Question

missed this? watch kcv: simple gas laws and ideal gas law; read section 6.3. you can click on the review link to access the section in your etext. a sample of gas has an initial volume of 13.4 l at a pressure of 1.33 atm. if the sample is compressed to a volume of 10.8 l (at constant temperature), what is its pressure? express the pressure in atmospheres to three significant figures. view available hint(s) p₂ = atm

Explanation:

Step1: Recall Boyle's Law

Boyle's Law states that \(P_1V_1 = P_2V_2\) (at constant temperature), where \(P_1\) and \(V_1\) are the initial pressure and volume, and \(P_2\) and \(V_2\) are the final pressure and volume.

Step2: Rearrange the formula to solve for \(P_2\)

We can rewrite the formula as \(P_2=\frac{P_1V_1}{V_2}\).

Step3: Substitute the given values

Given \(P_1 = 1.33\) atm, \(V_1=13.4\) L, and \(V_2 = 10.8\) L.

$$P_2=\frac{1.33\times13.4}{10.8}$$

First, calculate the numerator: \(1.33\times13.4 = 17.822\).
Then, divide by \(10.8\): \(P_2=\frac{17.822}{10.8}\approx1.65\) atm.

Answer:

\(1.65\) atm