2H2 + O2 ==> 2H2O
This may be solved the usual stoichiometric way by changing g H2 and g O2 to mols, determining which is the limiting reagent, etc etc. OR, the shortcut way is to simply use volumes since all are gases. If you don't get this way, I can explain how it works in detail. Let me know.
To use volumes only, 725 mL H2 will form 725 mL H2O since the ratio of H2 to H2O is 2:2 (or 1:1). 325 mL O2 will form 325 x (2 mols H2O/1 mol O2) = 650 mL H2O. Therefore, 650 mL H2O will be the final product (O2 is the limiting reagent). There will be excess H2 remaining unreacted.
For #2, write the equation and balance it.
C3H8 + 5O2 ==> 3CO2 + 4H2O
Convert 10 g propane to mols. #mols = grams/molar mass propane.
Convert mols Propane to mols O2 using the coefficients in the balanced equation.
Use PV = nRT to convert mols O2 to volume O2 at the conditions cited.
Convert to volume of air by the following:
volume oxygen at cited conditions/0.21 = volume air.
Post your work if you get stuck or if you have any questions.
Assuming the volumes of all gases in the reaction are measured at the same temperature and pressure, calculate the volume of water vapor obtainable by the explosive reaction of a mixture of 725mL of hydrogen gas and 325mL of oxygen gas.
andd...
Calculate the volume of air at 30 degrees C and 1.00atm that is needed to burn completely 10.0 grams of propane. Assume that air is 21.0% oxygen (O2) by volume.
2 answers
another question...
I have a problem that states:
Find the pressure of a sample of carbon tetrachloride, CCl4 if 1.00 mol occupies 35.0L at 77.0 degress C (slightly above its normal boiling point). Assume that CCl4 obeys (a) the ideal gas law; (b) the van der Waals equation. The van der Waals constants for CCl4 are a= 20.39(L^2)(atm)/mol^2 and b= 0.1383L/mol.
I tried to do the problems and the answers I got are (a)=.814atm and (b)=.800atm but the back of the book is telling me that (a)=0.821atm an (b)=0.805. I'm not sure if i'm wrong or if the book is off.
I have a problem that states:
Find the pressure of a sample of carbon tetrachloride, CCl4 if 1.00 mol occupies 35.0L at 77.0 degress C (slightly above its normal boiling point). Assume that CCl4 obeys (a) the ideal gas law; (b) the van der Waals equation. The van der Waals constants for CCl4 are a= 20.39(L^2)(atm)/mol^2 and b= 0.1383L/mol.
I tried to do the problems and the answers I got are (a)=.814atm and (b)=.800atm but the back of the book is telling me that (a)=0.821atm an (b)=0.805. I'm not sure if i'm wrong or if the book is off.