Sulfur trioxide decomposes at high temperatures to form an equilibrium mixture containing sulfur dioxide and oxygen:
2SO3(g)⇌2SO2(g)+O2(g)2\text{SO}_3(\text{g}) \rightleftharpoons 2\text{SO}_2(\text{g}) + \text{O}_2(\text{g})2SO3(g)⇌2SO2(g)+O2(g)
A sample of sulfur trioxide was heated and allowed to reach equilibrium at a given temperature. The equilibrium mixture contained 12.82 g12.82\text{ g}12.82 g of sulfur dioxide. Calculate the mass, in ggg, of oxygen gas in the equilibrium mixture (take relative atomic masses: S=32.1S = 32.1S=32.1, O=16.0O = 16.0O=16.0).
A different mass of sulfur trioxide was heated and allowed to reach equilibrium at 1000 K1000\text{ K}1000 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 |
|---|---|
| sulfur trioxide | 0.600 |
| sulfur dioxide | 1.80 |
| oxygen | 0.600 |
For this reaction at 1000 K1000\text{ K}1000 K, the equilibrium constant, Kp=2.70×105 PaK_p = 2.70 \times 10^5\text{ Pa}Kp=2.70×105 Pa.
Use the value of KpK_pKp at 1000 K1000\text{ K}1000 K (2.70×105 Pa2.70 \times 10^5\text{ Pa}2.70×105 Pa) to calculate the value of KpK_pKp at 1000 K1000\text{ K}1000 K for the following equilibrium:
SO3(g)⇌SO2(g)+12O2(g)\text{SO}_3(\text{g}) \rightleftharpoons \text{SO}_2(\text{g}) + \frac{1}{2}\text{O}_2(\text{g})SO3(g)⇌SO2(g)+21O2(g)
Deduce the units of this new KpK_pKp.