# If the initial temperature of an ideal gas at 2.250 atm is 62.00 "^oC, what final temperature would cause the pressure to be reduced to 1.500 atm?

With a constant amount of gas, ${P}_{1} / {T}_{1} = {P}_{2} / {T}_{2}$, according to Charles' Law.
${T}_{2} = \frac{{T}_{1} \times {P}_{2}}{P} _ 1 = \frac{335.15 \cdot K \times 1.500 \cdot a t m}{2.250 \cdot a t m} = 223 \cdot K$
You should convert this temperature back to the $\text{Celsius scale}$. It is intuitively sound that a decrease in temperature should result in a decrease in temperature. Why?