For the reaction: CH 4( g )+2 O 2( g ) leftharpoons CO 2( g )+2 H 2 O ( l ) Δ H r =-170.8 kJ mol -1 Which of the following statements is not true?

Question

For the reaction: CH 4( g )+2 O 2( g ) leftharpoons CO 2( g )+2 H 2 O ( l ) Δ H r =-170.8 kJ mol -1 Which of the following statements is not true? (A) At equilibrium, the concentrations of C O2(g) and H2O (l) are not equal (B) The equilibrium constant for the reaction is given by Kp = ( [ CO2 ] / [ CH4 ] [ O2 ] )  (C) Addition of CH 4(g) or O 2(g) at equilibrium will cause a shift to the right (D) The reaction is exothermic

Tardigrade Admin · Accepted Answer

The given reaction is:- CH 4( g )+2 O 2( g ) leftharpoons CO 2( g )+2 H 2 O ( g ) Now, K C =([ CO 2][ H 2 O ]2/[ CH 4][ O 2]2) Now, H 2 O is pure liquid, so, [ H 2 O ]=1 ⇒ K C =([ CO 2]/[ CH 4][ O 2]2) ∵ Δ Hr =-170.8 KJ / mol is negative, so reaction is exothermic by adding O 2( g ) or CH 4( g ) at equilibrium, by Le Chatelier's principle, the equilibrium shift towards right side.

Q. For the reaction:
$C H_{4} (g) + 2 O_{2} (g) ⇌ C O_{2} (g) + 2 H_{2} O (l)$
$Δ H_{r} = - 170.8 k J m o l^{- 1}$
Which of the following statements is not true?

At equilibrium, the concentrations of $C O_{2} (g)$ and $H_{2} O (l)$ are not equal

The equilibrium constant for the reaction is given by $K_{p} = \frac{[ C O _{2} ]}{[ C H _{4} ] [ O _{2} ]}$

Addition of $C H_{4} (g)$ or $O_{2} (g)$ at equilibrium will cause a shift to the right

The reaction is exothermic

Q. For the reaction: CH4​(g)+2O2​(g)⇌CO2​(g)+2H2​O(l) ΔHr​=−170.8kJmol−1 Which of the following statements is not true?

At equilibrium, the concentrations of CO2​(g) and H2​O(l) are not equal

The equilibrium constant for the reaction is given by Kp​=[CH4​][O2​][CO2​]​

Addition of CH4​(g) or O2​(g) at equilibrium will cause a shift to the right

The reaction is exothermic

Q. For the reaction:
$C H_{4} (g) + 2 O_{2} (g) ⇌ C O_{2} (g) + 2 H_{2} O (l)$
$Δ H_{r} = - 170.8 k J m o l^{- 1}$
Which of the following statements is not true?

At equilibrium, the concentrations of $C O_{2} (g)$ and $H_{2} O (l)$ are not equal

The equilibrium constant for the reaction is given by $K_{p} = \frac{[ C O _{2} ]}{[ C H _{4} ] [ O _{2} ]}$

Addition of $C H_{4} (g)$ or $O_{2} (g)$ at equilibrium will cause a shift to the right