The volume of a gas at 23◦C and 0.13 atm is 73 mL. What volume will the same gas sample occupy at standard conditions?
Answer in units of mL
Better to the calculation yourself. I don't buy Samir's answer.
(P1V1/T1) = (P2V2/T2)
To find the volume that the same gas sample will occupy at standard conditions, we need to use the ideal gas law equation: PV = nRT.
In this equation:
- P represents the pressure of the gas.
- V represents the volume of the gas.
- n represents the number of moles of the gas.
- R is the ideal gas constant.
- T is the temperature in Kelvin.
Since we want to convert the volume to standard conditions, we need to convert the temperature from Celsius to Kelvin. To do that, we add 273 to the Celsius temperature.
Given:
- Temperature (T) = 23C + 273 = 296K
- Pressure (P) = 0.13 atm
- Volume (V) = 73 mL
We can rearrange the ideal gas law equation to solve for the new volume:
V1 / T1 = V2 / T2
Where:
- V1 is the initial volume
- T1 is the initial temperature
- V2 is the final volume
- T2 is the final temperature
Substituting the known values into the equation:
73 mL / 296 K = V2 / 273 K
Now, we can solve for V2:
V2 = (73 mL / 296 K) * 273 K
Calculating this equation will give us the volume at standard conditions:
V2 = (73 / 296) * 273 mL
Therefore, the volume that the same gas sample will occupy at standard conditions is approximately 67.75 mL.