Question

A container holds 50.0 mL of nitrogen at 25° C and a pressure of 736 mm Hg.

What will be its volume if the temperature increases by 35° C?

Answer 1

Since pressure is constant,

V1/T1=V2/T2

where, V1= 50ml; T1=25°C = 298K; T2=298 +35 = 333K

Putting these values in above formula we get,

V2= (50×333)/298 ≅55.87 ml

Answer 2

Answer:

The final volume when the temperature increases by $35\textdegree C$ is $55.86ml$.

Explanation:

Given,

The initial volume of nitrogen, V₁ = $50ml$

The initial temperature, T₁ = $25\textdegree C$

Convert °C in K

• $1\textdegree C = 273.15K$

• $25\textdegree C = 25 + 273.15K$ = $298.15K$

The pressure, P = $736mmHg$

The temperature increases by $35\textdegree C$

Therefore,

The final temperature, T₂ = $25 + 35$ = $60\textdegree C$ = $333.15K$

The final volume, V₂ =?

As we know,

• According to Charles's law, the volume of the gas is directly proportional to the temperature at constant pressure.

Therefore,

• $\frac{V_{1} }{V_{2} } = \frac{T_{1} }{T_{2} }$

After putting the given values in the equation, we get:

• $\frac{50 }{V_{2} } = \frac{298.15}{333.15}$
• $V_{2} = \frac{16657.5}{298.15}$
• $V_{2} = 55.86ml$

Hence, the final volume, V₂ = $55.86ml$.