What is the maximum volume in L occupied by the gas released at `300K` and `0.1 atm` when `0.15mol` of `CO_(2)` is passed over `3.55g` of `KO_(2)`? `(K=39, O=16, C=12` and `R=0.08 (L.atm)/(mol.K))`

What is the value if R when its units are L atm K^(-1) mol^(-1) ?

8.2 L of an ideal gas weights 9.0 g at 300 K and 1 atm pressure. The molecular mass of the gas is

Balance chemical equation is given as following: C_(2)H_(5)OH(l)+3O_(2)(g) rarr 2CO_(2)(g)+3H_(2)O(l) What value of the volume in litre of CO_(2) (g) measured at 200 K and 1 atm, produced from the combustion of 0.25 mole of C_(2)H_(5)OH (l) / [Use R = 0.08 L "atm mol"^(-1) K^(-1) ]

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).

What is the density of N_(2) gas at 227^(@)C and 5.00 atm pressure? (R= 0.0821 atm K^(-1)mol^(-1))

7.00 g of a gas occupies a volume of 4.1 L at 300 K and 1 atm pressure. What is the molecular mass of the gas?

A 1 mol gas occupies 2.4L volume at 27^(@) C and 10 atm pressure then it show :-

16 g of SO_(x) gas occupies 5.6 L at 1 atm and 273 K.What will be the value of x ?

Calculate the work done when 2.5 mol of H_(2)O vaporizes at 1.0 atm and 25^(@)C . Assume the volume of liquid H_(2)O is negligible compared to that of vapour. Given 1 L atm =101.3 J and R = 0.082 L atm "mol"^(-1)K^(-1) .

If volume occupied by CO_(2) molecules is negligible, then calculate pressure ((P)/(5.277)) exerted by one mole of CO_(2) gas at 300 K . (a=3.592 atm L^(2)mol^(-2))