Question

How many grams of co2 gas would occupy 33.7 liters of volume at a temperature of -22.2 degrees Celsius and a pressure of 990 mm hg

Answer 1

The answer to your question is 93.88 grams

Step-by-step explanation:

Data

mass of CO₂ = ?

Volume = 33.7 l

Temperature = -22.2°C

Pressure = 990 mmHg

constant of ideal gases = 0.082 atm l/mol°K

Process

1.- Convert temperature to °K

Temperature = -22.2 + 273

= 250.8°K

2.- Convert the pressure to atm

1 atm ------------- 760 mmHg

x ------------- 990 mmHG

x = (990 x 1) / 760

x = 1.3 atm

3.- Use the ideal gas law to find the moles of CO₂

PV = nRT

-Solve for n

n = PV/RT

-Substitution

n = (1.3 x 33.7) / (0.082 x 250.8)

-Result

n = 43.89 / 20.57

n = 2.13

4.- Calculate the grams of CO₂

Molar mass CO₂ = 44g

44 g of CO₂ ------------ 1 mol

x ------------ 2.13 moles

x = (2.13 x 44) / 1

x = 93.88 grams