Multiple Choice
How many moles of oxygen (O_2) are present in 33.6 L of the gas at 1 atm and 0°C?
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7. Gases
The Ideal Gas Law
Multiple Choice
Using the ideal gas law, what quantity in moles of chlorine gas (Cl_2) at 120.0 °C and 33.3 atm would occupy a vessel of 12.0 L?
A
24.6 mol
B
16.4 mol
C
8.1 mol
D
10.2 mol
Verified step by step guidance1
Identify the known variables from the problem: pressure \(P = 33.3\) atm, volume \(V = 12.0\) L, temperature \(T = 120.0\) °C, and the gas constant \(R = 0.0821\) L·atm/(mol·K).
Convert the temperature from Celsius to Kelvin using the formula \(T(K) = T(°C) + 273.15\) to ensure the temperature is in the correct units for the ideal gas law.
Write down the ideal gas law equation: \(P \times V = n \times R \times T\), where \(n\) is the number of moles of gas.
Rearrange the ideal gas law to solve for \(n\): \(n = \frac{P \times V}{R \times T}\).
Substitute the known values of \(P\), \(V\), \(R\), and \(T\) (in Kelvin) into the equation and solve for \(n\) to find the quantity of chlorine gas in moles.
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