Determine which of the following reactions at constant pressure represent surrounding that do work on the system environment :
(P) `4NH_(3)(g) + 7O_(2)(g) to 4 NO_(2)+ 6H_(2)O(g)`
(Q) `CO.O(g)+ 2H_(2)(g) to CH_(3)OH(l)`
(R) `C("s,graphite")+H_(2)O(g) to CO(g)+H_(2)(g)`
(S) `H_(2)O(s) to H_(2)O(l)`

Determine which of the following reactions at constant pressure represent surrounding that do work on the system environment : (P) 4NH_(3)(g) + 7O_(2)(g) to 4 NO_(2) (g) + 6H_(2)O(g) (Q) CO(g)+ 2H_(2)(g) to CH_(3)OH(l) (R) C("s,graphite")+H_(2)O(g) to CO(g)+H_(2)(g) (S) H_(2)O(s) to H_(2)O(l)

Determine which of the following reactions at constant pressure represents surroundings that do work on the system: I. 4NH_(3)(g)+7O_(2)(g)rarr4NO_(2)(g)+6H_(2)O(g) II. CO(g)+2H_(2)(g)rarrCH_(3)OH(l) III. C(s,"graphite")+H_(2)O(g)rarrCO(g)+H_(2)(g) IV. H_(2)OrarrH_(2)O(l)

Determine which of the following reactions at constant pressure represents surroundings that do work on the system: I. 4NH_(3)(g)+7O_(2)(g)rarr4NO_(2)(g)+6H_(2)O(g) II. CO(g)+2H_(2)(g)rarrCH_(3)OH(l) III. C(s,"graphite")+H_(2)O(g)rarrCO(g)+H_(2)(g) IV. H_(2)OrarrH_(2)O(l)

In which of the following reactions At 25^(@)C , does the standard enthalpy change correspond to the standard enthalpy of formation of H_(2)O(l) ? Give reasons. (i) H_(2)(g) +(3)/(2)O_(3)(g) to H_(2)O(l) (ii) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l) (iii) 2H(g)+O_(2)(g) to H_(2)O(l) .

In which of the following changes at constant pressure is work done by system on surrounding? By the surrounding on system ? {:("Initial state",,"Final state"),("(i) "H_(2)O(g),to,H_(2)O(l)),("(ii) "H_(2)O(s),to,H_(2)O(g)),("(iii) "H_(2)O(l),to,H_(2)O(s)),("(iv) "3H_(2)(g)+N_(2)(g),to,2NH_(3)(g)),("(v) "CaCO_(3)(s),to,CaO(s)+CO_(2)(g)):}

Calculate the enthalpy of combustion of glucose from the follwoing data : C("graphite") +O_(2)(g) to CO_(2)(g) Delta_(r)H^(@) = -395.0 kJ H_(2)(g) + 1/2 O_(2)(g) to H_(2)O(l) Delta_(r)H^(@) = - 269.4 kJ 6C("graphite") + 6H_(2)(g) + 3O_(2)(g) to C_(6)H_(12)O_(6)(s) Delta_(r)H^(@) = -1169.9 kJ

Calculate the enthalpy of formation of methane from the following data : C(s) + O_(2)(g) to CO_(2)(g) Delta_(r)H^(@) = -393.5 kJ 2H_(2)(g) + O_(2)(g) to 2H_(2)O(l) Delta_(r)H^(@) = -571.8 kJ CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l) Delta_(r)H^(@) = -890.3 kJ

Heat of formation of CH_(4) are: If given heat: C(s)+ O_(2)(g) rarr CO_(2) (g) " "DeltaH =-394 KJ 2H_(2) (g)+ O_(2)(g) rarr 2H_(2)O(l) rarr 2H_(2)O(l) " "DeltaH =-568 KJ CH_(4)(g) + 2O_(2)(g) rarr CO_(2)(g) + 2H_(2)O(l) " " DeltaH =- 892 KJ