The volume of a balloon containing an ideal gas is 3.78 l at 1.05 atm pressure. what would the volume be at 2.75 atm with constant temperature and molar amount

1.44 L

Explanation:

According with Ideal gas law, it can be represented the dependencies between temperature, pressure, volume and molar amount of a ideal gas as follows:

Where:

In this case the gas is contained in a balloon with a initial pressure, volume, molar amount and temperature () and changes to a second state with a final pressure, volume, molar amount and temperature (). As we know, R is the Ideal Gas Constant and do not change with the state changes, then it is possible to obtain the equation:

But the state change proceed at constant temperature and molar amount, then and and replacing in the previews equation we obtain:

So we can obtain the final Volume as follows:

the dependant variable is spilled water

the independent is the heat