For the reaction : CH4(g) + 2O2(g) $\rightleftharpoons$ CO2(g) + 2H2O(l), $\Delta $Hr = $-$ 170.8 kJ mol$-$1. Which of the following statements is not true?

Question

For the reaction :
CH4_(g) + 2O_2(g) $\rightleftharpoons$ CO_2(g) + 2H₂O_(l),
$\Delta $H_r = $-$ 170.8 kJ mol^$-$1.
Which of the following statements is not true?

The reaction is exothermic.

At equilibrium, the concentrations of CO_2(g) and H₂O_(l) are not equal.

The equilibrium constant for the reaction is given by K_p = ${{\left[ {C{O_2}} \right]} \over {\left[ {C{H_4}} \right]\left[ {{O_2}} \right]}}$

Addition of CH_4(g) or O_2(g) at equilibrium will cause a shift to the right.

Solution

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