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For the reaction A(s) rarr A(g), the var...

For the reaction `A(s) rarr A(g)`, the variation of log `K_(P)^(@)` us `(1)/(T)` is given by:

If `S_(m)^(@), A(g)` is `31.78 cal//K` mole, then calculate `S_(m)^(@) A(s)` in cal/K mole.

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Bomb calorimeters are the devices that are used to experimentally determine DeltaH and DeltaU of any reaction by measuring the temperature change in the water bath Hence , the experimatal data can be used for cross-checking theortical data, From the following theoretical data answer the question that follow: Thermodynamic data: DeltaH_(f)^(@)Ch_(4)(g)=- 15 kcal //"mole", DeltaH_(f)^(@) CO_(2)(g)=-90 kcal//"mole", DeltaH_(f)^(@)H_(2)O(l)=-60 Kcal//"mole" S_(m)^(@) CH_(4)(g)= 40 cal//"mole Kelivn" S_(m)^(@) O(g)= 45 cal//"mole Kelivn" S_(m)^(@) H_(2)O(g)= 15 cal//"mole Kelivn" S_(m)^(@) CO_(2)(g)= 50 cal//"mole Kelivn" Calorimeter data: (1) Water equivlent of calorimaeter = 36 gm (2) Sepcific heat capacity of water = 1 cal//gm .^(@)C (2) mass of water inthe water bath =164 gm All data at 300 K, R=2 cal//"mol "K . 1. Calculate DeltaU_("combustion") of CH_(4)(g) at 300 K.

Bomb calorimeters are the devices that are used to experimentally determine DeltaH and DeltaU of any reaction by measuring the temperature change in the water bath Hence , the experimatal data can be used for cross-checking theortical data, From the following theoretical data answer the question that follow: Thermodynamic data: DeltaH_(f)^(@)Ch_(4)(g)=- 15 kcal //"mole", DeltaH_(f)^(@) CO_(2)(g)=-90 kcal//"mole", DeltaH_(f)^(@)H_(2)O(l)=-60 Kcal//"mole" S_(m)^(@) CH_(4)(g)= 40 cal//"mole Kelivn" S_(m)^(@) O(g)= 45 cal//"mole Kelivn" S_(m)^(@) H_(2)O(g)= 15 cal//"mole Kelivn" S_(m)^(@) CO_(2)(g)= 50 cal//"mole Kelivn" Calorimeter data: (1) Water equivlent of calorimaeter = 36 gm (2) Sepcific heat capacity of water = 1 cal//gm .^(@)C (2) mass of water inthe water bath =164 gm All data at 300 K, R=2 cal//"mol "K . If calorimeter is modified so as to convert chemical energy into electrical by ensuring that the reaction is occurring at constant pressure then how much electron work can be obtained by combustion of 0.1 mole of CH_(4) (g) ?

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