The heat evolved from the combustion of carbon is used to heat water. Assuming `50%` efficiency, calculate mole of water vaporized at its boiling point `Delta H_(f)=(CO_(2))=-94K cal//mol` and `DeltaH_(vap)(H_(2)O)=9.6kcal //mol)` and `6g C` is undergoing combustion

The heat of combustion of liquid ethanol is -327.0 kcal calculate the heat of formation of ethanol. Given that the heats of formation of CO_(2)(g) and H_(2)O(l) are -94.0 kcal and -68.4 kcal respectively.

The heat of combustion of liquid ethanol is -327.0 kcal calculate the heat of formation of ethanol. Given that the heats of formation of CO_(2)(g) and H_(2)O(l) are -94.0 kcal and -68.4 kcal respectively.

In certan areas where coal is cheap, artificial gas is produced for household use by the ''water gas'' raction C(s) +H_(2)O(g) underset(600^(@)C)rarr H_(2)(g) +CO(g) Assuming that coke is 100% carbon, calculate the maximum heat obtainable at 298K from the combustion of 1kg of coke, and compare this value to the maximum heat obtainable at 298K from burning the water was produced from 1.00 kg of coke. GIven: Delta_(f)H^(Theta), H_(2)O(l) =- 68.32 kcal//mol Delta_(f)H^(Theta),CO_(2) (g) =- 94.05 kcal//mol Delta_(f)H^(Theta),CO(g) =- 26.42 kcal//mol

The value of Delta H for the combustion of C(s) is - 94.4 Kcal. The heat of formation of CO_(2)(g) is :-

The value of Delta H for the combustion of C(s) is - 94.4 Kcal. The heat of formation of CO_(2)(g) is :-

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 . Calculate rise in temperature of calorimeter if 0.01 moles of CH_(4)(g) undergoes combustion in the above bonb calorimeter 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 . 1. Calculate DeltaU_("combustion") of CH_(4)(g) at 300 K.

One mole of anhydrous MgCl_(2) dissolves in water and librates 25 cal//mol of heat. Delta H_("hydration") of MgCl_(2)=30 cal//mol . Heat of dissolution of MgCl.H_(2)O