You're viewing 1 free preview question for Chemistry HL — subscribe to unlock 224 more, plus the Full Question Bank, Mock Papers & Worksheets.Upgrade

How Much? The Amount of Chemical Change · Paper 2 — Free Chemistry HL Practice Questions

1MasterySAQ-SStoichiometry and mole-to-mole ratios5 marksPaper 2~8 min
In the Haber process, nitrogen and hydrogen react according to: N2(g)+3H2(g)→2NH3(g)ΔH=−92 kJ mol−1\text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \quad \Delta H = -92\,\text{kJ mol}^{-1} A reactor is charged with 5.00 mol5.00\,\text{mol} of N2\text{N}_2 and 12.00 mol12.00\,\text{mol} of H2\text{H}_2, which react to completion.
(a)
State the limiting reactant. [1 mark]
(b)
Calculate the amount, in mol, of NH3\text{NH}_3 produced. [1 mark]
(c)
Explain how increasing pressure from atmospheric to 200 atm200\,\text{atm} affects the equilibrium position and the yield of NH3\text{NH}_3. [2 marks]
(d)
Evaluate one reason why operating at pressures significantly above 200 atm200\,\text{atm} is not used industrial practice, despite further increasing equilibrium yield. [1 mark]

Solutions

Questions 2-225

Unlock these questions with Premium

Sign Up →

That's every free question here — 1 of 225.

+224 more questions, plus Mock Papers & Worksheets, are waiting in Premium.

Upgrade