Consider making the following changes to a fixed amount of gas: I. increasing th

Question

Consider making the following changes to a fixed amount of gas:

I. increasing the volume of the gas (keeping T constant)

II. increasing the pressure of the gas (keeping T constant)

III. increasing the temperature of the gas (keeping V constant)

Which of these changes would make the ideal gas law less accurate (increasing the importance of using the Van Der Waals Equation instead)?

A) Situation III only

B) Situation I only

C) Situations I and II only

D) Situation II only

E) Situations I and III only

Explanation / Answer

Option D) will be correct as the real gases show the ideal behavior at high temperature and low pressure. In case I pressure is deacreasing while in case III temperature is increasing. So only third case will show large deviation from ideal gas law.

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