Question

In the following reaction, how many grams of nitroglycerin C3H5(NO3)3 will decompose to give 25 grams of CO2? 4C3H5(NO3)3(l) 12CO2(g) + 6N2(g) + 10H2O(g) + O2(g) The molar mass of nitroglycerin is 227.0995 grams and that of carbon dioxide is 44.01 grams.

Answer 1

Answer : The mass of nitroglycerin will be, 43.15 grams

Explanation :

First we have to calculate the moles of $CO_2$

$\text{Moles of }CO_2=\frac{\text{Mass of }CO_2}{\text{Molar mass of }CO_2}=\frac{25g}{44.01g/mole}=0.57moles$

Now we have to calculate the moles of nitroglycerin.

The balanced chemical reaction is,

$4C_3H_5(NO_3)_3(l)\rightarrow 12CO_2(g)+6N_2(g)+10H_2O(g)+O_2(g)$

From the balanced reaction we conclude that

As, 12 moles of $CO_2$ obtained from 4 mole of $C_3H_5(NO_3)_3$

So, 0.57 moles of $CO_2$ obtained from $\frac{4}{12}\times 0.57=0.19$ mole of $C_3H_5(NO_3)_3$

Now we have to calculate the mass of nitroglycerin.

$\text{Mass of }C_3H_5(NO_3)_3=\text{Moles of }C_3H_5(NO_3)_3\times \text{Molar mass of }C_3H_5(NO_3)_3$

$\text{Mass of }C_3H_5(NO_3)_3=(0.19mole)\times (227.0995g/mole)=43.15g$

Therefore, the mass of nitroglycerin will be, 43.15 grams

Answer 2

43.00 grams I'm pretty sure