Question
A sample of hydrogen with a volume of 800mL exerts a pressure of 620 mm HG at 5 degrees. What volume will it occupy at STP?
Answers
GPT 3.5
To determine the volume of hydrogen at STP (standard temperature and pressure), we first need to convert the given pressure to the units typically used for STP, which are atmospheres (atm) and Kelvin (K).
1 atm = 760 mm Hg
1 atm = 101.3 kPa
1 atm = 101.3 J/cm^3
Given pressure = 620 mm Hg
Pressure in atm = 620 mm Hg * (1 atm / 760 mm Hg) = 0.8163 atm
Now we can use the ideal gas law, PV = nRT, to solve for the volume of hydrogen at STP.
P1V1 / T1 = P2V2 / T2
Since the initial temperature (5 degrees Celcius) is not at Kelvin, we need to convert it to Kelvin:
T1 = 5 + 273 = 278 K
T2 = 273 K (STP temperature)
Now we can rearrange the equation to solve for V2:
V2 = (P1V1 * T2) / (P2 * T1)
V2 = (0.8163 atm * 800 mL * 273 K) / (1 atm * 278 K)
V2 = 659.378 mL
Therefore, the volume of hydrogen at STP would be 659.378 mL.
1 atm = 760 mm Hg
1 atm = 101.3 kPa
1 atm = 101.3 J/cm^3
Given pressure = 620 mm Hg
Pressure in atm = 620 mm Hg * (1 atm / 760 mm Hg) = 0.8163 atm
Now we can use the ideal gas law, PV = nRT, to solve for the volume of hydrogen at STP.
P1V1 / T1 = P2V2 / T2
Since the initial temperature (5 degrees Celcius) is not at Kelvin, we need to convert it to Kelvin:
T1 = 5 + 273 = 278 K
T2 = 273 K (STP temperature)
Now we can rearrange the equation to solve for V2:
V2 = (P1V1 * T2) / (P2 * T1)
V2 = (0.8163 atm * 800 mL * 273 K) / (1 atm * 278 K)
V2 = 659.378 mL
Therefore, the volume of hydrogen at STP would be 659.378 mL.
Related Questions
A sample of hydrogen at 50◦C exerts a pressure of 0.377 atm. The gas is heated to 61◦C at constant v...
A sample of hydrogen with a volume of 800 mL exerts a pressure of 620 mm Hg at 5°C.
Approximately w...
A sample of hydrogen exerts a pressure of 0.418 atm at 57.0° C. The gas is heated to 88.0° C at cons...
A sample of hydrogen exerts a pressure of 0.418 atm at 57.0° C. The gas is heated to 88.0° C at cons...