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Chapter 5: Problem 61

Calculate the mass in grams of hydrogen chloride produced when \(5.6 \mathrm{~L}\) of molecular hydrogen measured at STP react with an excess of molecular chlorine gas.

Short Answer

Expert verified
The mass of hydrogen chloride produced is 18.25 grams.

Step by step solution

01

Calculating the Moles of Hydrogen Gas

Calculate the number of moles of hydrogen gas using the appropriate formula: moles of H2 = volume of H2 at STP / molar volume at STP. The volume of H2 given is 5.6 L, and the molar volume at STP is 22.4 L/mol. So, moles of H2 = 5.6 L / 22.4 L/mol = 0.25 mol.
02

Applying the Stoichiometry of the Reaction

The stoichiometry of the reaction is such that for every one mole of hydrogen gas, two moles of hydrogen chloride are produced. Therefore, the moles of HCl produced = 2 * moles of H2 = 2 * 0.25 mol = 0.5 mol.
03

Converting Moles to Grams

Finally, we convert the moles of HCl to grams using its molar mass. The molar mass of HCl is approximately 36.5 grammes per mole. Hence, grams of HCl = moles of HCl * molar mass of HCl = 0.5 mol * 36.5 g/mol = 18.25 g.

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