Question

part a
what is the final volume of a gas that initially occupies 2.50 l at 298 k and is subsequently heated to 321 k? (assume the pressure is constant and no gas particles are lost)
○ 2.32 l
○ 2.96 l
○ 2.23 l
○ 2.69 l
○ none of the above
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Explanation:

Step1: Identify the gas law

Since pressure is constant, we use Charles's Law, which is \(\frac{V_1}{T_1}=\frac{V_2}{T_2}\), where \(V_1\) is initial volume, \(T_1\) is initial temperature, \(V_2\) is final volume, and \(T_2\) is final temperature.

Step2: List the given values

\(V_1 = 2.50\space L\), \(T_1 = 298\space K\), \(T_2 = 321\space K\), and we need to find \(V_2\).

Step3: Rearrange the formula to solve for \(V_2\)

From \(\frac{V_1}{T_1}=\frac{V_2}{T_2}\), we get \(V_2=\frac{V_1\times T_2}{T_1}\).

Step4: Substitute the values into the formula

\(V_2=\frac{2.50\space L\times321\space K}{298\space K}\)
First, calculate the numerator: \(2.50\times321 = 802.5\)
Then, divide by the denominator: \(\frac{802.5}{298}\approx2.69\space L\)

Answer:

2.69L