At `25^(@)C` and 760 mm of Hg pressure, a gas occupies 600 mL volume. What will be its pressure at a height where temperature is `10^(@)C` and volume of the gas is 640 mL ?

Explanation

To solve the problem, we will use the Ideal Gas Law, which states that for a given amount of gas at constant moles, the relationship between pressure, volume, and temperature can be expressed as:

\[ P_1 V_1 / T_1 = P_2 V_2 / T_2 \]

Where:
- \( P_1 \) = initial pressure
- \( V_1 \) = initial volume
- \( T_1 \) = initial temperature (in Kelvin)
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