ection 14.1 In a study of the system, \( \mathrm{Cl}_{3}(\mathrm{~g})+2 \mathrm{NO}(\mathrm{g})=2 \mathrm{NOCl}(\mathrm{g}) \), at \( 425 \mathrm{~K} \), several different reaction mixtures, described below, were prepared, placed in 5.00 liter containers, and allowed to attain equilibrium at \( 425 \mathrm{~K} \). Despite having different starting compositions shown, four of the five mixtures had the identical composition at equilibrium. Which one of the systems attained a different equilibrium composition than the ofhers? a. System I: 0.100 moles of \( \mathrm{Cl}_{2}, 0.000 \) moles of \( \mathrm{NO} \) and 0.600 moles of \( \mathrm{NOCl} \) b. System 2: 0.250 moles of \( \mathrm{Cl}_{3}, 0.300 \) moles of \( \mathrm{NO} \) and 0.300 moles of \( \mathrm{NOCl} \) c. System 3: 0.400 moles of \( \mathrm{Cl}_{2}, 0.600 \) moles of \( \mathrm{NO} \) and 0.000 moles of \( \mathrm{NOCl} \) d. System 4: 0.300 moles of \( \mathrm{Cl}_{2}, 0.250 \) moles of \( \mathrm{NO} \) and 0.250 moles of \( \mathrm{NOCl} \) c. System 5: 0.350 moles of \( \mathrm{Cl}_{2}, 0.500 \) moles of \( \mathrm{NO} \) and 0.100 moles of \( \mathrm{NOCl} \) ction 14.2
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This means that for every 1 mole of Cl2 that reacts, 2 moles of NO are consumed and 2 moles of NOCl are produced. Show more…
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At $35^{\circ} \mathrm{C}, K=1.6 \times 10^{-5}$ for the reaction $$ 2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) $$ Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.0 moles of pure $\mathrm{NOCl}$ in a $2.0-\mathrm{L}$ flask b. 2.0 moles of $\mathrm{NO}$ and 1.0 mole of $\mathrm{Cl}_{2}$ in a 1.0 - $\mathrm{L}$ flask c. 1.0 mole of $\mathrm{NOCl}$ and 1.0 mole of $\mathrm{NO}$ in a 1.0 - $\mathrm{L}$ flask d. 3.0 moles of $\mathrm{NO}$ and 1.0 mole of $\mathrm{Cl}_{2}$ in a 1.0 - $\mathrm{L}$ flask e. 2.0 moles of $\mathrm{NOCl}, 2.0$ moles of $\mathrm{NO},$ and 1.0 mole of $\mathrm{Cl}_{2}$ in a 1.0 - $\mathrm{L}$ flask f. $1.00 \mathrm{mol} / \mathrm{L}$ concentration of all three gases
In a given experiment, 5.2 moles of pure NOCl were placed in an otherwise empty $2.0-\mathrm{L}$ container. Equilibrium was established by the following reaction: $$2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \quad K=1.6 \times 10^{-5}$$ a. Using numerical values for the concentrations in the Initial row and expressions containing the variable $x$ in both the Change and Equilibrium rows, complete the following table summarizing what happens as this reaction reaches equilibrium. Let $x=$ the concentration of $\mathrm{Cl}_{2}$ that is present at equilibrium. b. Calculate the equilibrium concentrations for all species.
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