How does the volume of an ideal gas at constant pressure change as the temperature increases?

Regards!

Boyle's law, which summarizes these observations, states that: the volume of a certain amount of gas, which is maintained at a constant temperature, is inversely proportional to the pressure exerted, which is summarized in the following expression:

P.V = constant or P = 1 / V

Example:

An inflated balloon with a volume of 0.55L at sea level (1.0 atm) is allowed to rise to a height of 6.5 km, where the pressure is about 0.40 atm.

Assuming that the temperature remains constant, what is the final volume of the balloon?

Reasoning and solution:

Note that the number of moles and the temperature of the gas remain constant, so Boyle's law is used. From the equation:

P1V1 = P2 V2

Where P1 = 1 atm, V1 = 0.55L and P2 = 0.40 atm, as well

V2 = V1 x (P1 / P2) = 0.55 L x (1 atm / 0.40 atm) = 1.4 L

When the pressure is reduced (at a constant temperature), the volume increases. The final volume is greater than the initial volume, so the answer is reasonable.

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.