Nitroglycerin (C3H5N3O9) is a powerful explosive. Its decomposition can be repre

Question

Nitroglycerin (C3H5N3O9) is a powerful explosive. Its decomposition can be represented by 4C3H5N3O9 à 6N2 + 12CO2 + 10H2O + O2 The reaction generates a large amount of heat and gaseous products. It is the sudden formation of these gases, together with their rapid expansion, that produces the explosion.

a) What is the maximum amount of carbon dioxide in grams that can be obtained from 2.000 x 102 grams of nitroglycerin?

b) Calculate the percent yield in this reaction if the amount of carbon dioxide generated is determined to be 10. 66 grams.

Explanation / Answer

4C3H5N3O9 ------> 6N2 + 12CO2 + 10H2O + O2

Molar mass of C3H5N3O9 = (3xAt.mass of C)+(5xAt.mass of H) + (3xAt.mass of N) + (9xAt.mass of O)

                                     = (3x12) + (5x1) +(3x14)+(9x16)

                                    = 227 g/mol

Molar mass of CO2 = At.mass of C + (2xAt.mass of O)

                            = 12 + (2x16)

                            = 44 g/mol

According to the balanced equation ,

4 moles of C3H5N3O9 produces 12 moles of CO2        

4x227 g of C3H5N3O9 produces 12x44 g of CO2        

2.000x102 = 200 g of C3H5N3O9 produces M g of CO2        

M = (12x44x200) /(4x227)

   = 116.3 g

Therefore the mass of CO2 produced is 116.3 g       ------(a)   which is the theoretical mass

Given actual mass of CO2 obtained is 10.66 g

Percent yield = (actual mass / theoretical mass ) x 100 '

                    = ( 10.66 / 116.3 ) x 100

                    = 9.16 %

Therefore the percent yield is 9.16%

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