Question

Nitroglycerin, an explosive compound, decomposes according to the equation below.
4 C3H5(NO3)3(s) 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g)
Calculate the total volume of gases when collected at 1.2 atm and 25°C from 1.3 multiplied by 102 g of nitroglycerin.

What are the partial pressures of the gases under these conditions?

Answer 1

Convert g nitroglycerin to moles. moles = grams/molar mass.
Using the coefficients in the balanced equation, convert moles nitroglycerin to
a. moles CO2
b. moles H2O
c. moles N2
d. moles O2
Add all moles to get a total moles, then use PV = nRT to calculate total volume of all the gases.
Then use PV = nRT to calculate partial pressure of each gas. Use n for each gas, total V, R, an T.
Check my thinking.