Nitrosyl chloride decomposes on heating to form an equilibrium mixture containing nitrogen monoxide and chlorine gas:
2NOCl(g)⇌2NO(g)+Cl2(g)2\text{NOCl}(\text{g}) \rightleftharpoons 2\text{NO}(\text{g}) + \text{Cl}_2(\text{g})2NOCl(g)⇌2NO(g)+Cl2(g)
A sample of nitrosyl chloride was heated and allowed to reach equilibrium at a given temperature. The equilibrium mixture contained 7.20 g7.20\text{ g}7.20 g of nitrogen monoxide. Calculate the mass, in ggg, of chlorine gas in the equilibrium mixture.
A different mass of nitrosyl chloride was heated and allowed to reach equilibrium at 650 K650\text{ K}650 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 |
|---|---|
| nitrosyl chloride | 0.600 |
| nitrogen monoxide | 1.80 |
| chlorine | 0.600 |
For this reaction at 650 K650\text{ K}650 K, the equilibrium constant, Kp=3.60×105 PaK_p = 3.60 \times 10^5\text{ Pa}Kp=3.60×105 Pa.
Use the value of KpK_pKp at 650 K650\text{ K}650 K (3.60×105 Pa3.60 \times 10^5\text{ Pa}3.60×105 Pa) to calculate the value of KpK_pKp at 650 K650\text{ K}650 K for the following equilibrium:
NOCl(g)⇌NO(g)+12Cl2(g)\text{NOCl}(\text{g}) \rightleftharpoons \text{NO}(\text{g}) + \frac{1}{2}\text{Cl}_2(\text{g})NOCl(g)⇌NO(g)+21Cl2(g)
Deduce the units of this new KpK_pKp.