For the combustion of `CH_(4)` at 1 atm pressure and 300 K, which of the following options is correct?

One mole of an ideal gas is subjected to adiabatic expansion form initail state of (10"atm",300K) to final pressure of 1 atm against constant external pressure. Which of the following option contain correct change in thermodynamic parameters for the above process. (Given: gamma=(4)/(3))

Enthalpy of CH_(4)+(1)/(2)O_(2)rarrCH_(3)OH is negative. If enthalpy of combustion of CH_(4) and CH_(4)OH are x and y respectively, then which relation is correct?

Enthalpy of CH_(4) + 1/2 O_(2) rightarrow CH_(3)OH is negative. If enthalpy of combustion of CH_(4) and CH_(3)OH are x and y repectively. Then which relation is correct ?

The heat of combustion of H_(2)(g) at constant pressure and 300k is -280kJ mol^(-1) . What will be the heat of combustion at constant volume and at 300K ?

The heat of combustion of H_(2)(g) at constant pressure and 300k is -280kJ mol^(-1) . What will be the heat of combustion at constant volume and at 300K ?

One litre of a gas weighs 2 g at 300 K and 1 atm pressure. If the pressure is made 0.75 atm, at which of the following temperature will one litre of the same gas weigh 1 gram : 1) 450K 2) 600K 3) 800K 4)900K

One litre of a gas weighs 2 g at 300 K and 1 atm. Pressure . If the pressure is made 0.75 atm, at which of the following temperature will one litre of the same gas weigh one gram ?