A sample of 0.35 L of argon gas (at a temperature of 13 oC and a pressure of 568 torr) is heated to 156 oC and a new pressure of 897 torr. Calculate the new volume of the gas.

The new volume of the gas is 0.332 liters.

Explanation:

Let suppose that argon behaves ideally, the equation of state of the ideal gas is:

Where:

- Pressure, measured in torr.

- Volume, measured in liters.

- Molar quantity, measured in moles.

- Temperature, measured in kelvins.

- Ideal gas constant, measured in .

Since gas sample is a closed system experimenting a heating process, that is, molar quantity remains constant, the following relationship is derived from the equation of state described above:

Where:

, - Initial and final pressures, measured in torr.

, - Initial and final volumes, measured in liters.

, - Initial and final temperatures, measured in kelvins.

Now, the final volume of the gas is found:

If , , , and , the new volume of the gas is:

The new volume of the gas is 0.332 liters.

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

that tool would be a compass