CIE Jun 2015 v1 Paper 2 Q2

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The relationship pV = nRT can be derived from the laws of mechanics by assuming ideal behaviour for gases. (a) The graph represents the relationship between pV and p for a real gas at three different temperatures, T1, T2 and T3. T1 T2 T3 pV (i) Draw one line on the graph to show what the relationship should be for the same amount of an ideal gas. [1] (ii) State and explain, with reference to the graph, which of T1, T2 or T3 is the lowest temperature.[1] (iii) Explain your answer to (ii) with reference to intermolecular forces.[1] (iv) State and explain the effect of pressure on the extent to which a gas deviates from ideal behaviour.[2]UCLES 2015 9701/21/M/J/15 [Turn over<br /> (b) Aask with a volume of 100 cm3 wasrst weighed with airlling theask, and then with another gas, Y,lling theask. The results, measured at 26 C and 1.00105 Pa, are shown. Mass ofask containing air = 47.930 g Mass ofask containing Y = 47.989 g Density of air = 0.00118 g cm3 Calculate the relative molecular mass, Mr, of Y. Mr of Y =[4] (c) Although nitrogen gas makes up about 79% of the atmosphere it does not easily form compounds. (i) Explain why nitrogen is so unreactive.[1] (ii) Explain why the conditions in a car engine lead to the production of oxides of nitrogen.[1] (iii) Give an equation for a reaction involved in the removal of nitrogen monoxide, NO, from a cars exhaust gases, in the catalytic converter.[1]UCLES 2015 9701/21/M/J/15<br /> One of the main reasons for reducing the amounts of oxides of nitrogen in the atmosphere is their contribution to the formation of acid rain. (iv) Write an equation for the formation of nitric acid from nitrogen dioxide, NO2, in the atmosphere.[1] (v) Write equations showing the catalytic role of nitrogen monoxide, NO, in the oxidation of atmospheric sulfur dioxide, SO2.[2] [Total: 15]UCLES 2015 9701/21/M/J/15 [Turn over<br />

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