Edexcel Jun 2011 Paper 1 Q17

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17 0.400 g of magnesium ribbon reacted with exactly 22.2 cm3 of hydrochloric acid of concentration 1.50 mol dm3. 400 cm3 of hydrogen gas was formed, the volume being measured at room temperature and pressure. In the calculations that follow, use the following molar masses: Mg = 24.0 g mol(cid:237)1 Cl = 35.5 g mol(cid:237)1 (a) Calculate the amount (in moles) of magnesium used. (b) Calculate the amount (in moles) of hydrochloric acid used. (c) Calculate the amount (in moles) of hydrogen produced. [Molar volume of any gas at room temperature and pressure = 24 000 cm3 mol(cid:237)1] PMT (1) (1) (1) (d) Show that the calculated amounts of magnesium, hydrochloric acid and hydrogen are consistent with the following equation for the reaction Mg + 2HCl (cid:111) MgCl2 + H2 (1) 12 *P38433A01224*<br /> (e) Calculate the maximum mass of magnesium chloride that would be formed in this reaction. Give your answer to three significant figures. (3) PMT (Total for Question 17 = 7 marks) *P38433A01324* 13 Turn over<br />

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