Multiple Choice
What happens to the pressure of a gas sample when the volume is halved and its Kelvin temperature is doubled, assuming the amount of gas remains constant?
7. Gases
The Ideal Gas Law
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What is the pressure in a 13.0 L cylinder filled with 45.8 g of oxygen gas (O2) at a temperature of 318 K, using the Ideal Gas Law? (R = 0.0821 L·atm/mol·K)
A
1.89 atm
B
4.56 atm
C
3.12 atm
D
2.35 atm
Verified step by step guidance1
First, calculate the number of moles of oxygen gas (O2) using its molar mass. The molar mass of O2 is approximately 32.00 g/mol. Use the formula: \( \text{moles of O2} = \frac{\text{mass of O2}}{\text{molar mass of O2}} \).
Substitute the given mass of oxygen (45.8 g) and the molar mass (32.00 g/mol) into the formula to find the number of moles.
Next, apply the Ideal Gas Law, which is expressed as \( PV = nRT \), 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.
Rearrange the Ideal Gas Law to solve for pressure (P): \( P = \frac{nRT}{V} \).
Substitute the values: n (number of moles calculated), R (0.0821 L·atm/mol·K), T (318 K), and V (13.0 L) into the equation to calculate the pressure.
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