Answer: The mass of water produced in the reaction is 47.25 grams.
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] .....(1)
Given mass of ammonia = 29.7 g
Molar mass of ammonia = 17 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of ammonia}=\frac{29.7g}{17g/mol}=1.75mol[/tex]
The given chemical reaction follows:
[tex]4NH_3(g)+5O_2(g)\rightarrow 4NO(g)+6H_2O(g)[/tex]
By stoichiometry of the reaction:
4 moles of ammonia produces 6 moles of water.
So, 1.75 moles of ammonia will produce = [tex]\frac{6}{4}\times 1.75=2.625mol[/tex] of water.
Now, calculating the mass of water by using equation 1, we get:
Molar mass of water = 18 g/mol
Moles of water = 2.625 moles
Putting values in equation 1, we get:
[tex]2.625mol=\frac{\text{Mass of water}}{18g/mol}\\\\\text{Mass of water}=47.25g[/tex]
Hence, the mass of water produced in the reaction is 47.25 grams.
