The critical constant for water are `374^@C`, 218 atm and 0.0566 L `mol^(-1)`. Calculate a, b and R.

The critical constants for water are 374^(@)C , 218 atm and 0.0566 litre mol^(-1) . Calculate a' and b' of water

The temperature of 1 mol of an ideal monoatomic gas at constant pressure of 1 atm changes from 25^(@)C and 50^(@)C . Calculate Delta U and Delta H in this process, (C_(V)=(3)/(2)R) .

The unit of rate constant of a chemical reaction is L^2. mol^(-2).s^(-1) . Calculate order of the reaction.

Vanderwaal's constants for hydrogen chloride gas are a = 3.67 atm lit^(-2) and b = 40.8 ml mol^(-1) . Find the critical temperature and critical pressure of the gas.

The inversion temperature Ti(K) of hydrogen is (Given van der Waal’s constant a and b are 0.244 atm L^2 mol^(-2) and 0.027 L mol^(-1) respectively.)

For the reaction: 2A+BrarrA_(2)B the rate k[A][B]^(2) " with "k=2.0xx10^(-6)"mol"^(-2).L^(2).s^(-1) . Calculate the initial rate of the reaction when [A]=0.1"mol.L"^(-1) , [B]=0.02"mol".L^(-1) . Calculate the rate of reaction after [A] is reduced to 0.06"mol.L"^(-1) .

At 25^(@)C , the heat of combustion of naphthalene at constant volume is -1230 " kcal mol"^(-1) . Calculate the heat of reaction at constant pressure and 25^(@)C .

For one mole of an ideal gas the slope of V vs T curve at constant pressure of 2 atm is X lit mol^(-1)K^(-1) . The value of the ideal universal gas constant 'R’ in term of X is

For one mole of an ideal gas the slope of V vs. T curve at constant pressure of 2 atm is XL*mol^(-1)*K^(-1) . The value of the ideal universal gas constant 'R' in terms of X is-

The vlaue of van der waals constant 'a' for nitrogen gas is 1.37L^(2)*atm*mol^(-2) , but that for ammonia gas is 4.30L^(2)*atm*mol^(-2) . What is the reason for this large difference ? Which one of these two gases would you expect to have higher critical temperature?