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.

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trelawneyacresouqrn5 trelawneyacresouqrn5 · Answer 1 · 2017-08-16T01:02:05+02:00

43.00 grams I'm pretty sure

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BarrettArcher BarrettArcher · Answer 2 · 2019-05-13T15:01:53+02:00

Answer : The mass of nitroglycerin will be, 43.15 grams

Explanation :

First we have to calculate the moles of [tex]CO_2[/tex]

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

Now we have to calculate the moles of nitroglycerin.

The balanced chemical reaction is,

[tex]4C_3H_5(NO_3)_3(l)\rightarrow 12CO_2(g)+6N_2(g)+10H_2O(g)+O_2(g)[/tex]

From the balanced reaction we conclude that

As, 12 moles of [tex]CO_2[/tex] obtained from 4 mole of [tex]C_3H_5(NO_3)_3[/tex]

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

Now we have to calculate the mass of nitroglycerin.

[tex]\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[/tex]

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

Therefore, the mass of nitroglycerin will be, 43.15 grams