120 g of ice at 0^(@)C is mixed with 100 g of water at 80^(@)C . Latent heat of fusion is 80 cal/g and specific heat of water is 1 cal/ g-.^(@)C . The final temperature of the mixture is
Calculate the change in enthalpy , DeltaH , for the combustion of 11.2 L of hydrogen gas , measured at 0^(@)C and 1 atm pressure , to orm H_(@)O(g) : {:(DeltaH_(f)^(@),(KJ.mol^(-1))),(H_(2)O(g),-241.8):}
50 g of ice at 0^@C is mixed with 50 g of water at 80^@C . The final temperature of the mixture is (latent heat of fusion of ice =80 cal //g , s_(w) = 1 cal //g ^@C)
The amount of heat required to raise the temperature of 75 kg of ice at 0°C to water at 10°C is (latent heat of fusion of ice is 80 cal/g, specific heat of water is 1 cal/g °C)
Ten grams of ice at - 20^(@)C is to be changed to steam at 130^(@)C . The specific heat of both ice and steam is 0.5 cal // ( g^(@)C) . The specific heat of water is 1.00 cal // ( g K ) . The heat of fusion is 80 cal // g and the heat of vaporization is 540 cal // g. The entire process requires.
From the following data , the enthalpy change for the sublimation of of ice at 223 K will be [mean heat capacity of ice =2 JK^(-1)g^(-1) , mean heat capacity of H_(2)O(l)=4.2 JK^(-1)g^(-1) , mean heat capacity of H_(2)O(v)=1.85 JK^(-1)g^(-1) , entalpy of fusion of ice at 0^(@) C = 334 Jg^(-1) .enthalpy of evaporation of water at 100^(@) C = 2255 J g^(-1) ]
The enthalpy of formation for C_(2)H_(4)(g) , CO_(2)(g) and H_(2)O(l) at 25^(@)C and 1 atm. Pressure be 52 , -394 and -286 kJ mol^(-1) respectively. The enthalpy of combustion of C_(2)H_(4)(g) will be
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
