What is the resulting pressure when a sample of gas at 25°C in a 500 ml balloon with a pressure of 800 torr is changed to 75°C and a volume of 2 liters?

233.56 torr

Explanation:

We'll begin by converting celsius temperature to Kelvin temperature. This can be obtained as follow:

T(K) = T(°C) + 273

Initial temperature (T₁) = 25 °C

Initial temperature (T₁) = 25 °C + 273

Initial temperature (T₁) = 298 K

Final temperature (T₂) = 75 °C

Final temperature (T₂) = 75 °C + 273

Final temperature (T₂) = 348 K

Next, we shall convert 2 L to mL. This can be obtained as follow:

1 L = 1000 mL

Therefore,

2 L = 2 L × 1000 mL / 1 L

2 L = 2000 mL

Finally, we shall determine the resulting pressure. This can be obtained as follow:

Initial temperature (T₁) = 298 K

Initial volume (V₁) = 500 mL

Initial pressure (P₁) = 800 torr

Final temperature (T₂) = 348 K

Final volume (V₂) = 2000 mL

Final pressure (P₂) =?

P₁V₁/T₁ = P₂V₂/T₂

800 × 500 / 298 = P₂ × 2000 / 348

400000 / 298 = P₂ × 2000 / 348

Cross multiply

P₂ × 2000 × 298 = 400000 × 348

P₂ × 596000 = 139200000

Divide both side by 596000

P₂ = 139200000 / 596000

P₂ = 233.56 torr

Therefore, the resulting pressure is 233.56 torr

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