Question

What measurement should be the sum of the mass of excess reactant that remains unreacted and...

What measurement should be the sum of the mass of excess reactant that remains unreacted and the theoretical yield of KCL based on limiting reagent?

Homework Answers

Answer #1
Following steps can be followed for obtaining the mass of excess reactant and theoretical yield
  1. Write the chemical equation.
  2. Calculate the moles of product from the first reactant.
  3. Calculate the moles of product from the second reactant.
  4. Identify the limiting reactant and the excess reactant.
  5. Calculate the mass of excess reactant used up.
  6. Calculate the mass of unused excess reactant.By performing these steps we can easily obtain the mass of excess reactant that remain unreacted.

And theoretical yield is the amount of product formed by the corresponding amount of limiting reactant. hence simply find the amount of product that can be obtained for the given limiting reactant with the help of balanced chemical equation.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
I am stuck at calculating mass of excess reactant used up in the reaction and mass...
I am stuck at calculating mass of excess reactant used up in the reaction and mass of excess reactant left over after the reaction 2Na3PO4*12H2O + 3Ba Cl*2H2O --> Ba3(PO4)2 + 6NaCl + 30H2O I got mass of precipitate : 0.063 Initial Mass of salt mixture 0.063 Moles of Ba3(PO4)2 precipitated: 1.04*10^-4 Moles of limiting reactant in the sal mixture : 3.14x10^-4 Mass of Limiting reactant in the salt Mixture :0.077 g Mass of excess reactant in the salt mixture...
Consider the reaction:   2 H2 + O2   → 2 H2O What if 3.0 mol H2 and...
Consider the reaction:   2 H2 + O2   → 2 H2O What if 3.0 mol H2 and 2.0 mol O2 were allowed react. The limiting reactant is ______. Complete consumption of the limiting reactant would mean the consumption of _____ mol of the other reactant; _____ mol of excess reactant would remain unreacted if the reaction went to completion. The theoretical yield is ____ mol or ____ g of _____. What if only 2.85 mol of product was obtained? Then, we...
How do you determine which reactant in a reaction remains in excess and how do you...
How do you determine which reactant in a reaction remains in excess and how do you determine that reactant's mass?
A 2.50 kg sample of ammonia is mixed with 2.65 kg of oxygen. A. Balance the...
A 2.50 kg sample of ammonia is mixed with 2.65 kg of oxygen. A. Balance the equation below. ____ NH3(g) + ____ O2(g)  ____ NO(g) + ____ H2O(g) B. Which is the limiting reagent? C. How much excess reactant remains on completion of the reaction? D. What is the theoretical yield of NO? E. 1.45 kg of NO are produced what is the percent yield of NO?
Determine the theorical yield (in grams) of strontium sulfate. What is your limiting reactant and excess...
Determine the theorical yield (in grams) of strontium sulfate. What is your limiting reactant and excess reactant? given 2.27×10^-3 mol Na2SO4 and 2.5×10^-3 mol SrCl2
A reaction vessel contains 8.00g NaCl and 8.00g H2SO4. a.) What is the limiting reactant b.)...
A reaction vessel contains 8.00g NaCl and 8.00g H2SO4. a.) What is the limiting reactant b.) How many grams of HCl was produced c.) How many grams of excess reactant are left unreacted/unconsumed
You are provided with 5.72 g  SO2 to react with 2.04 g  O2. Indicate your theoretical yield by...
You are provided with 5.72 g  SO2 to react with 2.04 g  O2. Indicate your theoretical yield by completing the following statements. Match the chemical formulas and amounts in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer. 0.61 g 0.0893 0.1275 0.02 g 10.2 g 7.15 g 1.43 g SO3 SO2 O2 0.0638 The limiting reagent in the reaction is______ . Regarding the theoretical yield based on...
For each of the following unbalanced reactions, suppose 5.18 g of each reactant is taken. Determine...
For each of the following unbalanced reactions, suppose 5.18 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent(s) will remain after the limiting reactant is consumed. a) CaC2(s) + H2O(l) → Ca(OH)2(s) + C2H2(g) b) NaCl(s) + H2SO4(l) → HCl(g) + Na2SO4(s) c) SiO2(s) + C(s) → Si + CO(g)
For each of the following unbalanced reactions, suppose 4.85 g of each reactant is taken. Determine...
For each of the following unbalanced reactions, suppose 4.85 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent(s) will remain after the limiting reactant is consumed. (Select all that apply.) 1. CaC2(s) + H2O(l) → Ca(OH)2(s) + C2H2(g) 2.NaCl(s) + H2SO4(l) → HCl(g) + Na2SO4(s) 3.SiO2(s) + C(s) → Si + CO(g)
What mass of which reagent is left unreacted?Hydrogen peroxide is used as a cleaning agent in...
What mass of which reagent is left unreacted?Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes upon contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams upon contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the action of...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT