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Ideal Gases · Paper 2 — Free Chemistry HL Practice Questions

1ChallengeSAQ-LIdeal gas law (PV = nRT)7 marksPaper 2~11 min

500\,\text{mL}

sealed glass flask contains a mixture of

\text{N}_2(\text{g})

and

\text{O}_2(\text{g})

at a total pressure of

2.50 \times 10^5\,\text{Pa}

and

300\,\text{K}

. The flask contains

0.0200\,\text{mol}

\text{N}_2

R = 8.31\,\text{J K}^{-1}\text{mol}^{-1}

(a)

(i) Calculate the partial pressure of

\text{N}_2

in the flask. [2]
(ii) Determine the number of moles of

\text{O}_2

in the flask. [2 marks]

(b)

Explain, using the assumptions of the ideal gas model, why the total pressure of a gas mixture equals the sum of the partial pressures of its components. [2 marks]

(c)

Evaluate whether the ideal gas law would accurately predict the pressure in the flask if it were cooled to

50\,\text{K}

. Justify your answer with reference to two assumptions of the kinetic molecular theory. [3 marks]

Solutions

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