A sample of zinc metal is allowed to react completely with an excess of hydrochl

Question

A sample of zinc metal is allowed to react completely with an excess of hydrochloric acid:

Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g)

The hydrogen gas produced is collected over water at 25.0°C. The volume of the gas is 8.90 L, and the atmospheric pressure is 0.911 atm. Calculate the amount of zinc metal in grams consumed in the reaction.

(Vapor pressure of water at 25°C = 23.8 mmHg.)

_______ g Zn A sample of zinc metal is allowed to react completely with an excess of hydrochloric acid:

Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g)

The hydrogen gas produced is collected over water at 25.0°C. The volume of the gas is 8.90 L, and the atmospheric pressure is 0.911 atm. Calculate the amount of zinc metal in grams consumed in the reaction.

(Vapor pressure of water at 25°C = 23.8 mmHg.)

_______ g Zn

Explanation / Answer

For H2 gas, volume = V = 8.90 L

Pressure = P = 0.911 atm

Temperature = T = 25.0°C = 273+ 25 = 298 K

Ideal gas equation, PV = nRT

n = PV/RT = (0.911)(8.90)/[(0.082)(298)] = 0.332 mol

According to reaction, 1 mol of Zn produces 1 mol of H2.

So, 0.332 mol of H2 will be produced from 0.332 mol of Zn.

Atomic mass of Zn = 65.38 g/mol

Mass of Zn consumed= moles*molar mass = 0.332*65.38 = 21.69 g

Amount of Zn metal used in reaction = 21.69 g

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