The ideal gas law is represented by PV= nRT. As volume is held constant and the temperature increases, how would the pressure be expected to change?

Question

A. It would decrease
B. It would become zero
C. It would remain constant
D. It would increase

Answer 1

According to the ideal gas law, \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles of gas, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin.

If the volume \( V \) is held constant and the temperature \( T \) increases, then the equation can be rearranged to show that pressure \( P \) is directly proportional to temperature:

\[ P = \frac{nRT}{V} \]

Since \( n \), \( R \), and \( V \) are constant, an increase in \( T \) will result in an increase in \( P \).

Therefore, the correct answer is:

D. It would increase.