H2 stored in a 50.0 L container has a pressure of 500.0 torr. O2 stored in a 25.0 L container has a pressure of 800.0 torr. If both these gases are released together to be stored in a 100.0 L container, what is the total pressure in the 100.0 L container?

There is a short way and a long way to do this. Here is the long way.

Use PV = nRT and solve for n = mols H2 gas in the 50.0L container. You don't have a T listed so make up one and use it throughout the problem.
Use PV = nRT and solve for n = mols O2 in the 25.0 L container. Add nH2 + nO2 = total mols and use PV = nRT and solve for P in the 100.0 L container. Remember to use the same T (in kelvin) throughout AND remember to convert torr to atm in PV = nRT

Well, when it comes to gases, I like to think of them as little party guests. So, let's imagine we're hosting a gas party in our 100.0 L container.

First, we have H2 gas, which likes to party at 500.0 torr pressure in its 50.0 L container. That's like having a group of really enthusiastic dancers.

Then we have O2 gas, which prefers a bit higher pressure of 800.0 torr in its 25.0 L container. That's like having a group of confident singers.

When we combine these two groups of party guests in our big 100.0 L container, we have to consider how the pressure will change. It's like trying to find the perfect balance of dance moves and singing in one big performance.

To find the total pressure, we can use the formula:

(P1 * V1) + (P2 * V2) = Ptotal * Vtotal

Plugging in the values we have:

(500.0 torr * 50.0 L) + (800.0 torr * 25.0 L) = Ptotal * 100.0 L

25,000 + 20,000 = Ptotal * 100.0 L

45,000 = Ptotal * 100.0 L

Now, let's solve for Ptotal:

Ptotal = 45,000 / 100.0

Ptotal = 450.0 torr

So, the total pressure in the 100.0 L container is 450.0 torr. It's like a harmonious blend of dancers and singers, all partying together in perfect balance.

To determine the total pressure in the 100.0 L container, you can use the ideal gas law equation, which states:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

Step 1: Convert the pressure values for H2 and O2 to units of atmospheres (atm). There are 760 torr in 1 atm.

For H2:
P(H2) = 500.0 torr / 760 torr/atm
P(H2) = 0.6579 atm

For O2:
P(O2) = 800.0 torr / 760 torr/atm
P(O2) = 1.0526 atm

Step 2: Determine the number of moles for H2 and O2 using the ideal gas law equation.

For H2:
PV = nRT
n(H2) = (P(H2) * V(H2)) / (RT)

Assuming the temperature (T) is constant, we can use this equation to find the number of moles of H2.

Step 3: Determine the number of moles for O2 in a similar manner.

For O2:
PV = nRT
n(O2) = (P(O2) * V(O2)) / (RT)

Step 4: Add the number of moles of H2 and O2 to find the total number of moles.

n(total) = n(H2) + n(O2)

Step 5: Use the total number of moles and the volume of the 100.0 L container to calculate the total pressure using the ideal gas law equation.

PV = n(total)RT
P(total) = (n(total) * R * T) / V(total)

Step 6: Plug in the known values to calculate the total pressure.

P(total) = (n(total) * R * T) / V(total)
P(total) = ((n(H2) + n(O2)) * R * T) / V(total)

Remember to convert the temperature to Kelvin (K) if necessary before plugging in the values.

Please specify the temperature (T) to proceed with the calculations.

To find the total pressure in the 100.0 L container after combining the hydrogen (H2) and oxygen (O2) gases, we can use Dalton's law of partial pressures. According to Dalton's law, the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of each individual gas.

Step 1: Determine the partial pressure of H2 and O2 gases separately.
The partial pressure of a gas is the pressure it would exert if it occupied the entire volume of the container on its own.

Given:
Partial pressure of H2 (PH2) = 500.0 torr
Partial pressure of O2 (PO2) = 800.0 torr

Step 2: Combine the partial pressures to find the total pressure.
Total pressure (PTotal) = PH2 + PO2

Substituting the given values:
PTotal = 500.0 torr + 800.0 torr
PTotal = 1300.0 torr

Therefore, the total pressure in the 100.0 L container would be 1300.0 torr.