Grade 10 Chemistry Second Term Plan 2024/2025

<p>Matter can be converted from one form to another in chemical reactions. (D)</p> Signup and view all the answers

<p>The elements are combined in a fixed ratio by mass, regardless of the source. (C)</p> Signup and view all the answers

<p>87.75 grams (B)</p> Signup and view all the answers

<p>20% (B)</p> Signup and view all the answers

<p>2 moles (C)</p> Signup and view all the answers

<p>Volume of an ideal gas at a given temperature (A)</p> Signup and view all the answers

<p>PA = (nA / total gas moles) × PT (C)</p> Signup and view all the answers

<p>XA = nA / (nA + nB) (B)</p> Signup and view all the answers

<p>Calculating each gas's pressure based on its mass (D)</p> Signup and view all the answers

<p>4 g of H2 will yield more moles than 4 g of O2. (C)</p> Signup and view all the answers

<p>Covalent bond (A)</p> Signup and view all the answers

<p>CO2 (A)</p> Signup and view all the answers

<p>Low melting and boiling points (A)</p> Signup and view all the answers

<p>It involves one atom donating a lone pair of electrons. (C)</p> Signup and view all the answers

<p>Van der Waals forces (B)</p> Signup and view all the answers

<p>Benzene (D)</p> Signup and view all the answers

<p>NH4+ (B)</p> Signup and view all the answers

<p>They are weaker than hydrogen bonds. (D)</p> Signup and view all the answers

<p>Heating copper in oxygen (D)</p> Signup and view all the answers

<p>12.5:1 (A)</p> Signup and view all the answers

<p>It confirms that a specific compound has a fixed ratio of its elements. (B)</p> Signup and view all the answers

<p>Volume is inversely proportional to pressure. (D)</p> Signup and view all the answers

<p>2.00 g (A)</p> Signup and view all the answers

<p>Calculating ratios and verifying they are constant in different samples. (C)</p> Signup and view all the answers

<p>180 mm Hg (A)</p> Signup and view all the answers

<p>Volume is directly proportional to temperature. (B)</p> Signup and view all the answers

<p>25:2 (B)</p> Signup and view all the answers

<p>The ratios of masses of elements in different compounds are consistent and form a ratio of whole numbers. (B)</p> Signup and view all the answers

<p>180 K (B)</p> Signup and view all the answers

<p>It oxidizes copper to form copper (II) oxide. (C)</p> Signup and view all the answers

<p>P1V1 = P2V2 (D)</p> Signup and view all the answers

<p>9.00 dm3 (B)</p> Signup and view all the answers

<p>Both A and B (D)</p> Signup and view all the answers

<p>Gas laws only apply to ideal gases. (B)</p> Signup and view all the answers

<p>$PV = nRT$, where $P$ is pressure, $V$ is volume, $n$ is moles, $R$ is the gas constant, $T$ is temperature. (B)</p> Signup and view all the answers

<p>The pressures exerted by gases are equal to the sum of their individual partial pressures. (D)</p> Signup and view all the answers

<p>$XA = \frac{nA}{nA + nB + nC}$ (D)</p> Signup and view all the answers

<p>The mole fractions can be calculated using the number of moles of each gas. (B)</p> Signup and view all the answers

<p>atm (A)</p> Signup and view all the answers

PV = nRT; relates pressure, volume, and temperature of gas.

States total pressure is the sum of individual gas pressures in a mixture.

XA = nA / (nA + nB + nC); ratio of moles of a component to total moles.

In a gas at constant temperature, pressure decreases as volume increases.

R = 0.0821 atm dm3 mol-1 K-1; constant in the ideal gas equation.

The total pressure equals the sum of the partial pressures of individual gases in a mixture.

The ratio of moles of a specific gas to the total moles of all gases in a mixture.

The force exerted by gas molecules per unit area, measured in atmospheres (atm).

A constant (0.0821 atm dm3 mol-1 K-1) used in the ideal gas equation.

The mole is a unit that measures the amount of substance.

The mass of one mole of a substance in grams per mole (g/mol).

The quantity of matter in an object, measured in grams (g).

Number of moles (n) equals mass (m) divided by molar mass (M).

Matter is neither created nor destroyed in chemical reactions.

Compounds always contain the same elements in the same proportions by mass.

When two elements form more than one compound, the masses combine in simple whole-number ratios.

88 g of CO2 contains 2 moles of carbon (C) based on its molar mass.

Compounds in solution that conduct electricity.

A bond formed by the sharing of electrons between two non-metals.

A covalent compound formed by hydrogen and sulfur sharing electrons.

Low melting/boiling points, non-electrolytes, insoluble in water.

A bond formed when one atom donates a lone pair of electrons for sharing.

An example of a molecule with a dative covalent bond.

Weak forces of attraction in gaseous molecules, leading to liquid formation.

Weak attraction between polar molecules, like in water.

Methods to prepare copper (II) oxide include heating copper with oxygen or via reactions with trioxonitrate (V) acid.

In the decomposition of mercuric oxide, the mass ratio of mercury to oxygen remains constant at 25:2.

In Experiment 1, 2.16 g of mercuric oxide decomposed to yield 2.00 g mercury and 0.16 g oxygen.

In Experiment 2, 17.28 g of mercuric oxide gave 16 g mercury and 1.28 g oxygen.

Obtaining copper (II) hydroxide by dissolving copper in trioxonitrate (V) acid followed by strong heating.

Laws that govern how elements combine to form compounds, including the law of multiple proportions.

An instructional approach using hands-on experiments and drawings of apparatus to teach chemistry.

Volume of gas is inversely proportional to pressure at constant temperature.

PV = K, where K is a constant of proportionality.

Initial and final states of pressure and volume in Boyle's law.

Volume of gas is directly proportional to absolute temperature at constant pressure.

V/T = k, showing volume related to temperature.

Combines Boyle’s and Charles’ laws: P1V1/T1 = P2V2/T2.

Temperature of 273 K and pressure of 760 mm Hg.

Use P1V1/T1 = P2V2 to find final volume under standard conditions.