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When 468 mg of $MgI_2$ is dissolved in enough water to create 50.0 mL of solution, what is the molarity?
When 468 mg of $MgI_2$ is dissolved in enough water to create 50.0 mL of solution, what is the molarity?
- 0.0107 M
- 0.0936 M
- 0.0297 M
- 0.0337 M (correct)
If 25.0 mL of a 0.188 M $Mg(NO_3)_2$ stock solution is diluted to 150.0 mL, what is the resulting concentration?
If 25.0 mL of a 0.188 M $Mg(NO_3)_2$ stock solution is diluted to 150.0 mL, what is the resulting concentration?
- 1.13 M
- 0.0887 M
- 0.0199 M
- 0.0313 M (correct)
According to the reaction $FeCl_2(aq) + 2 LiOH(aq) \rightarrow Fe(OH)_2(s) + 2 LiCl(aq)$, how many moles of $Fe(OH)_2$ can be formed from 175.0 mL of 0.227 M $LiOH$ solution, assuming excess $FeCl_2$?
According to the reaction $FeCl_2(aq) + 2 LiOH(aq) \rightarrow Fe(OH)_2(s) + 2 LiCl(aq)$, how many moles of $Fe(OH)_2$ can be formed from 175.0 mL of 0.227 M $LiOH$ solution, assuming excess $FeCl_2$?
- $3.97 \times 10^{-2}$ moles
- $1.99 \times 10^{-2}$ moles (correct)
- $5.03 \times 10^{-2}$ moles
- $2.52 \times 10^{-2}$ moles
What volume of 0.305 M $AgNO_3$ is required to react completely with 155.0 mL of 0.274 M $Na_2SO_4$ solution in the following reaction? $2AgNO_3(aq) + Na_2SO_4(aq) \rightarrow NaNO_3(aq) + Ag_2SO_4(s)$
What volume of 0.305 M $AgNO_3$ is required to react completely with 155.0 mL of 0.274 M $Na_2SO_4$ solution in the following reaction? $2AgNO_3(aq) + Na_2SO_4(aq) \rightarrow NaNO_3(aq) + Ag_2SO_4(s)$
What mass (in g) of $AgCl$ is formed from the reaction of 75.0 mL of a 0.078 M $AgC_2H_3O_2$ solution with 55.0 mL of 0.109 M $MgCl_2$ solution? $2 AgC_2H_3O_2(aq) + MgCl_2(aq) \rightarrow 2 AgCl(s) + Mg(C_2H_3O_2)_2(aq)$
What mass (in g) of $AgCl$ is formed from the reaction of 75.0 mL of a 0.078 M $AgC_2H_3O_2$ solution with 55.0 mL of 0.109 M $MgCl_2$ solution? $2 AgC_2H_3O_2(aq) + MgCl_2(aq) \rightarrow 2 AgCl(s) + Mg(C_2H_3O_2)_2(aq)$
The pressure exerted on a fixed amount of gas is tripled at constant temperature, and then the temperature of the gas in kelvins is tripled at constant pressure. By what factor does the final volume change compared to the initial volume?
The pressure exerted on a fixed amount of gas is tripled at constant temperature, and then the temperature of the gas in kelvins is tripled at constant pressure. By what factor does the final volume change compared to the initial volume?
The pressure of 12.8 g of hydrogen gas is doubled at constant volume, and then the volume is doubled at constant pressure. What is the final temperature relative to the initial temperature?
The pressure of 12.8 g of hydrogen gas is doubled at constant volume, and then the volume is doubled at constant pressure. What is the final temperature relative to the initial temperature?
An unknown gas has a mass of 1.56 g. Its volume is 0.50 L at a temperature of 315 K and a pressure of 1.14 atm. Which gas is it?
An unknown gas has a mass of 1.56 g. Its volume is 0.50 L at a temperature of 315 K and a pressure of 1.14 atm. Which gas is it?
Water can be generated from the following equation: $4 NH_3 (g) + 5 CO_2 (g) \rightarrow 4 NO (g) + 6 H_2O (g)$. How much $H_2O$(g) is produced if 9.0 g of $NH_3$(g) reacts with 13.4 g of $H_2O$(g) at STP?
Water can be generated from the following equation: $4 NH_3 (g) + 5 CO_2 (g) \rightarrow 4 NO (g) + 6 H_2O (g)$. How much $H_2O$(g) is produced if 9.0 g of $NH_3$(g) reacts with 13.4 g of $H_2O$(g) at STP?
A balloon contains 0.76 mol $H_2$, 0.18 mol Ne, 0.031 mol Rn and 0.026 mol $Cl_2$ at 739 mm Hg. What is the partial pressure of Ne?
A balloon contains 0.76 mol $H_2$, 0.18 mol Ne, 0.031 mol Rn and 0.026 mol $Cl_2$ at 739 mm Hg. What is the partial pressure of Ne?
This graph shows the distribution of molecular velocities for two different molecules (A and B) at the same temperature. Which of the following statements is true?
This graph shows the distribution of molecular velocities for two different molecules (A and B) at the same temperature. Which of the following statements is true?
A system releases 742 kJ of heat and does 143 kJ of work on the surroundings. What is the change in internal energy of the system?
A system releases 742 kJ of heat and does 143 kJ of work on the surroundings. What is the change in internal energy of the system?
A 21.8 g sample of ethanol ($C_2H_5OH$) is burned in a bomb calorimeter. If the temperature rises from 25.0 to 62.3°C, determine the heat capacity of the calorimeter, in $kJ/^{\circ}C$. The molar mass of ethanol is 46.07 g/mol. $C_2H_5OH(l) + 3 O_2(g) \rightarrow 2 CO_2(g) + 3 H_2O(g)$ $\Delta H_{rxn} = -1235 kJ$
A 21.8 g sample of ethanol ($C_2H_5OH$) is burned in a bomb calorimeter. If the temperature rises from 25.0 to 62.3°C, determine the heat capacity of the calorimeter, in $kJ/^{\circ}C$. The molar mass of ethanol is 46.07 g/mol. $C_2H_5OH(l) + 3 O_2(g) \rightarrow 2 CO_2(g) + 3 H_2O(g)$ $\Delta H_{rxn} = -1235 kJ$
According to the following thermochemical equation, what mass of HF (in g) must react in order to produce 690 kJ of energy? Assume excess $SiO_2$. $SiO_2(s) + 4 HF(g) \rightarrow SiF_4(g) + 2 H_2O(l)$ $\Delta H_{rxn} = -184 kJ$
According to the following thermochemical equation, what mass of HF (in g) must react in order to produce 690 kJ of energy? Assume excess $SiO_2$. $SiO_2(s) + 4 HF(g) \rightarrow SiF_4(g) + 2 H_2O(l)$ $\Delta H_{rxn} = -184 kJ$
How much energy is evolved during the reaction of 55.2 g of Al, according to the reaction below? Assume that there is excess $Fe_2O_3$. $Fe_2O_3(s) + 2 Al(s) \rightarrow Al_2O_3(s) + 2 Fe(s)$ $\Delta H_{rxn} = -852 kJ$
How much energy is evolved during the reaction of 55.2 g of Al, according to the reaction below? Assume that there is excess $Fe_2O_3$. $Fe_2O_3(s) + 2 Al(s) \rightarrow Al_2O_3(s) + 2 Fe(s)$ $\Delta H_{rxn} = -852 kJ$
Flashcards
What is Molarity?
What is Molarity?
Molarity is defined as the number of moles of solute per liter of solution.
What is a net ionic equation?
What is a net ionic equation?
The net ionic equation shows only the chemical species that participate in a reaction, excluding spectator ions.
What is a strong electrolyte?
What is a strong electrolyte?
A strong electrolyte is a substance that completely dissociates into ions when dissolved in water.
What is oxidation state?
What is oxidation state?
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What is a balanced molecular equation?
What is a balanced molecular equation?
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What is heat of reaction (ΔHrxn)?
What is heat of reaction (ΔHrxn)?
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What is an endothermic reaction?
What is an endothermic reaction?
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What are standard reaction enthalpies used for?
What are standard reaction enthalpies used for?
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What is wavelength?
What is wavelength?
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What is frequency?
What is frequency?
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What is the principal quantum number (n)?
What is the principal quantum number (n)?
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What is the angular momentum quantum number (l)?
What is the angular momentum quantum number (l)?
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What is the magnetic quantum number (ml)?
What is the magnetic quantum number (ml)?
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What is the spin quantum number (ms)?
What is the spin quantum number (ms)?
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Study Notes
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- 00 moles of NaCl dissolved in enough water to yield 4.00 L of solution results in a 0.750 M solution.
- Dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution results in a 0.0337 M solution.
- There are 5.02 g of solute in 500.0 mL of 0.179 M KOH.
- The concentration of FeCl3 is 0.785 M in a solution prepared by dissolving 35.0 g of FeCl3 in enough water to make 275 mL of solution.
- To make 250. mL of a 0.145 M AgNO3 solution, 6.16 g of AgNO3 are needed.
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- 0 mL of 0.0887 M MgCl2 solution is needed to make 275.0 mL of 0.0600 M MgCl2 solution.
- Diluting 25.0 mL of a stock 0.188 M Mg(NO3)2 solution to 150.0 mL yields a concentration of 0.0313 M.
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- 99 × 10-2 moles of Fe(OH)2 can form from 175.0 mL of 0.227 M LiOH solution, assuming excess FeCl2 with the equation: FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq).
- 278 mL of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution in the reaction AgNO3(aq)+Na2SO4(aq)→NaNO3(aq)+Ag₂SO₄(s).
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- 838 g of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl2 solution, according to the equation: 2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq).
- Ammonia is a weak electrolyte and a weak base.
- MgCO3 is not a strong electrolyte.
- Hydrofluoric acid is a weak electrolyte and a weak acid.
- Sulfuric acid is a strong electrolyte and a strong acid.
- The net ionic equation for the reaction between aqueous solutions of K2S and Fe(NO3)2 is Fe2+(aq) + S2-(aq) → FeS(s).
- The net ionic equation for the reaction between aqueous solutions of H2SO4 and KOH is H+(aq) + OH-(aq) → H2O(l).
- There is no net ionic equation for the reaction between aqueous solutions of Al(C2H3O2)3 and LiNO3.
- The balanced molecular equation for the reaction between nitric acid and calcium hydroxide is 2 HNO3 (aq) + Ca)OH)2 (aq) → 2 H2O (l) + Ca(NO3)2 (aq).
- The balanced molecular equation for the reaction between acetic acid and barium hydroxide is 2 HC2H3O2 (aq) + Ba(OH)2 (aq) → 2 H2O (l) + Ba(C2H3O2)2 (aq).
- The oxidation state of C in CO32- is +4.
- The oxidation state of sulfur in SO2 is +4.
- When the pressure exerted on a fixed amount of gas is tripled at constant temperature, and then the temperature of the gas in kelvins is tripled at constant pressure, the final volume of the gas is the same as the initial volume.
- When the pressure of 12.8 g of hydrogen gas is doubled at constant volume, and then the volume is doubled at constant pressure, the final temperature of the gas is four times the initial temperature.
- An unknown gas with a mass of 1.56 g, a volume of 0.50 L at 315 K, and a pressure of 1.14 atm is Cl2.
- A 0. 435-g sample of an unknown pure gas occupying 0.333 L at 1.00 atm and 100.0°C is argon.
- The amount of argon gas in a 450 mL container at 2131.1 mmHg and 83°F is 2.04 g.
- In order of increasing density at STP: NH3 < Ne < Kr < N2O4.
- In order of decreasing density at STP: Br2 > HCl > O2 > H2O > H2.
- With 9.0 g of NH3 (g) reacting with 13.4 g of H2O (g) at STP, 6.31 g of H2O (g) is produced, following the following equation: 4 NH3 (g) + 5 CO2 (g) → 4 NO (g) + 6 H2O (g).
- Generating hydrogen gas involves reacting 9.25 grams of barium hydride with water at 20°C and 755 mm Hg pressure produces 3.21 L of hydrogen gas: BaH2(s) + 2 H2O(l) → Ba(OH)2(aq) + 2 H2(g).
- A balloon contains 0.76 mol H2, 0.18 mol Ne, 0.031 mol Rn, and 0.026 mol Cl2 at 739 mm Hg, the partial pressure of Ne is 130 mm Hg.
- Gas A has the higher molar mass, according to the distribution of molecular velocities for two different molecules (A and B) at the same temperature.
- Gas D has the largest molar mass, according to the graph.
- If ∆Esys = 423 J, the system is gaining 423 J, while the surroundings are losing 423 J.
- If a system releases 742 kJ of heat and does 143 kJ of work on the surroundings, the change in internal energy of the system is -885 kJ.
- The air in an inflated balloon (defined as the system) warms over a toaster and absorbs 185 J of heat, and as it expands, it does 82 kJ of work, the change in internal energy for the system is -82 kJ.
- When a 21.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, and the temperature rises from 25.0 to 62.3°C, the heat capacity of the calorimeter is 15.7 kJ/°C.
- When a 12. 8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ/°C and the initial temperature is 25.0°C, the final temperature of the calorimeter is 85.7°C.
- An endothermic reaction has a positive ΔH, absorbs heat from the surroundings, and feels cold to the touch.
- An endothermic reaction does not give off heat to the surroundings.
- For SiO2(s) + 4 HF(g) → SiF4(g) + 2 H2O(l) with ΔH°rxn = -184 kJ, 300. g of HF must react to produce 690 kJ of energy.
- 872 kJ of energy is evolved during the reaction of 55.2 g of Al, according to the reaction Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) with ΔH°rxn = -852 kJ.
- The reaction that illustrates ∆H°f for Mg(NO2)2 is Mg(s) + N2(g) + 2 O2(g) → Mg(NO2)2(s).
- The reaction that illustrates ∆H°f for LiHSO4 is Li(s) + 1/2 H2(g) + S(s) + 2 O2(g) → LiHSO4(s).
- For 4 NO(g) + 2 O2(g) → 4 NO2(g), the enthalpy is -234 kJ.
- For 4 S(s) + 6 O2(g) → 4 SO3(g), the enthalpy is -1583 kJ.
- For SO2Cl2(g) + 2 H2O(l) → 2 HCl(g) + H2SO4(l), the enthalpy is -62 kJ.
- The enthalpy for IF is -63.8 kJ/mol.
- Increasing wavelength order: gamma rays < ultraviolet light < radio waves.
- Decreasing energy order: x-rays > infrared light > radio waves.
- The frequency of the red light emitted by a neon sign with a wavelength of 710 nm is 4.26 × 1014 s-1.
- The energy of a photon of UV-B electromagnetic radiation at 280 nm is 7.1 × 10-19 J.
- The statement that best describes atoms is that atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape.
- The spin quantum number (ms) describes the orientation of the spin of the electron.
- The transition (in a hydrogen atom) representing the absorption of the shortest wavelength photon is n = 1 to n = 2.
- The transition (in a hydrogen atom) representing the absorption of the smallest frequency photon is n = 5 to n = 6.
- For n = 4, the possible orbitals are s, p, d, f.
- The value of l represented by a d orbital is 2.
- The value of l represented by a s orbital is 0.
- In the second principal level, there are 2 different values of l.
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