A reaction becomes spontaneous only at 500K. If `Delta H` at 500 K is 3.0 kJ, the change in entropy at 500 K

For the reactions at 298 K, 2A + B to C, Delta H = 400 kj mol^(-1) and Delta S = 0.2 kj K^(-1) mol^(-1) . At what temperature will the reaction become spontaneous considering Delta H and Delta S to be constant over the temperature range ?

Values of Delta H Delta S for the given reaction are -95.4 kJ and -198.3 J*K^(-1) respectively: N_(2)(g)+3H_(2)(g) to 2NH_(3)(g) State whether the reaction will be spontaneous at 500 K or not. Consider Delta H and DeltaS are independent of temperature.

For the following reaction at 298K 2X + Y rarr Z DeltaH = 300 kj mol (-1) and DeltaS = 0.2 kj K^(-1) mol^(-1) At what tempreature will the reaction become spontaneous considering Delta H and DeltaS to be constnt over the temperature range?

At 300 K, the enthalpy change and entropy change of a reaction are -10 kcal and -30 " cal". K^(-1) respectively. Does the reaction occur spontaneously at 400 K ? If not, then calculate the maximum temperature at which the reaction will occur spontaneously ?

For the reaction at 300 K, 2A + B to C Delta H = 450 kJ mol^(-1) and DeltaS = 0.2 kJ K^(-1) mol^(-1) .At what temperature will the reaction become spontaneous considering DeltaH and DeltaS to be constant over the temperature range?

Latent heat of vaporisation of a liquid at 500K and 1 atm pressure is 10.0 kcal//mol . What will be the change in internal energy (DeltaE) of 3 mol of liquid at same temperature?

For the homogeneous gaseous reaction A+B iff 2C+D at 500 K, K_(p)=0.04 bar. The K_(c) of the reaction at 500 K is approximately