# Chemistry: Please check my work!I am stumped

When nitroglycerin (C3H5N3O9) explodes, it decomposes into the following gases: CO2, N2, NO, and H2O. If 239g of nitroglycerin explodes, what volume will the mixture of gaseous produces occupy at 1.00 atm pressure and 2678oC?

a. Write a balanced equation for the reaction.

b. Use stoichiometry to find the moles of ALL the gas products combined.

c. Use the ideal gas law to solve the volume of the products of the explosion.

Is A correct?
A. 4C3H5N3O9>12CO2+5N2+2NO+10H2O

Not sure about the other yet. I am trying to figure it out , so I can explain it to my daughter. Is A correct?

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1. I didn't check the oxidation numbers and electron change but the coefficients appear to be ok.
To continue, convert 239 g nitro into mols. mol = grams/molar mass
Use the coefficients in the balanced equation to convert mols nitro to mols N2, mols H2O, mols CO2, mols NO. That's part b.
Add the mols together to find total mols, then use PV = nRT to find V. This is part C. Don't forget that P is in atmospheres and T must be in kelvin. which is 273 + C

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