How many moles of NH3 are in a flask with a volume of 60.8 L at a pressure of 73 kPa and a temperature of 250°C?
n = PV / RT
P = 73 kPa
V = 60.8 L
T = 250+ 273 = 523 K
R = 8.314
n = 73 * 60.8 / (8.314* 523) = 1.02 mol
thank you so much i over thought this so much it made me go insane. :)
To determine the number of moles of NH3 in the given flask, we can use the ideal gas law equation, which is defined as:
PV = nRT
Where:
P = pressure in atmospheres (atm)
V = volume in liters (L)
n = number of moles (mol)
R = ideal gas constant, which is approximately 0.0821 L·atm/(mol·K)
T = temperature in Kelvin (K)
First, we need to convert the given pressure from kilopascals (kPa) to atmospheres (atm):
73 kPa * (1 atm / 101.325 kPa) ≈ 0.72 atm
Next, we need to convert the given temperature from Celsius (°C) to Kelvin (K). The relationship between Celsius and Kelvin is given by the equation:
T(K) = T(°C) + 273.15
Thus, 250°C + 273.15 ≈ 523.15 K
Now we have enough information to calculate the number of moles (n) using the ideal gas law:
n = (PV) / (RT)
n = (0.72 atm * 60.8 L) / (0.0821 L·atm/(mol·K) * 523.15 K)
Now we can plug in the values and calculate:
n ≈ 0.826 moles
Therefore, there are approximately 0.826 moles of NH3 in the given flask.