a 2.7 L of N2 is collected at 121kpa and 288 K . if the pressure increases to 202 kpa and the temperature rises to 303 K , what volume will the gas occupy?

The gas will occupy a volume of 1.702 liters.

Explanation:

Let suppose that the gas behaves ideally. The equation of state for ideal gas is:

(1)

Where:

- Pressure, measured in kilopascals.

- Volume, measured in liters.

- Molar quantity, measured in moles.

- Temperature, measured in Kelvin.

- Ideal gas constant, measured in kilopascal-liters per mole-Kelvin.

We can simplify the equation by constructing the following relationship:

(2)

Where:

, - Initial and final pressure, measured in kilopascals.

, - Initial and final volume, measured in liters.

, - Initial and final temperature, measured in Kelvin.

If we know that , , , and , the final volume of the gas is:

The gas will occupy a volume of 1.702 liters.

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !