Question

question 11
5 points
a sample of argon gas occupies a volume of 525 ml at a pressure of 842 mmhg. what is the pressure of the gas (in mmhg) if the volume is reduced at constant temperature to 136 ml?
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Explanation:

Step1: Identify the gas law

Since the temperature is constant, we use Boyle's Law: \(P_1V_1 = P_2V_2\).

Step2: Substitute the given values

Given \(V_1 = 525\space mL\), \(P_1=842\space mmHg\), \(V_2 = 136\space mL\).
From \(P_1V_1 = P_2V_2\), we can solve for \(P_2\) as \(P_2=\frac{P_1V_1}{V_2}\).
Substitute the values: \(P_2=\frac{842\times525}{136}\).

Step3: Calculate \(P_2\)

First, calculate \(842\times525 = 842\times(500 + 25)=842\times500+842\times25=421000+21050 = 442050\).
Then, \(P_2=\frac{442050}{136}\approx3250\space mmHg\).

Answer:

\(3250\space mmHg\)