B 7.2 × 1021 C 0.05 D 6.6 × 1022 QUESTION 3.011 × 1022 atoms of an element weighs 1.15 gm. The atomic mass of the element is: A 10 amu B 2.3 amu C 35.5 amu D 23 amu QUESTION Na2SO4 xH2O has 50% H2O by mass. Hence, x is A 4 B 5 C 6 D 8 QUESTION The hydrated salt 𝐍𝐚𝟐 𝐂𝐎𝟑 ⋅ 𝐱𝐇𝟐 𝐎 undergoes 63% loss in mass on heating and becomes anhydrous. The value of x is: A 10 B 12 C 8 D 18 QUESTION 45.4 L of dinitrogen reacted with 22.7 L of dioxygen and 45.4 L of nitrous oxide was formed. The reaction is given below. 2N2(g) + O2(g) → 2N2O(g) Which law is being obeyed in this experiment? A Law of conservation of mass B Law of definite proportion C Law of multiple proportion D Gay Lussac's law of gaseous volumes QUESTION The mass per cent of different elements present in sodium sulphate, (Na2SO4) respectively are A 32.37; 45.06 and 22.57 B 22.57; 32.37 and 45.06 C 45.06; 32.37 and 40.06 D 32.37; 22.57 and 45.06 QUESTION The number of atoms present in one mole of an element is equal to Avogadro's number. Which of the following element contains the greatest number of atoms? A 4 g He B 46g Na C 0.40 g Ca D 12 g He QUESTION What is the mass per cent of carbon in carbon dioxide? A 0.034% B 27.27% C 3.4% D 28.7% QUESTION Which of the following reactions is not correct according to the law of conservation of mass? A 2Mg(s) + O2(g) → 2MgO(s) B C3H8(S) + O2(g) → CO2(g) + H2O(g) C P1(s) + 5O2(g) → P4O10(s) D CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) QUESTION A compound has haemoglobin like structure. It has one Fe. It contains 5.6% of Fe. The approximate molecular mass is A 1000 B 1200 C 1400 D 1600 QUESTION A compound possesses 8% sulphur by mass. The least molecular mass is? [AIIMS 2015] A 200 B 400 C 155 D 355 QUESTION The percentage of Se in peroxidase enzyme is 0.5% by mass (atomic mass of Se = 78.4 amu). Then, the minimum molecular mass of enzyme which contains not more than one Se atom is: QUESTION The empirical formula and molecular mass of a compound are CH2O and 180 g respectively. What will be the molecular formula of the compound? A C9H18O9 B CH2O C C6H12O6 D C2H4O2 QUESTION The simplest formula of the compound containing 50% X (atomic mass 10 amu) and 50% Y (atomic mass 20 amu) is: QUESTION Calculate the empirical formula if a compound has C, H & N in the ratio 9 : 1 : 3.5. Also calculate its Molecular Formula if Molecular mass is 108. QUESTION An organic compound contains 78% (by wt. carbon and remaining percentage of hydrogen. The right option for the empirical formula of this compound A CH3 B CH4 C CH D CH2 QUESTION An oxide of iodine (atomic mass = 127) contains 25.4 g of iodine and 8 g of oxygen. Its formula would be A I2 O 3 B I2 O C I2 O 5 D I2 O 7 QUESTION 0.30 g of an organic compound containing C, H and O on combustion yields 0.44 g CO2 and 0.18 g H2O. If one mole of compound weighs 60 g, then molecular formula of the compound is A C3H8O B C2H4O2 C CH2O D C4H6O QUESTION An organic compound containing C, H and O has 49.3% carbon, 6.84% hydrogen and its vapour density is 73. Molecular formula of the compound is A C3H5O2 B C4H10O2 C C6H10O4 D C3H10O2 QUESTION An organic compound on analysis was found to contain 10.06% carbon, 0.84% hydrogen and 89.10% chlorine. What will be the empirical formula of the substance? A CH2Cl2 B CHCl3 C CCl4 D CH3Cl QUESTION Insulin contains 3.4% sulphur. The minimum mol. wt. of insulin is: A 941.176 B 944 C 945.27 D None QUESTION What will be the mass of one 12C atom in gram? A 2.227  10–23 g B 1.9927  10–23 g C 2.227  10–20 g D 1.9927  10–19 g QUESTION Match the following Column I with Column II and choose the correct codes from the option given below. Column I Column II A. 46 g of Na 1. 0.01 mol B. 6.022  1023 molecules of H2O 2. 2 mol C. 0.224 L of O2 at STP 3. 1 mol D. 84 g of N2 4. 6.022  1023 E. 1 mole of any gas 5. 3 mol A B C D E A B C D E A 2 3 5 4 B 1 2 3 4 5 C 4 2 3 4 D 5 4 3 2 QUESTION The formula of a hypothetical gas in (N2)x and its vapour density is 70. Find x? QUESTION A hydrocarbon CnH2n+2 has Vapour density 29. What is the value of n? QUESTION Vapour density of a gas is 11.2. The valume occupied by 11.2 g of this gas at STP is: A 22.4 L B 11.2 L C 1L D 2.25 L QUESTION Find empirical formula of the compound if M = 68% (atomic mass = 34) and remaining 32% oxygen. A MO B M2 O C MO2 D M2O3 QUESTION 0.0833 mole of carbohydrate of empirical formula CH2O contain 1 g of hydrogen. The molecular formula of the carbohydrate is A C5H10O5 B C3H4O3 C C12H22O11 D C6H12O6 QUESTION A compound contains 69.5% oxygen, 30.5% nitrogen and its molecular weight is 92. The formula of compound is A N2O B NO2 C N2O4 D N2O5 QUESTION An organic compound has an empirical formula (CH2O). Its vapour density is 45. The molecular formula of the compound is A CH2O B C2H5O C C2H2O D C3H6O3 QUESTION For complete combustion of 3g ethane find required moles of O2 and formed moles of CO2. Also find volume of O2 and CO2 at STP. QUESTION 𝟑 The equation 𝟐𝐀𝐥(𝐬) + 𝐎𝟐 ՜ 𝐀𝐥𝟐 𝐎𝟑 (𝐬) shows that 𝟐 3 A 2 moles of aluminium react with moles of oxygen to produce one mole of 2 aluminium oxide 3 B 2 atoms of aluminium react with atoms of oxygen to produce one atom of 2 aluminium oxide 3 C 2g of aluminium react with g of oxygen to produce 1 g of aluminium oxide 2 3 D 2g of aluminium react with litres of oxygen to produce 1 g of aluminium oxide 2 QUESTION In the following reaction, if 10 g of H2, react with N2. What will be the volume of NH3 at STP. N2 + 3H2 → 2NH3 QUESTION 0.5 moles of O2 combine with Mg to form oxide MgO. The mass of Mg (At. Mass 24) that has combined is: A 72 g B 36 g C 24 g D 94 g QUESTION What quantity of lime stone on heating will give 56 kg of CaO: A 1000 kg B 56 kg C 44 kg D 100 kg QUESTION In this reaction, 2Al + O2 → Al2O3, 9 grams of Al will react, with A 6 gm O2 B 8 gm O2 C 9 gm O2 D 4 gm O2 QUESTION The number of moles of Ca(HCO3)2 required to prepare 1.50 moles of CO2, according to the equation Ca(HCO3)2 + 2HCl → CaCl2 + 2CO2 + 2H2O is A 1.00 mol B 2.00 mol C 0.750 mol D 1.50 mol QUESTION Find maximum moles of CCl4 formed when 10 moles of CH4 undergoes chlorination with excess of chlorine: CH4 + 4Cl2 → CCl4 + 4HCl A 2 moles B 5 moles C 8 moles D 10 moles QUESTION 2.76 g of silver carbonate on being strongly heated yields a residue weighing: Ag2CO3 → 2 Ag + CO2 + ½ O2 A 2.16 g B 2.48 g C 2.32 g D 2.64 g QUESTION The volume of gas at NTP produced by 100 gm of CaC2 with water: CaC2 + 2H2O → Ca(OH)2 + C2H2 A 70 litre B 35 litre C 17.5 litre D 22.4 litre QUESTION In the following reaction, if 64 g of O2, react with SO2. What will be volume of SO3 at STP. 2SO2 + O2 → 2SO3 A 5.6 L B 22.4 L C 89.6 L D 112.5 L QUESTION Write a balanced equation for the combustion of propane, C3H8. When balanced, the equation indicates that ___ moles of O2 are required for each mole of C3H8. A 1.5 B 3 C 35 D 5 QUESTION How many grams of calcium oxide is obtained on heating 100 g of CaCO3(s)? A 50 g B 40 g C 56 g D 44 g QUESTION What is the mass of glucose required to produce 44 g of CO2 on complete combustion? A 30 g B 45 g C 60 g D 22 g QUESTION The volume of O2 at STP required for the complete combustion of 4g CH4 is A 5.6 litre B 2.88 litre C 22.4 litre D 11.2 litre QUESTION What is the weight of oxygen required for the complete combustion of 2.8 kg of ethylene? A 2.8 kg B 6.4 kg C 9.6 kg D 96 kg QUESTION How many grams of H2 are required to consume 2 mol of CO? CO(g) + 2H2(g) → CH3OH(g) A 2g B 4g C 8g D 16 g QUESTION When a certain amount of octane, C8H18, is burnt completely, 7.04 g CO2 is formed. What is the mass of H2O formed simultaneously? A 1.62 g B 6.48 g C 3.24 g D 2.28 g QUESTION What volume at STP of CO is required to reduce one mole of Fe2O3 in the following reaction Fe2O3 + CO → Fe + CO2 A 11200 cm3 B 22400 cm3 C 67200 cm3 D 33600 cm3 QUESTION Calculate the mass of hydrogen formed when 27 g of aluminum reacts with excess hydrochloric acid according to the balanced equation below. 2Al + 6HCl → 2AlCl3 + 3H2 A 1.5 g B 2.0 g C 3.0 g D 6.0 g QUESTION How many grams of SO3 are produced from 1 mol of S8? A 1280.0 B 640.0 C 960.0 D 320.0 QUESTION If 1/2 moles of oxygen combine with aluminium to form Al2O3 then weight of Aluminium metal used in the reaction is (Al = 27) A 27 g B 18 g C 54 g D 40.5 g QUESTION Which of the following statement is correct? A 28g CO contains 12 g carbon and 16 g oxygen B One mole of CO reacts completely with half mole of O2 to form CO2 C N2 and CO have same molar mass D All of these QUESTION 0.9 g Al reacts with dil. HCl to give H2. The volume of H2 evolved at STP is (Atomic weight of Al = 27) A 1.12 litre B 2.24 litre C 3.33 litre D 4.44 litre QUESTION The number of moles of oxygen obtained by the electrolytic decomposition of 90 g water is elec. (2H2O 2H2 + O2) A 2.5 B 5 C 7.5 D 10 QUESTION Butane, C4H10, burns with the oxygen in air to give carbon dioxide and water. What is the amount (in moles) of carbon dioxide produced from 0.15 mol C4H10? C4H10(g) + O2(g) → CO2(g) + H2O(g) A 0.15 mol CO2 B 0.30 mol CO2 C 0.45 mol CO2 D 0.60 mol CO2 QUESTION The right option for the mass of CO2 produced by heating 20 g of 20% pure limestone is (Atomic mass of Ca = 40) 𝟏𝟐𝟎𝟎 𝐊 𝐂𝐚𝐂𝐎𝟑 𝐂𝐚𝐎 + 𝐂𝐎𝟐 A 1.76 g B 2.64 g C 1.32 g D 1.12 g QUESTION A sample of calcium carbonate is 80% pure. 25g of this sample is treated with excess of HCl. How much volume of CO2 will be obtained at NTP. A 4.48 litre B 5.6 litre C 11.2 litre D 2.24 litre QUESTION 20.0 g of a magnesium carbonate sample decompose on heating to give carbon dioxide and 8.0 g magnesium oxide. What be the percentage purity of magnesium carbonate in the sample? A 60 B 84 C 75 D 96 QUESTION 10g of MnO2 on reaction with HCl forms 2.24 L of Cl2(g) at NTP, the percentage impurity of MnO2 is MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O A 87% B 25% C 33.3% D 13% QUESTION If 300 g of CaCO3 on reaction with excess of H2SO4 gives 272 g of CaSO4. Find the % age yield of product? A 66.66% B 33.33% C 50% D 25% QUESTION Limiting reagent in a chemical reaction is that reactant which A Left some amount unreacted after the completion of reaction B Reacts completely in the reaction C Does not react in the reaction D All of these QUESTION When 5 mole N2 react with 10 mole H2 in Haber’s process, the mole of NH3 formed will be A 10 mole B 10/3 mole C 20/3 mole D 5 mole QUESTION When 22.4 L H2(g) is mixed with 11.2 L Cl2(g) at STP the moles of HCl formed are equal to A 1 mole of HCl (g) B 2 mole of HCl (g) C 0.5 mole of HCl (g) D 1.5 mole of HCl (g) QUESTION 1.0 g magnesium is burnt with 0.56 g O2 in a closed vessel. Which reactant is left in excess and how much? (At. wt. Mg = 24, O = 16) A Mg, 0.16 g B O2, 0.16 g C Mg, 0.44 g D O2, 0.28 g QUESTION The mass of Mg3N2 produced if 48 gm of Mg metal is reacted with 34 gm NH3 gas is Mg + NH3 ⎯→ Mg3N2 + H2 200 A gm 3 100 B gm 3 400 C gm 3 150 D gm 3 QUESTION How many grams of nitric acid, HNO3, can be prepared from the reaction of 138 g of NO2 with 54.0 g H2O according to the equation below? 3NO2 + H2O → 2HNO3 + NO A 126 gm B 105 gm C 136 cm D 120 gm QUESTION 𝟏 12 moles of each A & B are allowed to react as given: 3A + 2B → C + D. If 60g 𝟐 of D is produced then calculate the atomic mass of D. A 30 B 45 C 60 D 15 QUESTION 4 g of hydrogen is ignited with 4 g of oxygen, the amount of water formed is? A 2.5 g B 0.5 g C 4.5 g D 8g QUESTION Calculate ate the weight of FeO produced from 6.7 g VO & 4.8 g Fe2O3 VO + Fe2O3 → FeO + V2O5 (At. wt. of V = 51, At. wt. of Fe = 56) A 4.32 B 7.755 C 2.585 D 0.0718 QUESTION 8 g H2 and 32 g O2 is allowed to react to form water then which of the following statement is correct? A O2 is limiting reagent B O2 is reagent in excess C H2 is limiting reagent D 40 g water is formed QUESTION Equal volume of N2 and H2 react to form ammonia under suitable condition then the limiting reagent is A H2 B NH3 C N2 D No one reactant is limiting reagent QUESTION 0.5 mole of H2SO4 is mixed with 0.2 mole of Ca(OH)2. The maximum number of moles of CaSO4 formed is A 0.2 B 0.5 C 0.4 D 1.5 QUESTION For the reaction: 7A + 13B + 15C → 17P If 15 moles of A, 26 moles of B & 30.5 moles of C are taken initially then limiting reactant is A A B B C C D None of these QUESTION 10g H2 reacts with 64g of O2 determine number of moles of gaseous product formed. A 1 mole B 4 mole C 3 mole D 5 mole QUESTION Solder is an alloy of tin and lead that is used in electronic circuits. It has melting point of 225°C. It is............. °F. A 498 °F B –437 °F C 437 °F D 400 °F QUESTION At what temperature will a Fahrenheit thermometer give a reading that is twice on the Celsius thermometer? A 53.3° B –123° C 30.0° D 160.0° QUESTION 10g H2 reacts with 64g of O2 determine number of moles of gaseous product formed. A 1 mole B 4 mole C 3 mole D 5 mole QUESTION According to the equation, N2O3(g) + 6H2(g) → 2NH3(g) + 3H2O(g) how many moles of NH3(g) could be formed from the reaction of 0.22 mol of N2O3 (g) with 0.87 mol of H2(g)? A 0.29 mol B 0.44 mol C 0.73 mol D 1.1 mol QUESTION The number of moles of C and D produced on mixing 5 moles of A and 7 moles of B are respectively: (3A + 5B → 7C + 9D) A 9 moles and 11 moles B 11.66 moles and 15 moles C 9.8 moles and 12.6 moles D 1 moles and 13 moles QUESTION How many moles of lead (II) chloride will be formed from a reaction between 6.5 g of PbO and 3.2 g of HCl? A 0.029 B 0.044 C 0.333 D 0.011 QUESTION 4g CaCO3 on reacting with excess HCl produces 0.88 g CO2 according to reaction: CaCO3 + 2HCl → CaCl2 + CO2 + H2O The percentage purity of CaCO3: A 50 % B 60 % C 70 % D 80 % QUESTION Match the following prefixes with their multiples: Prefixes Multiples (i) micro 106 (ii) deca 109 (iii) mega 10–6 (iv) giga 10–15 (v) femto 10 QUESTION Count the significant digits. 0.01346 = 0.0103046 = 13.0460 = 13.0046 = 0.0001346 = 1346.000 = QUESTION The density of the solution is 2.15 g mL–1, then mass of 2.5 mL solution in correct significant figures is A 5375 × 10–3 g B 5.4 g C 5.38 g D 53.75 g QUESTION An average adult has 5.2 L of blood. Volume of blood in m3 is A 5.2 × 103 m3 B 5.2 × 10–3 m3 C 5.2 × 10–6 m3 D 5.2 × 10–2 m3