General Chemistry 1 Practice Questions (Set 4)

1) How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen.

6 Li(s) + N2(g) → 2 Li3N(s)

  • A) 18.3 g Li3N
  • B) 20.3 g Li3N
  • C) 58.3 g Li3N
  • D) 61.0 g Li3N
  • E) 15.1 g Li3N

2) How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol.

4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

  • A) 0.290 mol O2
  • B) 0.580 mol O2
  • C) 18.5 mol O2
  • D) 0.724 mol O2
  • E) 1.73 mol O2

3) How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol.

4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

  • A) 0.290 mol N2
  • B) 0.580 mol N2
  • C) 18.5 mol N2
  • D) 0.724 mol N2
  • E) 1.73 mol N2

4) Two samples of calcium fluoride are decomposed into their constituent elements. The first sample produced 0.154 g of calcium and 0.146 g of fluorine. If the second sample produced 294 mg of fluorine, how many g of calcium were formed?

  • A) 0.280 g
  • B) 3.09 × 102 g
  • C) 3.13 g
  • D) 0.309 g
  • E) 2.80 × 102 g

5) Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kg of iodine were produced?

  • A) 13.3 kg
  • B) 22.5 kg
  • C) 79.4 kg
  • D) 44.4 kg
  • E) 92.4 kg

6) A 14.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3). If ammonia is the only product, what mass of ammonia is formed?

  • A) 17.01 g
  • B) 1.10 g
  • C) 14.01 g
  • D) 3.02 g
  • E) 23.07 g

7) Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol.

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

  • A) 38.0 g H2O
  • B) 21.7 g H2O
  • C) 43.4 g H2O
  • D) 10.9 g H2O
  • E) 26.5 g H2O

8) Consider the following balanced reaction. What mass (in g) of CO2 can be formed from 288 mg of O2? Assume that there is excess C3H7SH present.

C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)

  • A) 0.396 g CO2
  • B) 0.209 g CO2
  • C) 0.792 g CO2
  • D) 0.126 g CO2
  • E) 0.198 g CO2

9) According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed?

2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(l)

  • A) 99.8 g S
  • B) 66.6 g S
  • C) 56.1 g S
  • D) 44.4 g S
  • E) 14.0 g S

10) A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl3). If it is the only product, what mass of PCl3 is formed?

  • A) 30.15 g
  • B) 54.93 g
  • C) 140.01 g
  • D) 79.71 g
  • E) 91.86 g

11) Determine the molarity of a solution formed by dissolving 3.00 moles of NaCl in enough water to yield 4.00 L of solution.

  • A) 1.33 M
  • B) 2.00 M
  • C) 0.750 M
  • D) 3.00 M
  • E) 12.00 M

12) Determine the molarity of a solution formed by dissolving 4.00 moles of KBr in enough water to yield 3.00 L of solution.

  • A) 1.33 M
  • B) 2.00 M
  • C) 0.750 M
  • D) 3.00 M
  • E) 12.00 M

13) Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

  • A) 1.50 M
  • B) 1.18 M
  • C) 0.130 M
  • D) 0.768 M
  • E) 2.30 M

14) Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution.

  • A) 0.0297 M
  • B) 0.0337 M
  • C) 0.0936 M
  • D) 0.0107 M
  • E) 0.0651 M

15) A solution is prepared by adding 1.70 g of solid NaCl to 50.0 mL of 0.100 M CaCl2. What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

  • A) 0.782
  • B) 0.682
  • C) 0.134
  • D) 0.234
  • E) 0.582

16) What is the molarity of a NaOH solution if 28.2 mL of a 0.112 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?

  • A) 0.253
  • B) 0.0993
  • C) 0.199
  • D) 39.5
  • E) 0.126

17) How many milliliters of 0.111 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

  • A) 0.438
  • B) 0.0142
  • C) 70.3
  • D) 0.0281
  • E) 35.5

18) Which of the following is an acid-base reaction?

  • A) C(s) + O2(g) → CO2(g)
  • B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq)
  • C) Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq)
  • D) MgSO4(aq) + Pb(NO3)2(aq) → Mg(NO3)2(aq) + PbSO4(s)
  • E) None of the above is an acid-base reaction.

19) Which of the following is a gas-evolution reaction?

  • A) 2 C2H6(l) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)
  • B) 2 H2(g) + O2(g) → 2 H2O(g)
  • C) KCl(aq) + NaNO3(aq) → KNO3(aq) + NaCl(s)
  • D) NH4Br(aq) + KOH(aq) → KBr(aq) + NH3(g) + H2O(l)
  • E) None of the above is a gas-evolution reaction.

20) Identify acetic acid.

  • A) strong electrolyte, weak acid
  • B) weak electrolyte, weak acid
  • C) strong electrolyte, strong acid
  • D) weak electrolyte, strong acid
  • E) nonelectrolyte

General Chemistry 1 Practice Questions (Set 4)

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