a) Find the enthalpy of the reaction,
C(graphite) + `O_2(g)rightarrowCO_2(g)`
Given,
i) C(graphite)`+frac{1}{2}O_2(g)rightarrowCO(g),DeltaH=-110.5kJmol^-1`
ii) CO(g)`+frac{1}{2}O_2(g)rightarrowCO_2(g),DeltaH=-283.0kJmol^-1`
b) Melting of ice is a spontaneousnprocess. What are the criteria for spontaneity of a process?

Comment on the thermodynamic stability of NO(g) and NO_2(g) given : frac{1}{2}N_2(g)+frac{1}{2}O_2(g)rightarrowNO(g) , Delta_fH^o=90 kJ mol^-1 NO(g)+frac{1}{2}O_2(g)rightarrowNO_2(g) , Delta_fH^o=-74 kJ mol^-1

Calcutae the enthalpy of the reaction CO(g)+1/2O_2(g)rarrCO_2(g) from the following data C(s)+O_2(g)rarrCO_2(g) , Delta_rH^0=-394.7kJ ---------(1) C(s)+1/2O_2(g)rarrCO(g) , Delta_rH^0=-110.5kJ ---------(2)

2NO_2(g) harr N_2O_4(g): DeltaH =-52.7 kJmol_1 What is the effect of increase in pressure in the above equilibrium?

The enthalpy change in a process is the same, whether the process is carried out in a single step or inseveral steps. a) Identify tha law stated here. b) Calculate the enthalpy of formation of CH_4 from the following data : i) C_((s))+O_(2(g))rightarrowCO_(2(g)) DeltaH = -393.7kJ/mol ii) H_(2(g))+frac{1}{2}O_(2(g))rightarrowH_2O_((l)) DeltaH = -285.8kJ/mol iii) CH_(4(g))+2O_(2(g))rightarrowCO_(2(g)) DeltaH =-890.4kJ/mol

Calculate the enthalpy of formation of CH_4 from the following data: C_(s) + O_(2(g)) rarr CO_2(g) DeltaH = -393.5 kJ//mol 2H_(2(g) + O_(2(g)) rarr 2H_2O_(l) DeltaH = -571.8 kJ//mol CH_4(g)+ 2O_(2(g)) rarr CO_2(g) +2H_2O_(l) DeltaH = -890.3 kJ//mol

Predict the sign of entropy change in the following reactions. i) O_2(g)+2 SO_2(g) rarr 2 SO_3(g) ii) 2 H_2(g)+O_2(g) rarr 2 H_2 O(g)

2NO_2(g) harr N_2O_4(g): DeltaH =-52.7 kJmol_1 What change will happen if we increase the temperature?

The molecularity of a complex reaction given below is: 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g)