Asked by Daniel
If the rocket engine contains 1500.0 g of H2O2 and an excess of N2H4, what volume of water vapor will be produced when the rocket fires up to a temperature of 540oC and a pressure of 1.2 atm?
I honestly don't GET this thing, ugh =(
Please Help!!
I honestly don't GET this thing, ugh =(
Please Help!!
Answers
Answered by
DrBob222
It's just two problems in 1.
The first one is stoichiometry to find the moles of water vapor; the second part is to use PV = nRT to calcualte the volume
1. Write the equation for the reaction between H2O2 and N2H4. I assume that was done in the problem.
2. Convert g H2O2 to moles. Moles = grams/molar mass.
3. Using the coefficients in the balanced equation, convert moles H2O2 to moles H2O.
4. Now use PV = nRT to calculate volume. Don't forget to change C to Kelvin in the second equation. (K =- 273 + C).
The first one is stoichiometry to find the moles of water vapor; the second part is to use PV = nRT to calcualte the volume
1. Write the equation for the reaction between H2O2 and N2H4. I assume that was done in the problem.
2. Convert g H2O2 to moles. Moles = grams/molar mass.
3. Using the coefficients in the balanced equation, convert moles H2O2 to moles H2O.
4. Now use PV = nRT to calculate volume. Don't forget to change C to Kelvin in the second equation. (K =- 273 + C).
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