Question

A sample of diborane gas a substance that bursts into flame when exposed to air, has a pressure of 345 tore at a temperature of -15C and a volume of 3.48 L. If conditions are changed so that the temperature is 36C and the pressure is 468 tore, what will be the volume of the sample?

Answer 1

3.072 L

Step-by-step explanation:

We are given;

• Initial pressure, P₁ = 345 torr
• Initial temperature,T₁ = -15°C

But, K = °C + 273

= -15°C + 273

= 258 K

• Initial volume, V₁ =3.48 L
• Final pressure, P₂ = 468 torr
• Final temperature, T₂ = 36°C

= 36 °C + 273

= 309 K

We are required to calculate the new volume, V₂

• Using the combined gas law;

P₁V₁/T₁ = P₂V₂/T₂

• We can calculate the new volume, V₂;
• Rearranging the formula;

V₂ =(P₁V₁T₂) ÷ (T₁P₂)

= (345 torr × 3.48 L × 309 K) ÷ (258 K × 468 torr)

= 3.072 L

Therefore, the new volume of the sample is 3.072 L