At the temperature T(K) for the reaction X2O4(i) - 2XO2(g) Δ U = x kJ mol-, Δ S = y JK-1 mol-1 . Gibbs energy change for the reaction is (Assume X2O4. XO2 are ideal gases) Δ U = x kJ mol -1, Δ S = y JK -1 mol -1

Question

At the temperature T(K) for the reaction X2O4(i) -> 2XO2(g) Δ U = x kJ mol-, Δ S = y JK-1 mol-1 . Gibbs energy change for the reaction is (Assume X2O4. XO2 are ideal gases) Δ U = x kJ mol -1, Δ S = y JK -1 mol -1 (A) 1000 x + 2R (T - y) J mol-1 (B) 1000 x + T (2R - y) J mol-1 (C)  x + T (2R - y) J mol-1 (D)  x + 2R (T - y) J mol-1

Tardigrade Admin · Accepted Answer

Correct answer is (b) 1000 x + T (2R - y) J mol-1

Q. At the temperature T(K) for the reaction $X X_{2} O X_{4 (i)} 2 XO X_{2 (g)} Δ U = x k J mol X^{-}, ΔS = y JK X^{- 1} mol X^{- 1}$ . Gibbs energy change for the reaction is
(Assume $X X_{2} O X_{4} \cdot XO X_{2}$ are ideal gases) $Δ U = x k J m o l^{- 1}, Δ S = y J K^{- 1} m o l^{- 1}$

$1000 x + 2 R (T - y) J m o l^{- 1}$

$1000 x + T (2 R - y) J m o l^{- 1}$

$x + T (2 R - y) J m o l^{- 1}$

$x + 2 R (T - y) J m o l^{- 1}$

Correct answer is (b) $1000 x + T (2 R - y) J m o l^{- 1}$

Q. At the temperature T(K) for the reaction XX2​OX4(i)​​​2XOX2(g)​​ ΔU=x kJ molX−,ΔS=y JKX−1 molX−1. Gibbs energy change for the reaction is (Assume XX2​OX4​⋅XOX2​ are ideal gases) ΔU=xkJmol−1,ΔS=yJK−1mol−1

1000x+2R(T−y)Jmol−1

1000x+T(2R−y)Jmol−1

x+T(2R−y)Jmol−1

x+2R(T−y)Jmol−1