a gas has a volume of 95 mL at a pressure of 930 torr. What volume will the gas occupy if the pressure is increased to 970 torr and the temperature remains constant
91 mL
To solve this question, we can use the combined gas law, which relates the initial and final states of a gas when there are changes in pressure, volume, and temperature.
The combined gas law equation 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
In this case, the initial volume (V₁) is given as 95 mL and the initial pressure (P₁) is given as 930 torr. We are asked to find the final volume (V₂) when the pressure (P₂) is increased to 970 torr while keeping the temperature constant.
Now, we can set up and solve the equation:
(P₁ × V₁) / T₁ = (P₂ × V₂) / T₂
Given:
P₁ = 930 torr
V₁ = 95 mL
P₂ = 970 torr
T₁ = T₂ (constant)
Plugging in the values into the equation, we get:
(930 torr × 95 mL) / T₁ = (970 torr × V₂) / T₁
As the temperature is constant, we can cancel it out:
930 torr × 95 mL = 970 torr × V₂
Now, we can solve for V₂:
V₂ = (930 torr × 95 mL) / 970 torr
Calculating this, we find:
V₂ ≈ 90.4639 mL
Therefore, the gas will occupy approximately 90.4639 mL when the pressure is increased to 970 torr and the temperature remains constant.