Nitric acid can be produced by the reaction of
gaseous nitrogen dioxide with water.
3 NO2(g) + H2O(ℓ) −→
2 HNO3(ℓ) + NO(g)
If 916 L of NO2 gas react with water, what
volume of NO gas will be produced? Assume
the gases are measured under the same
conditions.
Answer in L.
305.3333
I agree with 305.3333 L but I would round the answer to 305 L.
To find the volume of NO gas produced, we can use the stoichiometry of the balanced chemical equation.
According to the balanced chemical equation:
3 NO2(g) + H2O(ℓ) → 2 HNO3(ℓ) + NO(g)
We can see that the ratio between NO2 and NO gases is 3:1. This means that for every 3 moles of NO2, 1 mole of NO is produced.
To solve for the volume of NO gas produced, we need to follow these steps:
Step 1: Convert the given volume of NO2 gas to moles.
Given volume of NO2 gas = 916 L
We need to convert volume to moles. To do this, we use the ideal gas law equation:
PV = nRT
n (number of moles) = PV / RT
Assuming the temperature and pressure are constant and equal for both gases, we can use the equation:
n(NO2) = (P(NO2) * V(NO2)) / (R * T)
Considering that R (the ideal gas constant) and T (temperature) are constant, we can ignore them for the calculations.
Step 2: Determine the moles of NO gas produced.
Since the ratio of NO2 to NO is 3:1, the moles of NO gas produced will be equal to one-third of the moles of NO2.
n(NO) = (1/3) * n(NO2)
Step 3: Convert the moles of NO gas to volume.
The conversion from moles to volume can be calculated using the same ideal gas law equation:
Volume(NO) = n(NO) * RT / P(NO)
Since the gases are measured under the same conditions, the pressure and temperature for both gases are assumed to be the same.
By following these steps, we can find the volume of NO gas produced.