Question

Given the following chemical reaction 4Al(s) + 3O2(g)=2Al2O3(s). If 10.0grams of Al and 19.0gram of O2...

Given the following chemical reaction 4Al(s) + 3O2(g)=2Al2O3(s). If 10.0grams of Al and 19.0gram of O2 are mixed together how many moles of each reactants you have.

b) how many moles of the product you will form

c) which of these two reactant is the limiting reactant

d) what is the theoritical yield of this reaction (in gram)

e) If 15.0grams of Al2O3 was obtained, what is the percent yield of this reaction.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Using this reaction: 4Al(s) + 3O2(g) ----> 2Al2O3(s) a. Determine the limiting reactant and the maximum...
Using this reaction: 4Al(s) + 3O2(g) ----> 2Al2O3(s) a. Determine the limiting reactant and the maximum yield if 4.70g Al reacts with 5.00L of O2 at STP. ( I got Al as the limiting reactant and the maximum yield of .087mol.) b. If the actual yield is 8.03 grams, what is the % yield. ( I got 90.4%) Did I do these right?
Aluminum oxide is synthesized according to the following reaction: 4Al + 3O2 → 2Al2O3 If 60.72...
Aluminum oxide is synthesized according to the following reaction: 4Al + 3O2 → 2Al2O3 If 60.72 g of aluminum oxide was formed from 40.81 g oxygen and 50.37 g of aluminum. What is the limiting reactant? What is the theoretical yield? What is the percent yield? Limiting reactant = _____________ Theoretical yield= ______________ Percent yield= _________________
Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s) What volume of O2...
Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s) What volume of O2 gas (in L), measured at 783 mmHg and 33 ∘C, is required to completely react with 52.1 g of Al?
For the reaction, calculate how many moles of the product form when 0.046 mol of O2...
For the reaction, calculate how many moles of the product form when 0.046 mol of O2 completely reacts. Assume that there is more than enough of the other reactant. 2Ca(s)+O2(g)→2CaO(s) For the reaction, calculate how many moles of the product form when 0.018 mol of O2 completely reacts. Assume that there is more than enough of the other reactant. 4Fe(s)+3O2(g)→2Fe2O3(s) For the reaction, calculate how many moles of the product form when 0.044 mol of K completely reacts. Assume that...
For the reaction shown, find the limiting reactant for each of the following initial amounts of...
For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants. 4Al(s)+3O2(g)→2Al2O3(s) 16 mol Al, 13 mol O2 11.4 mol Al, 9.5 mol O2 4 mol Al, 2.6 mol O2 1 mol Al, 1 mol O2 Can you please explain how to figure this out?
(10) Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s). Part A What...
(10) Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s). Part A What volume of O2 gas (in L), measured at 778 mmHg and 19 ∘C, is required to completely react with 53.3 g of Al? Part B Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)→CO(g)+3H2(g) In a particular reaction, 26.0 L of methane gas (measured at a pressure of 732 torr and...
For the oxidation-reduction reaction equation given here, 4Al + 3O2 --> 2Al2O3 indicate how many electrons...
For the oxidation-reduction reaction equation given here, 4Al + 3O2 --> 2Al2O3 indicate how many electrons are transferred in the formation of 1 formula unit of product. _ _ _ _ _ _
Consider the reaction: 4Al + 3MnO2 è 3Mn + 2Al2O3. if 22 grams of Al react...
Consider the reaction: 4Al + 3MnO2 è 3Mn + 2Al2O3. if 22 grams of Al react with 13 grams of manganese (IV) oxide, how much excess reactant remains aRer the reac/on has run to completion?
Consider the balanced chemical reaction shown below. 4 PH3(g) + 8 O2(g) 6 H2O(l) + 1...
Consider the balanced chemical reaction shown below. 4 PH3(g) + 8 O2(g) 6 H2O(l) + 1 P4O10(s) In a certain experiment, 3.118 g of PH3(g) reacts with 6.294 g of O2(g). (a) Which is the limiting reactant? (Example: type PH3 for PH3(g)) is the limiting reactant. (b) How many grams of H2O(l) form? g of H2O(l) form. (c) How many grams of P4O10(s) form? g of P4O10(s) form. (d) How many grams of the excess reactant remains after the limiting...
1. Given the following reaction     2C2H6(l)   +      7 O2(g)   ®           4CO2(g)      +     
1. Given the following reaction     2C2H6(l)   +      7 O2(g)   ®           4CO2(g)      +        6H2O(l) How many moles of water are produced when 4.5 moles of oxygen react?        (Hint: Use slides 5-8) 2. Given: I2     +    3 F2      ®     2 IF3 How many moles of I2 are needed to form 3 moles of IF3? How many moles of F2 are needed to form 10 moles of IF3? How many moles of I2 are needed to react with 3.5 moles of F2?        ...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT