Nitrogen monoxide, NO\text{NO}NO, and oxygen, O2\text{O}_2O2, react to form nitrogen dioxide, NO2\text{NO}_2NO2, in the reversible reaction shown below:
2NO(g)+O2(g)⇌2NO2(g) 2\text{NO}\text{(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{NO}_2\text{(g)} 2NO(g)+O2(g)⇌2NO2(g)Write an expression for KcK_cKc for this equilibrium and state the units.
A chemist mixes together nitrogen monoxide and oxygen in a container of volume 4.0 dm34.0\text{ dm}^34.0 dm3.
Calculate the amount, in mol\text{mol}mol, of NO2\text{NO}_2NO2 in the equilibrium mixture.
The values of KpK_pKp for this equilibrium at 400 K400\text{ K}400 K and 600 K600\text{ K}600 K are shown below:
| Temperature / K\text{K}K | KpK_pKp / atm−1\text{atm}^{-1}atm−1 |
|---|---|
| 400400400 | 3.2×1033.2 \times 10^{3}3.2×103 |
| 600600600 | 1.5×10−21.5 \times 10^{-2}1.5×10−2 |
Predict, with a reason, whether the forward reaction is exothermic or endothermic.
The chemist increases the pressure of the equilibrium mixture at the same temperature. State, and explain in terms of KpK_pKp, how you would expect the equilibrium position to change.
