Nitrogen dioxide decomposes on heating to form an equilibrium mixture containing nitrogen monoxide and oxygen:
2NO2(g)⇌2NO(g)+O2(g)2\text{NO}_2(\text{g}) \rightleftharpoons 2\text{NO}(\text{g}) + \text{O}_2(\text{g})2NO2(g)⇌2NO(g)+O2(g)
A sample of nitrogen dioxide was heated and allowed to reach equilibrium at a given temperature. The equilibrium mixture contained 4.50 g4.50\text{ g}4.50 g of nitrogen monoxide. Calculate the mass, in g\text{g}g, of oxygen gas in the equilibrium mixture.
A different mass of nitrogen dioxide was heated and allowed to reach equilibrium at 700 K700\text{ K}700 K.
Table 1: Amounts of substances at equilibrium \text{Table 1: Amounts of substances at equilibrium} Table 1: Amounts of substances at equilibrium| Substance | Amount at equilibrium / mol |
|---|---|
| nitrogen dioxide | 0.400 |
| nitrogen monoxide | 1.50 |
| oxygen | 0.600 |
For this reaction at 700 K700\text{ K}700 K, the equilibrium constant, Kp=1.35×105 PaK_p = 1.35 \times 10^5\text{ Pa}Kp=1.35×105 Pa.
Use the value of KpK_pKp at 700 K700\text{ K}700 K (1.35×105 Pa1.35 \times 10^5\text{ Pa}1.35×105 Pa) to calculate the value of KpK_pKp at 700 K700\text{ K}700 K for the following equilibrium:
NO2(g)⇌NO(g)+12O2(g)\text{NO}_2(\text{g}) \rightleftharpoons \text{NO}(\text{g}) + \frac{1}{2}\text{O}_2(\text{g})NO2(g)⇌NO(g)+21O2(g)
Deduce the units of this new KpK_pKp.