Container A holds 767 mL of ideal gas at 2.50 atm. Container B holds 144 mL of ideal gas at 4.70 atm. If the gases are allowed to mix together, what is the resulting pressure?

To find the resulting pressure when the gases are mixed together, we can use the ideal gas law equation: PV = nRT. In this case, since the two gases are mixing together, the total volume and total number of gas molecules will change.

First, let's calculate the number of moles of gas in each container using the ideal gas law equation:

Container A:
P₁V₁ = n₁RT
(2.50 atm) * (767 mL) = n₁ * (0.0821 L·atm/mol·K) * T₁

Container B:
P₂V₂ = n₂RT
(4.70 atm) * (144 mL) = n₂ * (0.0821 L·atm/mol·K) * T₂

Since the temperature (T) is constant and the gas constant (R) is the same, we can set up a ratio of number of moles:

(n₁/n₂) = [(P₁V₁)/(P₂V₂)]

Now, let's find the total number of moles of gas when the two containers are mixed together:

n_total = n₁ + n₂

To find the resulting pressure, we can use the total number of moles and the total volume:

P_total = (n_total * R * T) / V_total

However, we need to find the total volume first. The total volume can be calculated by adding the individual volumes:

V_total = V₁ + V₂

Now, we can substitute the values into the equation:

P_total = (n_total * R * T) / (V₁ + V₂)

To summarize the steps:
1. Calculate the number of moles in each container using the ideal gas law equation.
2. Find the total number of moles when the containers are mixed.
3. Calculate the total volume by adding the individual volumes.
4. Use the total number of moles, total volume, gas constant, and temperature to find the resulting pressure by substituting the values into the equation.

To determine the resulting pressure when the gases are mixed together, we can use the combined gas law. The combined gas law states:

(P1 * V1) / T1 = (P2 * V2) / T2

where P1 and P2 are the initial pressures of the gases, V1 and V2 are their initial volumes, and T1 and T2 are their initial temperatures.

Since the volume and temperature are not given, we can assume that they remain constant. Therefore, we can simplify the equation to:

P1 / P2 = (V1 / V2)

Substituting the given values, we get:

P1 / P2 = (767 mL / 144 mL)

P1 / P2 = 5.33

Now, to find the resulting pressure, we can multiply the two initial pressures:

Resulting Pressure = P1 * P2 = 2.50 atm * 4.70 atm

Resulting Pressure = 11.75 atm