`2 mol` `'H_(2)` is mixed with `2 gm ` of `H_(2)`. The molar heatr capacity at constant pressure for the mixture is

1 mol of H_(2) SO_(4) in mixed with 2 mol of NaIH . The heat evolved will be

56g of N_(2) ( molar mass = 28) are mixed with 44g of CO_(2) ( molar mass = 44) and the pressure of the resulting gaseous mixture is 3 atm. The partial pressure of N_(2) in the mixture is :

A mixture of O_(2) and H_(2) gases contains 20% of H_(2) gas. At a certain temperature, the total pressure of the mixture is found to be 1 bar. What is the partial pressure of O_(2) (in bar) in the mixture?

2 mol of N_(2) is mixed with 6 mol of H_(2) in a closed vessel of one litre capacity. If 50% N_(2) is converted into NH_(3) at equilibrium, the value of K_(c) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)

2 mol of N_(2) is mixed with 6 mol of H_(2) in a closed vessel of one litre capacity. If 50% N_(2) is converted into NH_(3) at equilibrium, the value of K_(c) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)

When 1g H_(2) is mixed with 1 g He than find (I ) gamma (=( C_(p))/( c_( v ))) of the mixture (ii) c_(p) ( molar specific heat at constant pressure ) of the gas mixture

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 :

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 :