Respuesta :
Answer: The mass of product formed is 79.344 g.
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 oxygen = 16.7 g
Molar mass of oxygen = 32 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of oxygen}=\frac{16.7g}{32g/mol}=0.522mol[/tex]
The chemical reaction for the formation of chromium oxide follows the equation:
[tex]4Cr+3O_2\rightarrow 3Cr_2O_3[/tex]
By Stoichiometry of the reaction:
3 moles of oxygen produces 3 moles of chromium oxide.
So, 0.522 moles of oxygen will produce = [tex]\frac{3}{3}\times 0.522=0.522mol[/tex] of chromium oxide.
Now, calculating the mass of chromium oxide from equation 1, we get:
Molar mass of chromium oxide = 152 g/mol
Moles of chromium oxide = 0.522 moles
Putting values in equation 1, we get:
[tex]0.522mol=\frac{\text{Mass of chromium oxide}}{152g/mol}\\\\\text{Mass of chromium oxide}=79.344g[/tex]
Hence, the mass of chromium oxide produced in the given reaction is 79.344 grams.
