John Gunurei
Feb 25
A sample of hydrogen gas collected at STP occupies 181 mL. The gas is heated to 25 degree Celsius and is found to occupy 200 mL. What is its new pressure in mm Hg?
Exact solution working to this question please?
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ChatGPT
Feb 25
To find the new pressure of the hydrogen gas, we can use the combined gas law equation:
(P1)(V1) / (T1) = (P2)(V2) / (T2)
Where:
P1 = initial pressure (STP = 1 atm)
V1 = initial volume (181 mL)
T1 = initial temperature (273 K)
P2 = final pressure
V2 = final volume (200 mL)
T2 = final temperature (25 + 273 = 298 K)
Plugging in the values:
(1 atm)(181 mL) / (273 K) = (P2)(200 mL) / (298 K)
Solving for P2:
P2 = (1 atm)(181 mL)(298 K) / (200 mL)(273 K)
P2 = 1.33 atm
To convert the pressure to mm Hg, we can use the conversion factor:
1 atm = 760 mm Hg
P2 = 1.33 atm * 760 mm Hg/atm
P2 = 1011.8 mm Hg
Therefore, the new pressure of the hydrogen gas at 25 degrees Celsius is 1011.8 mm Hg.
(P1)(V1) / (T1) = (P2)(V2) / (T2)
Where:
P1 = initial pressure (STP = 1 atm)
V1 = initial volume (181 mL)
T1 = initial temperature (273 K)
P2 = final pressure
V2 = final volume (200 mL)
T2 = final temperature (25 + 273 = 298 K)
Plugging in the values:
(1 atm)(181 mL) / (273 K) = (P2)(200 mL) / (298 K)
Solving for P2:
P2 = (1 atm)(181 mL)(298 K) / (200 mL)(273 K)
P2 = 1.33 atm
To convert the pressure to mm Hg, we can use the conversion factor:
1 atm = 760 mm Hg
P2 = 1.33 atm * 760 mm Hg/atm
P2 = 1011.8 mm Hg
Therefore, the new pressure of the hydrogen gas at 25 degrees Celsius is 1011.8 mm Hg.
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