Answer:
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
Answer:
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
