Question

The value K for H2 + CO2 is 1.80 at 1000°C. if 1.0 mole of each H2 and CO2 are place in 1 litre flask, the final equilibrium concentration of CO at 1000°C will be

Answer 1

Answer : The final equilibrium concentration of CO is 0.5730 mole/L

Solution : Given,

The value of equilibrium constant, K = 1.80

Moles of $H_2$ = 1 mole

Moles of $CO_2$ = 1 mole

Volume = 1 L

The Net equilibrium reaction is,

                                          $H_2+CO_2\rightleftharpoons CO+H_2O$

initial concentration      1 M      1 M          0        0

At equilibrium              (1-x)M    (1-x)M    (x) M     (x) M

The expression for equilibrium reaction is,

$K=\frac{[H_2O][CO]}{[H_2][CO_2]}$

Now put all the values in this expression, we get the value of 'x'

$1.8=\frac{(x)\times (x)}{(1-x)\times (1-x)}$

By rearranging the terms, we get 'x'

x = 0.5730 M

Therefore, the concentration of CO at equilibrium = (x) M = 0.5730 M = 0.5730 mole/L.

Answer 2

Explanation:

how equation rearranged????