10 L of Cl2 gas reacts with 40L of H2 gas under same condiitions of temperature and pressure. How much volume of HCl should be produced?
Correct answer: C. 20L
- A. 40L
- B. 30L
- C. 20L
- D. 10L
Explanation
The balanced chemical equation π»2 + πΆπ2 = 2π»πΆπ shows that each mole of Cl2 produces two moles of HCl. At constant temperature and pressure, volumes of gases are proportional to moles. Thus, 10L of Cl2 will react with 10L of H2 to produce 20L of HCl. Cl2 is the limiting reactant, and the excess H2 remains unreacted. Option C is correct; other options either misinterpret the stoichiometry or the limiting reactant concept.
This question appeared on the ETEA MDCAT 2008 paper, which you can sit online with every answer explained.
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The mole connects the microscopic number of particles with measurable mass, using Avogadro's number, 6.022 Γ 10Β²Β³ particles per mole. Questions involve molar mass, conversion between mass, moles and particles, percentage composition, empirical and molecular formulas, and distinguishing atoms, molecules, ions and formula units.
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