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What is the volume (in liters) of 1.50 mole of Carbon Dioxide gas that has a pressure of 1140

mm Hg and a temperature of 25.0°℃? (R= 0.0821 L atm/mol K)
A. 16.3
B. 24.5
C. 1.37
D. 2.05
E. 7.80


User Vlad Schnakovszki
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1 Answer

24 votes
24 votes

Answer:

B. 24.5

Step-by-step explanation:

To find the volume of CO₂, you need to use the Ideal Gas Law:

PV = nRT

In this equation,

-----> P = pressure (atm)

-----> V = volume (L)

-----> n = number of moles

-----> R = Ideal Gas Constant (0.0821 L*atm/mol*K)

-----> T = temperature (K)

Before you can solve for "V", you need to...

(1) convert the pressure from mmHg to atm (760 mmHg = 1 atm)

(2) convert the temperature from Celsius to Kelvin (°C + 273 = K)

P = 1,140 mmHg / 760 = 1.500 atm R = 0.0821 L*atm/mol*K

V = ? L T = 25.0°C + 273 = 298 K

n = 1.50 moles

PV = nRT <----- Ideal Gas Law Equation

(1.500 atm)V = (1.50 moles)(0.0821 L*atm/mol*K)(298 K) <----- Insert values

(1.500 atm)V = 36.6987 L*atm <----- Multiply right side

V = 24.5 L <----- Divide both sides by 1.500 atm

User Geni
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