Calculate the volume occupied by 8.8 g of `CO_2` at 31.1°C and 1 Bar pressure ( R= 0.083 Bar L `K^(-1) mol^(-1)` )

Calculate the volume occupied by 4.4 g of CO_2 at STP?

The volume of 2.8g of CO at 27°C and 0.821 atm pressure is (R = 0.0821 l atm Km^(-)ol^(-) )

Energy required for excitation of electron in 1 mole H atom from ground state to 3^(rd) excited state is 2.67 times (lesser than) dissociation energy per mole of H_(2(g)) . Calculate the amount of energy needed to excite each H atom of H_(2(g)) confined in 1 L at 27^(@)C and 1 bar pressure. (R=0.083 bar litre K^(-1)" mol"^(-1), R_(B)=1.1xx10^(-7) m^(-1) ).

Calculate the temperature of '4.0' omoles of a gas occupying '5 dm^3' at '3.32' bar '[R=0.083bar dm^3 K^(-1) mol^(-1)]'

Calculate the pressure exerted by 4.4 g of CO_2 gas which is kept in a 1 litre flask at 0^circ C .