Is there an equation used to fond remaining pressure

When CS2 at partial pressure 1930 torr reacts with H2 at partial pressure 8650 torr at constant volume and constant temperature according to the balanced equation, determine the partial pressure (atm) of H2 that remains.

CS2(g) + 4H2(g) → CH4(g) + 2H2S(g)

Not one of which I'm aware. What you must do is calculate the moles CS2 used and the moles H2 used and subtract from the initial amounts. From the wording in the problem, I think CS2 is the limiting reagent.

Yes, there is an equation that can be used to find the remaining pressure of a gas after a reaction.

To determine the partial pressure of H2 that remains, we need to use the stoichiometry of the balanced equation and the given partial pressures of CS2 and H2.

First, let's calculate the moles of CS2 and H2 using their partial pressures and the ideal gas law equation:

PV = nRT

Where:
P is the partial pressure
V is the volume
n is the number of moles
R is the ideal gas constant
T is the temperature

For CS2:
nCS2 = (PCS2 * V) / (RT)

For H2:
nH2 = (PH2 * V) / (RT)

Next, we need to determine which reactant will be completely consumed during the reaction. The balanced equation shows that the stoichiometric ratio between CS2 and H2 is 1:4. This means that for every 1 mole of CS2 that reacts, 4 moles of H2 will react.

Since the stoichiometry of H2 in the balanced equation is greater than the stoichiometry given by its partial pressure, H2 is the limiting reactant.

Now, let's calculate the moles of H2 that react:

nH2_react = nH2_initial - (1/4 * nCS2_initial)

Finally, to find the partial pressure of H2 that remains, we will use the remaining moles of H2 and the volume:

PH2_remain = (nH2_remain * RT) / V

Please provide the values for the volume, temperature, and the initial moles of CS2 and H2 to find the final partial pressure of H2.