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In an experiment, a student places a small piece of pure Mg(s) into a beaker containing 250.mL of 6.44MHCl(aq) . A reaction occurs, as represented by the equation above.

The student collects the H2(g) produced by the reaction and measures its volume over water at 298 K after carefully equalizing the water levels inside and outside the gas-collection tube. The volume is measured to be 45.6mL . The atmospheric pressure in the lab is measured as 765 torr , and the equilibrium vapor pressure of water at 298 K is 24 torr

(ii) The number of moles of H2(g) produced in the reaction

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Answer:

0.81 moles H2

Explanation:

The equation of the reaction is;

Mg(s) + 2HCl(aq) ------>MgCl2(aq) + H2(g)

Number of moles of HCl reacted = concentration * volume

Number of moles of HCl reacted = 6.44 * 250/1000

Number of moles of HCl reacted = 1.61 moles of HCl

If 2 moles of HCl produces 1 mole of H2

1.61 moles of HCl produces 1.61 * 1/2 = 0.81 moles H2

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