To understand the ideal gas law and be able to apply it to a wide variety of sit

Question

To understand the ideal gas law and be able to apply it to a wide variety of situations.

The absolute temperature T, volume V, and pressure p of a gas sample are related by theideal gas law, which states that

pV=nRT.

Here n is the number of moles in the gas sample and R is a gas constant that applies to all gases. This empirical law describes gases well only if they are sufficiently dilute and at a sufficiently high temperature that they are not on the verge of condensing.

In applying the ideal gas law, p must be the absolute pressure, measured with respect to vacuum and not with respect to atmospheric pressure, and T must be the absolute temperature, measured in kelvins (that is, with respect to absolute zero, defined throughout this tutorial as ?273?C). If p is in pascals and V is in cubic meters, use R=8.3145J/(mol?K). If p is in atmospheres and V is in liters, use R=0.08206L?atm/(mol?K) instead

Part A

A gas sample enclosed in a rigid metal container at room temperature (20.0?C) has an absolute pressure p1. The container is immersed in hot water until it warms to 40.0?C. What is the new absolute pressure p2?

Express your answer in terms of p1.

Explanation / Answer

Use the ideal gas law here.

pV = nRT.

Here V, n and R are constant.

Hence p/T is constant

If T increases, then P must increase also.

p1/T1 = p2/T2

P2 = p1*(T2/T1)

But you must use T in Kelvin. ie T1 = 293 K and T2 = 313 K

p2 = 313p1/293

p2 = 1.068p1

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