A vessel of volume V=5.0 litre contains 1.4 g of nitrogen at temperature, T=1800 K. Find the pressure (in N / m 2 ) of the gas if 30 % of its molecules are dissociated into atoms at this temperature. (1.94 × 105)

Question

A vessel of volume V=5.0 litre contains 1.4 g of nitrogen at temperature, T=1800 K. Find the pressure (in N / m 2 ) of the gas if 30 % of its molecules are dissociated into atoms at this temperature. (1.94 × 105) (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

Mass of molecular nitrogen =(70/100) × 1.4=0.98 g Mass of atomic nitrogen =(30/100) × 1.4=0.42 g Number of moles of molecular nitrogen, n1=(0.98/28)=0.035 Number of moles of atomic nitrogen n2=(0.42/14)=0.03 The pressure of the gas = pressure exerted by molecular nitrogen + pressure exerted by atomic nitrogen i.e., P=P1+P2 =(n1 R T/V)+(n2 R T/V)=((n1+n2) R T/V) =((0.035+0.03) × 8.31 × 1800/5 × 10-3) =1.94 × 105 N / m 2

Q. A vessel of volume V=5.0 litre contains 1.4g of nitrogen at temperature, T=1800K. Find the pressure (in N/m2 ) of the gas if 30% of its molecules are dissociated into atoms at this temperature. ___ (1.94×105)

Q. A vessel of volume $V = 5.0$ litre contains $1.4 g$ of nitrogen at temperature, $T = 1800 K$ . Find the pressure (in $N / m^{2}$ ) of the gas if $30%$ of its molecules are dissociated into atoms at this temperature. ___ $(1.94 \times 1 0^{5})$