Question

How many grams of CO2 or an 800 mL at 94.5 K PA at -10°C?

Answer 1

1.52g

Step-by-step explanation:

First, let us calculate the number of mole of CO2 present. This is illustrated below:

V = 800mL

Recall: 1000mL = 1L

800mL = 800/1000 = 0.8L

P = 94.5 KPa = 94500Pa

Recall: 101325Pa = 1atm

94500Pa = 94500/101325 = 0.93atm

T = -10°C = -10 + 273 = 263K

R = 0.082atm.L/Kmol

n =?

PV = nRT

n = PV/RT

n = (0.8x0.93)/(0.082x263)

n = 0.0345mol

Now, we can obtain the mass of CO2 as follows:

Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol

Number of mole of CO2 = 0.0345mol

Mass of CO2 = number of mole x molar Mass

Mass of CO2 = 0.0345 x 44 = 1.52g