How many moles of ammonia would be required to react exactly with 0.470 moles of cooper (ll) oxide in the following chemical rea
ction? 2 NH₃ (g) + 3 CuO (s) → 3 Cu (s) + N₂ (g) + 3H₂O (g)
1 answer:
You might be interested in
Answer : The equilibrium concentration of in the trial solution is
Explanation :
First we have to calculate the initial moles of and
.
and,
The given balanced chemical reaction is,
Since 1 mole of reacts with 1 mole of
to give 1 mole of
The limiting reagent is,
So, the number of moles of = 0.0020 mmole
Now we have to calculate the concentration of .
Using Beer-Lambert's law :
where,
A = absorbance of solution
C = concentration of solution
l = path length
= molar absorptivity coefficient
and l are same for stock solution and dilute solution. So,
For trial solution:
The equilibrium concentration of is,
= 0.00050 M
Now calculate the .
Now calculate the concentration of .
Therefore, the equilibrium concentration of in the trial solution is