A gas has a volume of 36.0 L and a pressure of 750. torr when the temperature is 10. °C. What is the pressure if the volume changes to 15.0 L and the temperature changes to 78 °C, if the amount of gas stays the same?

2230 torr

P1V1/T1 = P2V2/T2

750 * 36 /(273+10) = P2 * 15 /(273+78)

mnm

178.02

To solve this problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas. The combined gas law formula is:

(P₁ * V₁) / T₁ = (P₂ * V₂) / T₂

Where:
P₁ and P₂ are the initial and final pressures,
V₁ and V₂ are the initial and final volumes,
T₁ and T₂ are the initial and final temperatures.

Given:
P₁ = 750. torr
V₁ = 36.0 L
T₁ = 10. °C = 273.15 + 10 = 283.15 K (converted to Kelvin)

We need to find P₂ when:
V₂ = 15.0 L
T₂ = 78. °C = 273.15 + 78 = 351.15 K (converted to Kelvin)

Now we can plug in the values into the formula:

(750. torr * 36.0 L) / 283.15 K = (P₂ * 15.0 L) / 351.15 K

Simplifying the equation:

P₂ = (750. torr * 36.0 L * 351.15 K) / (283.15 K * 15.0 L)

Calculating the value:

P₂ = 1084725. torr / 4247 K

The pressure is approximately 255.1 torr when the volume changes to 15.0 L and the temperature changes to 78. °C.