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Use the ideal gas law to solve for the pressure (in atm) that is present in 5.6 moles of gas, at a temperature of 285 Kelvin and a volume of 20.0 liters.

a. 3.3 atm
b. 13 atm
c. 5.6 atm
d. 6.6 atm

User Sovanlandy
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1 Answer

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Final answer:

To find the pressure of 5.6 moles of gas at a temperature of 285 Kelvin and a volume of 20.0 liters, we use the ideal gas law, which yields approximately 1.19 atm.

Step-by-step explanation:

To calculate the pressure (in atm) of 5.6 moles of a gas at a temperature of 285 Kelvin in a volume of 20.0 liters, we use the ideal gas law: PV=nRT. Here, P is the pressure, V is the volume, n is the number of moles, T is the temperature in Kelvin, and R is the ideal gas constant, which is 0.0821 (atm·L)/(mol·K) when pressure is in atmospheres.

Inserting the given values into the ideal gas law equation, we get:

P (20.0 L) = (5.6 mol) (0.0821 atm·L/mol·K) (285 K)

To solve for P, we calculate:

P = ​(5.6 mol × 0.0821 atm·L/mol·K × 285 K) / 20.0 L

P = ​1.192924 atm

Therefore, the pressure of the gas in the given conditions is approximately 1.19 atm.

User EduSanCon
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