Calculate the enthalpy of formation of ethăne from the following data:
i) 'C(s)+O_2(g) eq CO_2(g) , Delta_r H^circ=-393.5 kJ'
ii) 'H_2(g)+1/2 O_2(g) rarr H_2 O(l) , Delta_r H^circ=-285.8 k J'
iiii) 'C_2 H_6(g)+7/2 O_2(g) rarr 2 CO_2(g)+3 H_2 O(l) , Delta_r H^circ=1560.0 kJ'

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

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

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)

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)

Calculate the standard enthalpy of formation of CH_3OH (l) from the following data CH_3OH(l)+3/2O_2(g)rarrCO_2(g)+2H_2O(l)DeltaH^theta=-726kJ -----(1) C(s)+O_2(g)rarrCO_2(g) DeltaH^theta=-393kJ -----(2) H_2(g)+1/2O_2(g)rarrH_2O(l) DeltaH^theta=-286kJ -----(3)

The equations representing the combustion of carbon and carbon monoxide are: 'C(s)+O_2(g) rarr CO_2(g) Delta H=394 kJ / mol' 'CO(s)+1/2 O_2(g) rarr CO_2(g) Delta H=-284.5 kJ / mol' the heat of formation of 1 mol of 'CO(g)' is

For which of the reactions, Delta S is not positive : I_2(s) rarr I_2(g) , CuO(s)+H_2(g) rarr Cu(s)+H_2 O(l) , 2 O_3(g) rarr 3 O_2(~g) , CH_4(g)+2 O_2(g) rarr CO_2(g)+2 H_2 O(g)