Grab a calculator and a copy of the periodic table

(This test has only 10 questions, but may take 15 - 20 mins).
1. In an experiment to investigate the rate of decomposition of hydrogen peroxide a student collected 240 cm3 of oxygen gas at rtp. How many moles of oxygen gas did he collect?

[Molar volume of any gas at rtp = 24,000 cm3]

  • A.   100
  • B.   10
  • C.   0.010
  • D.   0.1

Q2-3:
Industrially nitrogen gas reacts with hydrogen gas in the Haber process to produce 340 kg of ammonia gas.

N2(g)  +  3H2(g) → 2NH3(g)

  
2. How many moles of ammonia formed? [Mr of NH3 = 17]
  • A.   10
  • B.   20
  • C.   10,000
  • D.   20,000
3. What volume of nitrogen gas was needed to produce this amount of ammonia at rtp?

[Molar volume of any gas =24 dm3 at rtp]

  • A.   240 dm3
  • B.   240,000 dm3
  • C.   480 dm3
  • D.   480,000 dm3

Q4-5:
200 cm3 of a 2.0 mol/dm3 solution of potassium hydroxide was used to absorb carbon dioxide gas in the following reaction:

2KOH(aq)  +  CO2(g) → K2CO3(aq)  +  H2O(l)

4. How many moles of potassium hydroxide were used and what amount, in moles, of carbon dioxide could be absorbed by this solution?

  Moles of KOH used Moles of CO2 absorbed
A 0.4 0.4
B 0.4 0.2
C 400 400
D 400 200
5. What volume of carbon dioxide could be absorbed by this solution at room temperature and pressure?
[molar volume of any gas = 24 dm3 at rtp]
  • A.   4.8 cm3
  • B.   480 cm3
  • C.   4.8 dm3
  • D.   4800 dm3

Q6-7:
A student used a titration method to find the concentration of a solution of oxalic acid, H2C2O4. The equation for the reaction is:

2NaOH(aq) + H2C2O4(aq) → Na2C2O4(aq) + 2H2O(l)

She obtained the following results:

Volume of sodium hydroxide solution in conical flask 25.0 cm3
Concentration of sodium hydroxide solution 0.120 mol/dm3
Average volume of oxalic acid solution added 18.30 cm3
6. Calculate the amount, in moles, of sodium hydroxide used.
  • A.   3.00
  • B.   0.00300
  • C.   2.20
  • D.   0.00220
7. Calculate the concentration, in mol/dm3, of the oxalic acid.
  • A.   0.328
  • B.   0.164
  • C.   0.0820
  • D.   0.0440

Q8-9:
The salt copper(II)chloride was prepared by adding excess copper(II)carbonate to 0.100 mol of dilute hydrochloric acid.  The equation for the reaction is:

CuCO3(s) + 2HCl(aq) → CuCl2(aq) + H2O(l) + CO2(g)
8. Calculate the mass of copper(II)carbonate that will react with the 0.100 mol of hydrochloric acid.
[Mr of CuCO3 = 123.5]
  • A.   24.70 g
  • B.   18.53 g
  • C.   12.35 g
  • D.   6.18 g
9. Calculate the volume of carbon dioxide gas that will be formed in this reaction at room temperature and pressure.
[Molar volume of any gas = 24 dm3]
  • A.   0.6 dm3
  • B.   1.2 dm3
  • C.   2.4 dm3
  • D.   4.8 dm3
10. A student requires 0.032g of methane gas, CH4. What volume of gas, in cm3, should she collect at room temperature and pressure (rtp)?

[Mr of CH4 = 16; Molar volume of gas at rtp = 24dm3]

  • A.   0.048cm3
  • B.   32cm3
  • C.   48cm3
  • D.   768cm3