chemistry

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.

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  1. How much of this can you do?
    A seems easy enough. What do you have for that?
    B. What's the mol count?
    C. What's the ideal gas law and what do you plug into it?

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  2. 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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