Question

help with # 7

Data Table: Reactant 1 Identity_NaCO,H,O 124.00 g/mol Mass 1.02 g Reactant 2 Identity_MnS0, H,0 169.02 g/mol Mass_1.04 g Observation of chemical reaction. Include observations about color of precipitate! Immediately after adding the two aqueous solutions together a pale pink precipitate formed. 1.49 g Mass of filter paper + precipitate Mass of filter paper Mass of precipitate (actual yield) 0.83 g 0.66 g Analysis: 1. Write the balanced chemical equation for this reaction. 2. Use a solubility table to determine the identity of the precipitate formed. Write the net ionic equation for this reaction. Calculate the theoretical amount of product that could be produced by each reactant. 5. Determine the limiting reactant. 6. Calculate the percent yield. (The amount of product produced by the limiting reactant is the theoretical yield of the precipitate.) What are the primary sources of experimental error in this experiment? 3. 4. 7. 9. Answer these questions: 8. When a balanced chemical equation is written, what chemistry law is demonstrated? Define 'reactant' and 'product' as related to a chemical reaction. 10. Explain the difference between the limiting reactant (reagent) in a chemical reaction and the excess reactant (reagent)' in a chemical reaction. Define 'yield' as related to a chemical reaction. Explain the difference between the actual yield in a chemical reaction and the theoretical yield of that chemical reaction. Define *precipitate' as related to a chemical reaction. Define "supernatant' as related to filtration. Submission: You do not need to print these pages. Please put all you responses neatly on a separate sheet 11. 12. 13. 14.

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Answers

8. Balanced chemical equation demonstrate law of conservation of mass.

9 reactants are on the left side of chemical equation and products are on the right side of chemical equations.

Example

A + B = C + D

A and B are reactant and C and D are product

Reactant react to form product.

Nature of reactant and product are different.

10. The reagents which are consumed completely in a reaction are called limiting reagents

The reagents which are left in excess after reaction is completed is called excess reagents.

Example

2H2 + O2 = 2H2O

Suppose we have one mole of 1 mole of H2

And 2 mole of O2 then H2 limiting reagent

and O2 is excess reagent.

Because 1 mole H2 react with 1/2 mole O2

So 3/2 mole O2 remain in excess

11. The amount of product obtained in a chemical reaction is called yeild of reaction.

In question no 10 1 mole H2O is formed so

Yeild is 1.

12. The actual yield is the quantity of a product that is obtained from a chemical reaction. In contrast, the calculated or theoretical yield is the amount of product that could be obtained from a reaction if all of the reactant converted to product.Theoretical yield is based on the limiting reactant

The actual yeild is generally less than theoretical yeild

For example if we obtained .8 mole H2O actually

In problem 10 then this is actual yeild

And 1 mole is theoretical yeild which is maximum.