Solved

For the Reaction CuS(s)+ H₂(g) H₂S(g)+ Cu(s) $\Delta$ G°_f (CuS)= -53

Question 1

Short Answer

For the reaction CuS(s)+ H₂(g) $For the reaction CuS(s)+ H2(g) H2S(g)+ Cu(s), \Delta G°f (CuS)= -53.6 kJ/mol \Delta G°f (H2S)= -33.6 kJ/mol \Delta H°f (CuS)= -53.1 kJ/mol \Delta H°f (H2S)= - 20.6 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?$ H₂S(g)+ Cu(s),
$\Delta$ G°_f (CuS)= -53.6 kJ/mol
$\Delta$ G°_f (H₂S)= -33.6 kJ/mol
$\Delta$ H°_f (CuS)= -53.1 kJ/mol
$\Delta$ H°_f (H₂S)= - 20.6 kJ/mol
Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

For the Reaction CuS(s)+ H2(g) H2S(g)+ Cu(s) Δ\DeltaΔ G°f (CuS)= -53

Short Answer

Correct Answer:VerifiedShow Answer

For the Reaction CuS(s)+ H₂(g) H₂S(g)+ Cu(s) $\Delta$ G°_f (CuS)= -53

Correct Answer:
Verified