Question

Nitrous oxide is used as an anesthetic. The pressure on 2.50 L of N2O changes from 105 kPa to 40.5 kPa. If the temperature does not change, what will the new volume be?

Answer 1

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Answer 2

Nitrous oxide is used as an anesthetic. The pressure on 2.50 L of $N_{2}O$ changes from 105 kPa to 40.5 kPa. If the temperature does not change, the new volume will be 6.841 L.

Boyle's Law

Boyle's law is a gas law which states that at constant temperature, the pressure of a given quantity of a gas varies inversely with its volume occupied by it.  

According to the Boyle's Law:

PV = constant

Thus, $P_{1} V_{1} = P_{2} V_{2}$

where,

$P_{1}$ is the initial pressure

$V_{1}$ is the initial volume

$P_{2}$ is the final pressure

$V_{2}$ is the final volume

Now, put the values in above equation we get

$P_{1} V_{1} = P_{2} V_{2}$

105 kPa × 2.50 L = 40.5 kPa × $V_{2}$

$V_{2}$ = $\frac{105 kPa \times 2.50 L}{40.5 kPa}$

$V_{2} = \frac{262.5}{40.5}$

$V_{2}$ = 6.481 L

Thus, Nitrous oxide is used as an anesthetic. The pressure on 2.50 L of $N_{2}O$ changes from 105 kPa to 40.5 kPa. If the temperature does not change, the new volume will be 6.841 L.

Learn more on about the Boyle's Law here:  https://brainly.com/question/1696010

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