The heat of formation of HCl at 348 K from the following data will be :
`0.5H_(2)(g)+0.5Cl_(2)(g)toHCl " "DeltaH_(298)^(@)=-22060` cal. The mean heat capacities over this temperature range are,
`H_(2)(g)," " C_(p)=6.82 " cal" " mol"^(-1)K^(-1)`
`Cl_(2)(g)," " C_(p)=7.71 " cal" " mol"^(-1)K^(-1)`
`HCl(g)," " C_(p)=6.81 " cal" " mol"^(-1)K^(-1)`

The molar heat capacity of a gas at constant volume is to be 5 cal mol^(-1) K^(-1) .Find the ratio gamma=C_p // C_v for the gas.The gas constant R=2 cal mol^(-1) K^(-1) .

The molar heat capacity of a gas at constant volume is found to be 5 cal mol^(-1) K^(-1) . Find the ratio gamma = C_p/C_v for the gas. The gas constant R=2 cal mol^(-1) K^(-1).

The molar heat capacity of a gas at constant volume is found to be 5 cal mol^(-1) K^(-1) . Find the ratio gamma = C_p/C_v for the gas. The gas constant R=2 cal mol^(-1) K^(-1).

The molar heat capacity of a gas at constant volume is found to be 5 cal mol^(-1) K^(-1) . Find the ratio gamma = C_p/C_v for the gas. The gas constant R=2 cal mol^(-1) K^(-1).

Calculate the gas constant for 1 g of gas from the following data : C_p=0.245 "cal g"^(-1).^@C^(-1), C_v=0.165" cal g"^(-1).^@C^(-1)and J=4.2 xx10^7 erg cal^(-1)

Calculate the gas constant for 1 g of gas from the following data : C_p=0.245 "cal g"^(-1).^@C^(-1), C_v=0.165" cal g"^(-1).^@C^(-1)and J=4.2 xx10^7 erg cal^(-1)

The kinetic energy of 4 mol of nitrogen gas at 127^(@) C is …….. cal(R = 2 cal mol^(-1) K^(-1))

The standard enthalpy of formation of gaseous H_(2)O at 298 K is -241.82 kJ/mol. Calculate DeltaH^(@) at 373 K given the following values of the molar heat capacities at constant pressure : H_(2)O(g)=33.58 " JK"^(-1)" mol"^(-1), " "H_(2)(g)=29.84 " JK"^(-1)" mol"^(-1), " "O_(2)(g)=29.37 " JK"^(-1)" mol"^(-1) Assume that the heat capacities are independent of temperature :