You are given a crushed sample that is a mixture of limestone (calcium carbonate), lime (calcium...


You are given a crushed sample that is a mixture of limestone (calcium carbonate), lime (calcium oxide), and sand. The calcium carbonate, or limestone, is the only material present in the mixture that will decompose when heated. You subject a 6.0420 g sample of the mixture to strong heating and after the sample reaches constant mass (no more mass is lost with additional heating), the sample has a final weight of 3.9883 g.

What is the percentage of calcium carbonate present in the original mixture? (MW of calcium carbonate = 101.1 g/mol)

Equation for reaction = {eq}CaCO_{3}(s) \rightarrow CaO(s) + CO_{2}(g) {/eq}

Theoretical Yield:

The reaction yield of a product species in a chemical reaction, is its mass in grams formed from the consumption of a certain set of starting reactant quantities. If the reaction is assumed to proceed to completion and with no side reactions, then the reaction yield achieved is termed the product's theoretical yield. This value can be calculated and does not require experimentation. A known product theoretical yield can be used in a given reaction system to perform calculations going backwards. This means that you are trying to find the starting moles of a limiting reactant that was originally present, in order for this product theoretical yield to be formed.

Answer and Explanation: 1

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The only component of the mixture that decomposes is calcium carbonate, according to the given balanced equation:

{eq}\rm CaCO_{3}(s) \rightarrow...

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Learn more about this topic:

Calculating Reaction Yield and Percentage Yield from a Limiting Reactant


Chapter 9 / Lesson 6

How to calculate the theoretical yield? Learn the definition and formula of percent yield. Use the theoretical yield equation to calculate theoretical yield.

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