Question

If 0.44g of a colourless oxide of nitrogen occupies 224ml at 1520 mmHg and 273°c then the compound is

Answer 1

Answer:  $N_2O$

Explanation:

According to the ideal gas equation:'

$PV=nRT$

P= Pressure of the gas = 1520 mmHg = 2 atm

V= Volume of the gas = 224 mL = 0.224 L

T= Temperature of the gas = 273°C=(273+273)K=546 K   (0°C = 273 K)

R= Value of gas constant = 0.0821 Latm/K mol

$n=\frac{PV}{RT}=\frac{2\times 0.225L}{0.0821 \times 546}=0.010moles$

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}$

$0.010=\frac{0.44}{\text {Molar mass}}$

${\text {Molar mass}}=44g$

Thus the compound is $N_2O$ which has molar mass of 44.