AP Chemistry
7.10 Reaction Quotient and Le Châtelier’s Principle
7.3 Reaction Quotient and Equilibrium Constant
A student studies the equilibrium decomposition of nitrosyl chloride in a closed, rigid vessel at a certain temperature.
\(2\text{NOCl(g)} \rightleftharpoons 2\text{NO(g)}+\text{Cl}_2\text{(g)}\)
At this temperature, \(K_c=4.0\times10^{-4}\). The concentrations immediately after the gases are mixed, before appreciable reaction occurs, are shown below.
Which prediction and justification concerning the change in \([\text{NO}]\) as the system approaches equilibrium are correct?
\(2\text{NOCl(g)} \rightleftharpoons 2\text{NO(g)}+\text{Cl}_2\text{(g)}\)
At this temperature, \(K_c=4.0\times10^{-4}\). The concentrations immediately after the gases are mixed, before appreciable reaction occurs, are shown below.
| Species | Initial concentration |
|---|---|
| \(\text{NOCl(g)}\) | \(0.10\text{ M}\) |
| \(\text{NO(g)}\) | \(0.020\text{ M}\) |
| \(\text{Cl}_2\text{(g)}\) | \(0.10\text{ M}\) |
Which prediction and justification concerning the change in \([\text{NO}]\) as the system approaches equilibrium are correct?
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