When 0.526 L of Ar at 1.20 atm and 227°C is mixed with 0.270 L of O2 at 501 torr and 127°C in a 400. mL flask at 27°C, what is the pressure in the flask?

Convert Ar to moles using PV = nRT

Do the same for O2. Add the moles together and use PV = nRT again with 400 mL final volume (converted to L of course).

To find the pressure in the flask, we need to use the ideal gas law. The ideal gas law is represented by the equation 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.

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

For Ar:
P1 = 1.20 atm
V1 = 0.526 L
T1 = (227°C + 273.15) K = 500.15 K (converting to Kelvin)
R = 0.0821 L·atm/(mol·K) (ideal gas constant)

Using the ideal gas law: P1V1 = n1RT1
n1 = (P1V1) / (RT1)

For O2:
P2 = 501 torr * (1 atm / 760 torr) = 0.659 atm (converting to atm)
V2 = 0.270 L
T2 = (127°C + 273.15) K = 400.15 K
R = 0.0821 L·atm/(mol·K) (ideal gas constant)

Using the ideal gas law: P2V2 = n2RT2
n2 = (P2V2) / (RT2)

Now, let's calculate the total number of moles in the flask:
n_total = n1 + n2

To calculate the pressure in the flask, we can rearrange the ideal gas law equation to solve for P:
P_total = (n_total * R * T) / V_total

V_total = 0.526 L + 0.270 L + 0.400 L = 1.196 L

Now, substitute the calculated values into the equation to find the pressure in the flask:

P_total = (n_total * R * T) / V_total

Remember to convert the temperature to Kelvin by adding 273.15:
T = 27°C + 273.15 K = 300.15 K

Now, substitute the values and solve for P_total:

P_total = ((n1 + n2) * R * T) / V_total

And that's how you can calculate the pressure in the flask.