Explore BrainMass
Share

Limiting reactants in stoichiometry and percent yield.

This content was STOLEN from BrainMass.com - View the original, and get the already-completed solution here!

Use the following equation:
H2SO4 + Al produces Al2(SO4)3 + H2
Given this information: 350.00 mL of 6.00 M H2SO4 reacts with 10.00 grams of Al. This collects 13.55 L of H2. What is the percent yield of the reaction?

© BrainMass Inc. brainmass.com October 16, 2018, 4:10 pm ad1c9bdddf
https://brainmass.com/chemistry/reaction-stoichiometry/16010

Solution Preview

In solving this problem, the first thing you need to do is balance the presented equation, such that there are equimolar quantities of reagents and products, thus:

H2SO4 + Al produces Al2(SO4)3 + H2

is balanced to give:

3H2SO4 + 2Al produces Al2(SO4)3 + 3H2

since the product Al2(SO4)3 contains 2xAl and 3xSO4 (ie 3xH2SO4 are required). In turn, 3xH2SO4 will produce 3xH2.

If we use 350ml of 6M H2SO4, the number of moles of H2SO4 is equal ...

Solution Summary

The ideal gas equation states that pV=nRT.

p=pressure
V=volume
n=number of moles
R=ideal gas constant
T=Temperature

$2.19
Similar Posting

Chemical Reactions and Stoichiometry Problems

Please assist with answering the following questions. I'd love to be able to see a step to step process for solving these, that way when I come across problems similar to this in the future and then, I don't get lost again.

1. 2Mn02 + 4KOH + O2 + CL2 ---> 2KMnO4 + 2KCL + 2H2O
For the reaction above, there is 100.0 g of each reactant available. Which reagent is the limiting reagent?

2. The reaction of 7.8 g of benzene (C6H6) with excess nitric acid resulted in 0.90 g of H2O. What is the percentage yield?
Molar mass (g/mol): C6H6=78, HNO3=63, C6H5NO2=123, H2O=18
C6H6 + HNO3 ----> C6H5NO2 + H2O

3. 6H+ + 5H2O + 2MnO4- ----> 5O2 + 2Mn2+ + 8H2O
According to the balanced equation above, how many moles of permanganate ion are required to react completely with 25.0 ml of .100 M hydrogen peroxide?

4. How many grams of water will be formed when 32.0 g of hydrogen is allowed to react with 16.0 g of oxygen according to the following reaction:
2H2 + O2 = 2H2O

5. What mass of Aluminum is produced when 0.5 mole of Al2S3 is completely reduced with excess H2?

View Full Posting Details