The reaction of Cyanamide `NH_2CN_((s))` with dioxygen carried out in a bomb calorimeter and AU was found to be-741.7 KJ/mol at 298K. Calculates the enthalpy change for the reaction at 298K .

For a reaction, DeltaH = 9.08 kJ mol^-1 and DeltaS =35.7 J K^-1 mol^-1 at 298 K. Which of the following is CORRECT for the reaction at 298 K?

The enthalpy of formation of ammonia is -46.0 kJ mol^(-1) . The enthalpy for the reaction 2N_(2)(g)+6H_(2)(g)to4NH_(3)(g)

DeltaH for the reaction,2C(s) + 3H2(g) C2H6(g) is -84.4 kJ at 25 0C. Calculate ∆U for the reaction at 25 0C. (R = 8.314 J K-1 mol-1)​

The rate law for the reaction C_2H_4Br_2+3I^- rarr C_2H_4+2Br^-+I_3^- is rate = k[C_2H_4Br_2] [I^-] . The rate of the reaction is found to be 1.1xx10^(-4)M//s when the concentrations of C_2H_4Br_2 and I^- are 0.12M and 0.18M respectively. Calculate the rate constant of the reaction.

Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are -382.64 kJ mol^(-1) and -145.6 JK^(-1)mol^(-1) respectively. Standard Gibbs energy change for the same reaction at 298 K is

K_p for the reaction. 2SO_(2(g)) O2_((g)) rarr 2SO_(3(g)) is 7.1 x 10^(24) at 298 K . Calculate DeltaG° for the reaction. R = 8.314 J K^(-1) mol^(-1) .

The standard enthalpy or the decomposition of N_2 O_5 to NO_2 is 58.04 kJ and standard entropy of this reaction is 176.7 J/K. The standard free energy change for this reaction at 25^@ C is_____________.

For the reaction Ag_(2)O(s)rarr 2Ag(s)+1//2O_(2)(g) the value of Delta H=30.56 KJ mol^(_1) and Delta S = 66 JK^(-1)mol^(-1) . The temperature at which the free energy change for the reaction will be zero is :-