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.
Please check A. And help with B and C!!
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?
See your post above.
Yes, your balanced equation for the reaction is correct.
Now, let's move on to solving part B - finding the moles of all the gas products combined.
To do this, we need to use the balanced equation and the molar masses of the compounds involved.
The molar mass of nitroglycerin (C3H5N3O9) can be calculated as follows:
(3 x atomic mass of Carbon) + (5 x atomic mass of Hydrogen) + (3 x atomic mass of Nitrogen) + (9 x atomic mass of Oxygen)
Molar mass of C3H5N3O9 = (3 x 12.01 g/mol) + (5 x 1.01 g/mol) + (3 x 14.01 g/mol) + (9 x 16.00 g/mol)
Once you have calculated the molar mass of nitroglycerin, you can use this information to convert the mass of nitroglycerin given (239g) to moles.
Moles of nitroglycerin = Mass of nitroglycerin / Molar mass of nitroglycerin
Now, since the balanced equation shows the molar ratios between the reactant and products, we can use these ratios to find the moles of the gas products.
For example, in the balanced equation, we see that 1 mole of nitroglycerin produces 12 moles of CO2, 5 moles of N2, 2 moles of NO, and 10 moles of H2O.
To find the moles of each gas product, we multiply the moles of nitroglycerin by the corresponding stoichiometric coefficient from the balanced equation.
Now you have the moles of all the gas products combined.
Moving on to part C - using the ideal gas law to solve for the volume of the products of the explosion.
Before we can apply the ideal gas law (PV = nRT), we need to convert the given temperature from degrees Celsius to Kelvin.
To do this, you simply add 273.15 to the Celsius temperature.
Once you have the temperature in Kelvin, you can rearrange the ideal gas law equation to solve for volume (V).
V = (nRT) / P
Substitute the values of moles (from part B), temperature (in Kelvin), and pressure (1.00 atm) into the equation.
Calculate the volume using these values, and you will have your answer.
I hope this explanation helps you understand the steps involved in solving this problem. If you have any more questions, feel free to ask!