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?

7.00 g of a gas occupies a volume of 4.1 L at 300 K and 1 atm pressure

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?
Answer» Solution :In the PRESENT case, `P= 1 " atm, " V= 4.1 L, T = 300 K, m= 7.0 g, " and " R=0.0821 L " atm " K^(-1) mol^(-1)` `:."" PV = m/M RT` `:."" M=(mRT)/(PV)= (7.0 xx0.0821 xx 300)/(1 x 4.1)= 42` AMU and `:. ""d = m/V` `:. "" d=(7.0)/(4.1)=1.7g L^(-1)` Hence, the molecular mass of the given gas is 42 amu and its density in the given conditions is`1.7 g L^(-1)`.