Question

question 30 of 30
according to boyle’s law, what would happen to the pressure of a gas if the
temperature were doubled as the number of moles and the volume were held
constant?

a. the pressure would be reduced by half.

b. the pressure would remain the same.

c. the pressure would quadruple.

d. the pressure would double.

Explanation:

Boyle's Law is \( P_1V_1 = P_2V_2 \) for constant temperature, moles. But here, we consider the ideal gas law \( PV = nRT \). Given \( n \) (moles) and \( V \) (volume) are constant, \( P \propto T \) (pressure is proportional to temperature). If \( T \) doubles (\( T_2 = 2T_1 \)), from \( \frac{P_1}{T_1}=\frac{P_2}{T_2} \) (since \( \frac{P}{T}=\frac{nR}{V} \) constant), substituting \( T_2 = 2T_1 \) gives \( P_2 = 2P_1 \). So pressure doubles.

Answer:

D. The pressure would double.