To solve this problem, we can use the combined gas law which states that the ratio of the product of pressure and volume to temperature remains constant. The formula is:

P1V1/T1 = P2V2/T2

Where:
P1 = initial pressure = 1.00 atm
V1 = initial volume = 825 mL
T1 = initial temperature = 21°C = 294.15 K (convert from Celsius to Kelvin by adding 273.15)

P2 = final pressure (what we're solving for)
V2 = final volume = 655 mL
T2 = final temperature = 52°C = 325.15 K

Rearranging the formula to solve for P2 gives us:

P2 = P1V1T2 / T1V2

Substituting the known values:

P2 = (1.00 atm * 825 mL * 325.15 K) / (294.15 K * 655 mL)

P2 = 1.39 atm

So, the pressure of the hydrogen gas after being heated to 52°C and compressed to a volume of 655 mL will be 1.39 atm.

Question

To solve this problem, we can use the combined gas law which states that the ratio of the product of pressure and volume to temperature remains constant. The formula is:

P1V1/T1 = P2V2/T2

Where:
P1 = initial pressure = 1.00 atm
V1 = initial volume = 825 mL
T1 = initial temperature = 21°C = 294.15 K (convert from Celsius to Kelvin by adding 273.15)

P2 = final pressure (what we're solving for)
V2 = final volume = 655 mL
T2 = final temperature = 52°C = 325.15 K

Rearranging the formula to solve for P2 gives us:

P2 = P1V1T2 / T1V2

Substituting the known values:

P2 = (1.00 atm * 825 mL * 325.15 K) / (294.15 K * 655 mL)

P2 = 1.39 atm

So, the pressure of the hydrogen gas after being heated to 52°C and compressed to a volume of 655 mL will be 1.39 atm.

Knowee AI · Accepted Answer

To solve this problem, we can use the combined gas law which states that the ratio of the product of pressure and volume to temperature remains constant. The formula is:

P1V1/T1 = P2V2/T2

Where:
P1 = initial pressure = 1.00 atm
V1 = initial volume = 825 mL
T1 = initial temperature = 21°C = 294.15 K (convert from Celsius to Kelvin by adding 273.15)

P2 = final pressure (what we're solving for)
V2 = final volume = 655 mL
T2 = final temperature = 52°C = 325.15 K

Rearranging the formula to solve for P2 gives us:

P2 = P1V1T2 / T1V2

Substituting the known values:

P2 = (1.00 atm * 825 mL * 325.15 K) / (294.15 K * 655 mL)

P2 = 1.39 atm

So, the pressure of the hydrogen gas after being heated to 52°C and compressed to a volume of 655 mL will be 1.39 atm.

A sample of hydrogen gas in a compressible container occupies a volume of 825 mL at 21oC and 1.00 atm. What will its pressure be if the container is heated to 52oC and the volume is changed to 655 mL?Multiple choice question.3.12 atm0.509 atm1.13 atm1.39 atm

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