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)
Bob Pursley worked this problem or one similar to it. Let me try to find that post and I'll give you a link.
This is close.
http://www.jiskha.com/display.cgi?id=1270968045
To find the remaining partial pressure of H2, you need to determine the moles of CS2 and H2 that react and compare them to the balanced equation.
Let's start by calculating the moles of CS2 and H2:
Moles of CS2 = (Partial Pressure of CS2) / (Total Pressure) * (Volume) / (RT)
Moles of CS2 = (1930 torr) / (total pressure) * (volume) / (RT)
Here, "Total Pressure" refers to the sum of the partial pressures of all the gases in the system, and "R" is the ideal gas constant. "T" represents the temperature in Kelvin.
Since we are working at a constant volume, the total pressure is equal to the sum of the partial pressures:
Total Pressure = Partial Pressure of CS2 + Partial Pressure of H2
Let's assume the total pressure is P torr. Then:
Total Pressure = 1930 torr + 8650 torr
P = 10580 torr
Now, we can calculate the moles of CS2:
Moles of CS2 = (1930 torr) / (10580 torr) * (volume) / (RT)
Next, we need to determine the moles of H2 that will react. According to the balanced equation, it reacts in a 1:4 ratio with CS2. So:
Moles of H2 = (Moles of CS2) * 4
Once we have the moles of H2 that reacted, we can subtract it from the initial moles of H2 to find the remaining moles of H2.
Moles of H2 remaining = Initial moles of H2 - Moles of H2 that reacted
Finally, we can calculate the partial pressure of H2 that remains:
Partial Pressure of H2 remaining = (Moles of H2 remaining) * (RT) / (Volume)