a gas has a volume of 95 mL at a pressure of 930 torr. What volume will the gas occupy at standard temperature if pressure is held constant?
(V1/T1) = (V2/T2)
To find the volume of the gas at standard temperature, we need to use the ideal gas law equation: PV = nRT.
The ideal gas law equation relates the pressure, volume, temperature, and number of moles of a gas. Since we are holding the pressure constant, we can write the equation as:
V₁/T₁ = V₂/T₂
Where:
V₁ = initial volume of the gas
T₁ = initial temperature of the gas
V₂ = final volume of the gas (what we need to find)
T₂ = final temperature of the gas (standard temperature)
Given:
V₁ = 95 mL
P₁ = 930 torr
P₂ = 1 atm (standard pressure)
T₁ = ?
T₂ = 273 K (standard temperature)
First, we need to convert the given pressure from torr to atm. Since 1 atm = 760 torr, we can use the conversion factor:
P₁(atm) = P₁(torr) / 760
Now, we can plug in the values into the equation:
V₁ / T₁ = V₂ / T₂
Solving for V₂:
V₂ = V₁ * T₂ / T₁
Now, we need to convert the initial temperature from Celsius to Kelvin, as the ideal gas law requires temperature to be in Kelvin. To convert from Celsius to Kelvin, we add 273 to the temperature in Celsius:
T₁(K) = T₁(°C) + 273
Plug in the known values:
T₁(K) = T₁(°C) + 273 = ? + 273
Finally, substitute all the values into the equation and solve for V₂:
V₂ = V₁ * T₂ / T₁
After following these steps, you should be able to calculate the final volume of the gas at standard temperature.