Calculate the resulting pressure if 4.50 liters of nitrogen at 35 degrees Celsius and 790 torr and 3.7 liters of oxygen at 15 degrees Celsius and 750 torr are pumped into a 1.00 liters container at 25 degrees celsius. Assume ideal gas behavior.

Use PV = nRT and solve for n N2.

Use PV = nRT and solve for n O2
Add n = mols to find total mols.
Then use PV = nRT and solve for P in the new container at the new conditions.

To calculate the resulting pressure, we can use the ideal gas law equation:

PV = nRT

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

First, let's calculate the number of moles for each gas using the ideal gas law equation by rearranging it to solve for n:

n = PV / RT

For nitrogen:
P = 790 torr
V = 4.50 liters
T = 35 °C + 273.15 (convert to Kelvin) = 308.15 K

Using the ideal gas constant R = 0.0821 L · atm/(mol · K), we can calculate the number of moles of nitrogen:

n₁ (nitrogen) = (790 torr) * (4.50 L) / (0.0821 L · atm/(mol · K) * 308.15 K)

Now, let's calculate the number of moles for oxygen:
P = 750 torr
V = 3.7 liters
T = 15 °C + 273.15 (convert to Kelvin) = 288.15 K

Using the same ideal gas constant R, we can calculate the number of moles of oxygen:

n₂ (oxygen) = (750 torr) * (3.7 L) / (0.0821 L · atm/(mol · K) * 288.15 K)

Next, we need to calculate the total number of moles (n_total) by adding the moles of nitrogen and oxygen:

n_total = n₁ (nitrogen) + n₂ (oxygen)

Now, we can calculate the total pressure (P_total) by using the ideal gas law equation:

P_total = n_total * R * T / V

Since the nitrogen and oxygen are being pumped into a 1.00 liters container at 25 °C, we can use the same temperature for the final calculation:

T = 25 °C + 273.15 (convert to Kelvin) = 298.15 K

Now, substituting the values into the equation:

P_total = n_total * R * T / V
= (n₁ + n₂) * (0.0821 L · atm/(mol · K)) * (298.15 K) / (1.00 L)

Finally, calculate the resulting pressure:

P_total = (n₁ + n₂) * 0.0821 * 298.15

By plugging in the calculated values for n₁ and n₂, we can find the resulting pressure.