A mixture of one mole of H _ 2 O and 1 mole of CO is taken in a...

$CO ( g ) + {H}_{2}O ( g ) ⇌ {CO}_{2} ( g ) + {H}_{2} ( g ) initialmoles11molesatequilibrium1 - 0 . 41 - 0 . 40 . 40 . 4Molarity0 . 6 / 100 . 6 / 100 . 4 / 100 . 4 / 10$

Now, the equilibrium constant ${K}_{C} = \dfrac{\left[{CO}_{2}\right]\left[{H}_{2}\right]}{\left[CO\right]\left[{H}_{2}O\right]}$

$⇒ {K}_{C} = \dfrac{0 . 04 \times 0 . 04}{0 . 06 \times 0 . 06} = 0 . 44$

$∴ {K}_{c} \times {10}^{2} = 44$