given the reaction 4NH3 + 3O2 =2N2 + 6H20
how many moles of N2 would form if 2.77 moles of NH3 reacted completely?
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To determine the number of moles of N2 that would form if 2.77 moles of NH3 reacted completely, we can utilize the balanced equation.
The balanced equation is: 4NH3 + 3O2 → 2N2 + 6H2O
From the balanced equation, we can see that 4 moles of NH3 react to form 2 moles of N2.
Now we are given that we have 2.77 moles of NH3. To find the number of moles of N2, we can set up a proportion using the ratio of moles:
(4 moles of NH3 / 2 moles of N2) = (2.77 moles of NH3 / x moles of N2)
To solve for x (the number of moles of N2), we can cross multiply:
4 moles of NH3 * x moles of N2 = 2 moles of N2 * 2.77 moles of NH3
4x = (2 * 2.77)
4x = 5.54
x = 5.54 / 4
x = 1.385
Therefore, if 2.77 moles of NH3 react completely, 1.385 moles of N2 would form.