ideal gas laws chemistry

Question

At what temperature (in Kelvin) would 4.00 moles of hydrogen gas in a 100 liter container exert a pressure of 1.00 atmospheres?

Answer 1

PV=nRT

P=pressure in atm

V=volume

n=number of moles

R=the gas constant{0.082mol*k}

T=temperature in kelvin.

So pressure in P is inversely proportional to volume and directly proportional to temperature.

Volume is also directly proportional to temperature. And they are all related in with the formula P₁V₁/T_{1 =}P₂V₂/T_2.

_{so PV=nRT}

_T=PV/nR

_{T=1*100/4*0.082}

_T=100/0.328

_{T=304.88. approximately 304.9}

Answer 2

For this question, we need to use the Ideal Gas Law Equation, which is:

PV = nRT

P = the pressure (in atm, for this problem)

V = the volume in L

n = the number of moles of the gas

R = the gas constant (it is usually given to you and is 0.082057 L*atm/(mol*K)

T = the temperature (in K)

The problem says that the the gas "exerts a pressure of 1 atmosphere", so P = 1 atm. The problem says that the gas is in a "100 L container", so V = 100 L. The problem says that there are "4.00 moles of hydrogen gas" so n = 4.00 moles. T is the temperature in K, which is what we are trying to find. If we put the information into the Ideal Gas Equation, the equation looks like this:

PV = nRT

1*100 = 4.00 * 0.082057 * T

100 = 4 * 0.082057 * T

100 = 0.328228 * T

100 / 0.328228 = T

304.66 = T

So the temperature needed is 304.7 Kelvin.