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?
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?
Answers
DrBob222
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.
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.