For the homogeneous reactions:
`xA+yBtolY+mZ`
`DeltaH=-30kJ" "mol^(-1),DeltaS=-100JK^(-1)" "mol^(-1)`
At what temperature the reaction is at equilibrium?

For a reaction DeltaH=+29kJ" "mol^(-1),DeltaS=-35KJ^(-1)" "mol^(-1) at what temperature, the reaction will be spontaneous?

At 1 atm pressure, DeltaS=75JK^(-1)mol^(-1),DeltaH=30kJ" "mol^(-1) , the temperature of the reaction at equilibrium is

For a reaction, P+Q rarr R+S . The value of DeltaH^(@) is -"30 kJ mol"^(-1) and DeltaS" is "-"100 J K"^(-1)"mol"^(-1) . At what temperature the reaction will be at equilibrium?

For a reaction, P+Q rarr R+S . The value of DeltaH^(@) is -"30 kJ mol"^(-1) and DeltaS" is "-"100 J K"^(-1)"mol"^(-1) . At what temperature the reaction will be at equilibrium?

For the reaction at 298 K 2A + B to C DeltaH = 40 kJ "mol"^(-1) and DeltaS = 0.2 kJ K^(-1) "mol"^(-1) . At what temperature will the reaction beccomes sponatneous considering DeltaH and DeltaS to be constant over the temperature range.

(i) State hess's law. (ii) For the following reaction at 298K 2X+Y to Z DeltaH=300kJ*mol^(-1) and DeltaS=0.2kJ*K^(-1)*mol^(-1) At what temperature will the reaction become spontaneous considering DeltaH and DeltaS to be constant over the temperature range?

For the reaction at 298 K 2A+B rarr C DeltaH=400 kJ mol^(-1) and DeltaS=0.2 kJ K^(-1) mol^(-1) At what temperature will the reaction becomes spontaneous considering DeltaH and DeltaS to be contant over the temperature range.

For the reaction at 298 K, 2A+BtoC DeltaH=400 kJ mol^(-1) and DeltaS=0.2 kJ K^(-1)mol^(-1). At what temperature will the reaction becomes spontaneous considering DeltaH and DeltaS to be constant over the temperature range?