Question

40ml of oxygen was collected at 10°C at 1 bar.Calculate its volume at 273K and 1.013 bar.
Class 11 chemistry ​

Answer 1

Answer:

38.09 ml is the right answer.

Explanation:

Refer attachment for explanation!!!

Answer 2

Answer:

Volume of oxygen at 273 K temperature and 1.013 bar pressure is 38.07 ml.

Explanation:

Given,

Volume of oxygen at 10°C temperature, V₁ = 40ml

Temperature, T₁ = 10°C

• Convert °C into K
• 1°C = 273.15 K
• 10°C = (10 + 273.15) K = 283.15 K

Pressure, P₁ = 1 bar

Volume of oxygen at 273 K temperature, V₂ = ?

Temperature, T₂ = 273 K

Pressure, P₂ = 1.013 bar

As we know,

The combined gas law states that the product of the volume and pressure of an ideal gas divided by its temperature is constant.

• $\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}$

From this equation, we can calculate the volume of oxygen (V₂) at 273 K temperature:

• $\frac{1 \times 40 }{283.15} = \frac{1.013 \times V_2}{273}$
• $V_2 = \frac{40 \times 273 }{283.15 \times 1.013}$
• V₂ = 38.07 ml

Hence, volume of oxygen at 273 K temperature, V₂ = 38.07 ml.