Question

If 13.0g of CO2 gas has a volume of 0.46L at 310K , what is its pressure in millimeters of mercury?

Answer 1

To find the pressure of CO2 gas in millimeters of mercury (mmHg), we can use the ideal gas law equation: PV = nRT. First, convert the mass of CO2 to moles. Next, rearrange the ideal gas law equation to solve for pressure and substitute the known values to find the pressure of CO2 gas to be 5.92 mmHg.

Step-by-step explanation:

To find the pressure of CO2 gas in millimeters of mercury (mmHg), we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, convert the mass of CO2 to moles. The molar mass of CO2 is 44.01 g/mol. So, 13.0 g of CO2 is equal to (13.0 g)/(44.01 g/mol) = 0.295 mol.

Next, rearrange the ideal gas law equation to solve for pressure: P = (nRT)/V. Substitute the known values: P = (0.295 mol)(0.0821 L.mmHg/mol.K)(310 K)/(0.46 L) = 5.92 mmHg.

Answer 2

pV = nRT ---> p = nRT/V
n = m/M, so: p = mRT/VM, where:
p - pressure
m - mass of CO2 in grams
R - universal gas constant
T - temperature in K
V - volume in L
M - molar mass of CO2 = 44 g/mol

133.3224 Pa = 1 mm Hg

so i think You can handle this right now.