[" Consider the following processes :- "],[qquad [Delta H(kJ/mol)],[(1)/(2)A rarr B],[3B rarr2C+D],[E+A rarr2D],[" For "B+D rarr E+2C,Delta H" will be : "]]

Consider the following process : {:((1)/(2)A to B , Delta H =+ 150(kJ //mol)), (3 B to 2 C +D, Delta H= -125 (kJ//mol)), (E +A to 2 D, Delta H = + 350 (kJ//mol)):} For B + D to E + 2C, Delta H will be

In the following process, H_(2)(g) to 2H(g), " "Delta_(H-H)H^(ө)=435.0" kJ "mol^(-1) the enthalpy change involved is the

Consider the following reaction : (A) H^(+)(aq) + OH^(-)(aq) = H_(2)O(l): Delta H = -X_(1) kJ mol^(-1) (B) H_(2)(g) + (1)/(2) O_(2)(g) = H_(2)O(l): Delta H = -X_(2) kJ mol^(-1) ( C ) CO_(2)(g) + H_(2)(g) = CO(g) + H_(2)O(l): Delta H = -X_(3) kJ mol^(-1) (D) C_(2)H_(2)(g) + (5)/(2) O_(2)(g) = 2CO_(2) + H_(2)O(l): Delta H = +X_(4) kJ mol^(-1) Enthalpy of formation of H_(2)O(l) is :

Enthalpy change in the following process is A+ e^(-) to A^(-) Delta H= - X kJ//"mole" Which of the following processes has enthalpy change=X kJ/mole ?

State whether the following processes is exothermic or endothermic : H_2O (l) to H_2O (s) , Delta H = - 6.01 kJ

Using the data provided calculate the multiple bond energy (KJ mol^(-)) of a C-=C bond in c_2H_2 consider the bond energy of a C-H bond is 350 KJ mol^(-1) 2C(s)+H_2(g)rarr C_2H_2(g), Delta H=225KJ mol^(-1) 2C(s)rarr2 C(g), Delta H=1410 KJ mol^(-1) H_2(g)rarr 2H(g), Delta H=330KJ mol^(-1)