What volume of O2 at 912 mmHg and 33 degrees C is required to synthesize 11.0 mol of NO?
To find the volume of O2 gas required to synthesize 11.0 mol of NO, we can use the ideal gas law equation,
PV = nRT
Where:
P = pressure of the gas (in this case, 912 mmHg)
V = volume of the gas (what we are trying to find)
n = number of moles of gas (in this case, the number of moles of O2)
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin (in this case, 33 degrees C = 33 + 273 = 306 K)
First, convert the pressure from mmHg to atm:
912 mmHg * (1 atm / 760 mmHg) = 1.2 atm
Now we have all the necessary values to solve for the volume (V). Rearranging the ideal gas law equation:
V = (nRT) / P
Substituting the values into the equation:
V = (11.0 mol * 0.0821 L·atm/mol·K * 306 K) / 1.2 atm
Calculating this expression will give you the volume of O2 gas required in liters.