6.01-L cylinder contains 1.25 mol of gas A and 4.54 mol of gas B, at a temperature of 32.8 °C. Calculate the partial pressure of each gas in the cylinder. Assume ideal gas I have work this question three time and can not get the rt answer
To calculate the partial pressure of each gas in the cylinder, we first need to determine the total pressure inside the cylinder using the ideal gas law equation:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles
R is the ideal gas constant (0.0821 L•atm/mol•K)
T is the temperature in Kelvin (32.8 °C + 273.15 = 305.95 K)
Since the cylinder contains two gases (A and B), we can calculate the total moles of gas in the cylinder by adding the moles of A and B together:
Total moles = moles of A + moles of B
Total moles = 1.25 mol + 4.54 mol
Total moles = 5.79 mol
Now we can rearrange the ideal gas law equation to solve for pressure (P):
P = (nRT) / V
Given that the volume (V) is 6.01 L and the total moles (n) is 5.79 mol, we can substitute these values into the equation:
P = (5.79 mol * 0.0821 L•atm/mol•K * 305.95 K) / 6.01 L
Calculating this expression will give us the total pressure inside the cylinder.
Next, we can calculate the partial pressure of each gas by multiplying the total pressure by the mole fraction of each gas.
Partial pressure of A = mole fraction of A * total pressure
Partial pressure of B = mole fraction of B * total pressure
To calculate the mole fraction of each gas, we divide the number of moles of the gas by the total number of moles in the cylinder:
Mole fraction of A = moles of A / total moles
Mole fraction of B = moles of B / total moles
Substituting the given values into these equations will give us the mole fractions of each gas.
Finally, substituting the mole fractions and the calculated total pressure into the partial pressure equations will give us the partial pressure of each gas in the cylinder.
PV = nRT
p = nRT/V
pA = 1.25*0.08206*(273.2 + 32.8)/6.01 = 5.22
pB = same thing.
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