A 0.63 mole sample of CO2 is in a 750 mL container. What is the pressure of the gas in torr when the has is held at -35.6oC?

12426torr

Explanation:

The following data were obtained from the question:

n = 0.63 mole

V = 750mL = 750/1000 = 0.75L

T = -35.6°C = -35.6 + 273 = 237.4K

R =0.082atm.L/Kmol

P =?

Using the ideal gas equation PV = nRT, the pressure can be obtained as follows:

PV = nRT

P = nRT/V

P = (0.63 x 0.082 x 237.4)/0.75

P = 16.35atm

Now let us convert this pressure (i.e 16.35atm) to a pressure in torr. This is illustrated below:

1atm = 760torr

16.35atm = 16.35 x 760 = 12426torr

Therefore, the pressure of the gas is 12426torr

The pressure will be 12441.2 torr

Explanation:

Step 1: Data given

Number of moles CO2 = 0.63 moles

Volume = 750 mL = 0.750 L

Temperature = -35.6 °C = 237.55 K

Step 2: Calculate pressure of the gas

p*V = n *R*T

⇒with p = the pressure of the gas = TO BE DETERMINED

⇒with V = the volume = 750 mL = 0.750 L

⇒with n = the number of moles CO2 = 0.63 moles

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 237.55 K

p = (n*R*T)/V

p = (0.63 * 0.08206  * 237.55) / 0.750

p = 16.37 atm = 12441.2 torr

The pressure will be 12441.2 torr

the earth would become to overheated and everything alive on it will eventually die from overheating. plants will eventually die as well, water will evaporate, and it will be nothing but a hot planet without anything living on it.