We'll begin by calculating the mass of HNO₃ that reacted and the mass of C₃H₅N₃O₉ produced from the balanced equation. This can be obtained as follow:

C₃H₈O₃ + 3HNO₃ —> C₃H₅N₃O₉ + 3H₂O

Molar mass of HNO₃ = 1 + 14 + (16×3)

= 1 + 14 + 48

= 63 g/mol

Mass of HNO₃ from the balanced equation = 3 × 63 = 189 g

Molar mass of C₃H₅N₃O₉ = (12×3) + (1×5) + (14×3) + (16 × 9)

= 36 + 5 + 42 + 144

= 227 g/mol

Mass of C₃H₅N₃O₉ from the balanced equation = 1 × 227 = 227 g

<h3>SUMMARY:</h3>

From the balanced equation above,

227 g of C₃H₅N₃O₉ were produced by 189 g of HNO₃.

Finally, we shall determine the mass of HNO₃ that will produce 2.8 g of C₃H₅N₃O₉. This can be obtained as follow:

From the balanced equation above,

227 g of C₃H₅N₃O₉ were produced by 189 g of HNO₃.

Therefore,

2.8 g of C₃H₅N₃O₉ will be produce by = $\frac{2.8 * 189}{227} \\\\$ = 2.33 g of HNO₃

Thus, the mass of nitric acid (HNO₃) required for the production of 2.8 g of nitroglycerin? (C₃H₅N₃O₉) is 2.33 g

Learn more: brainly.com/question/24918379

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2 years ago