At 0°C the density of nitrogen at 1 atm is 1.25 kg/m^3. The nitrogen which occupied 1500 ml at 0°C and 1 atm was compressed at 0°C and 575 atm and the gas volume was observed to be 3.92 ml, in violati

Question

At 0°C the density of nitrogen at 1 atm is 1.25 kg/m^3. The nitrogen which occupied 1500 ml at 0°C and 1 atm was compressed at 0°C and 575 atm and the gas volume was observed to be 3.92 ml, in violation of Boyle's law. What was the final density of this non-ideal gas?

Prashant Kotian · Accepted Answer

Correct answer: C. mass of nitrogen remains constant. initial volume v1 = 1500 ml = 1.5 × 10^-3 m^3, density d1 = 1.25 kg/m^3. mass = d1 × v1 = 1.875 × 10^-3 kg. final volume v2 = 3.92 ml = 3.92 × 10^-6 m^3. final density d2 = mass / v2 = 1.875 × 10^-3 / (3.92 × 10^-6) = 478.3 kg/m^3.

💡 Solution & Explanation

Practice 22,000+ questions like this