A 5.02 L sample of nitrogen dioxide gas is collected at 500°C and 5.00 atm. What is the volume of nitrogen dioxide at standard condition?
(P1V1)/T1 = (P2V2)/T2
STP = 273 Kelvin and 1 atmosphere pressure. Don't forget to change 500 C to Kelvin.
Why does a certain reagent shift the ionic reaction in the desired direction?
To find the volume of nitrogen dioxide at standard conditions (0°C and 1 atm), 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 find the number of moles of nitrogen dioxide using the ideal gas law equation. Rearranging the equation, we can solve for n:
n = PV / RT
Using the given values:
P = 5.00 atm
V = 5.02 L
T = 500°C = 500 + 273.15 K (converting to Kelvin)
Substituting the values into the equation:
n = (5.00 atm * 5.02 L) / (0.0821 L·atm/(mol·K) * (500 + 273.15) K)
Calculating:
n = 0.9205 mol
Now that we have the number of moles, we can use the ideal gas law equation again to find the volume at standard conditions. Rearranging the equation to solve for V:
V = nRT / P
Using the given values:
P = 1 atm
T = 0°C = 273.15 K (standard temperature in Kelvin)
n = 0.9205 mol
Substituting the values into the equation:
V = (0.9205 mol * 0.0821 L·atm/(mol·K) * 273.15 K) / 1 atm
Calculating:
V ≈ 21.28 L
Therefore, the volume of nitrogen dioxide at standard conditions is approximately 21.28 L.