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Chapter 7: Problem 76

A chemical reaction produces less than the expected amount of product. Is this result a violation of the law of conservation of mass?

Short Answer

Expert verified
Explain your answer. Answer: No, a chemical reaction producing less than the expected amount of product is not necessarily a violation of the law of conservation of mass. The discrepancy in the product amount might be due to incomplete reactions, side reactions, or experimental errors. To determine if there is a violation, it's essential to compare the total mass of reactants and products and investigate any potential factors affecting the reaction.

Step by step solution

01

1. Understand the Law of Conservation of Mass

The law of conservation of mass states that the total mass of the reactants in a chemical reaction must equal the total mass of the products. In other words, mass cannot be created or destroyed; it can only change forms.
02

2. Examine the Chemical Reaction

The given exercise states that a chemical reaction produces less than the expected amount of product. This means that the mass of the products is less than what we anticipated based on the balanced chemical equation.
03

3. Identify Possible Reasons for the Lower Amount of Product

There could be various reasons why the reaction produced less product than expected, such as an incomplete reaction, side reactions, or loss of reactants or products during the process due to human errors or equipment inefficiencies. It's important to consider these factors when evaluating the observed results.
04

4. Determine if There is a Violation of the Law of Conservation of Mass

The occurrence of producing less product than expected does not automatically mean that there is a violation of the law of conservation of mass. To determine if the law is violated, we need to consider the total mass of reactants and products. If the total mass is conserved, as expected, then there is no violation of the law. Otherwise, we have to investigate the factors mentioned in step 3 to understand the discrepancy in mass conservation.
05

5. Conclusion

While producing less than the expected amount of product may raise questions, it does not necessarily indicate a violation of the law of conservation of mass. The mass discrepancy might be related to various factors, such as incomplete reactions, side reactions, or experimental errors. To draw a conclusion, one should compare the total mass of reactants and products and investigate potential factors affecting the reaction.

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Most popular questions from this chapter

Balance the following reactions for the formation of nitrogen compounds: a. \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{NO}(g)\) b. \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{N}_{2} \mathrm{O}(g)\) c. \(\mathrm{NO}(g)+\mathrm{NO}_{3}(g) \rightarrow \mathrm{NO}_{2}(g)\) d. \(\mathrm{NO}(g)+\mathrm{O}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{HNO}_{2}(\ell)\)

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Phosgenite, a lead compound with the formula \(\mathrm{Pb}_{2} \mathrm{Cl}_{2} \mathrm{CO}_{3}\) is found in Egyptian cosmetics. Phosgenite was prepared by the reaction of \(\mathrm{PbO}, \mathrm{NaCl},\) and \(\mathrm{CO}_{2} .\) An unbalanced expression of the reactant mixture is $$\mathrm{PbO}(s)+\mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(g) \rightarrow $$ $$\quad\quad\quad\quad\quad \mathrm{Pb}_{2} \mathrm{Cl}_{2} \mathrm{CO}_{3}(s)+\mathrm{NaOH}(a q)$$ a. Balance the equation. b. How many grams of phosgenite can be obtained from \(10.0 \mathrm{g} \mathrm{PbO}\) and \(10.0 \mathrm{g} \mathrm{NaCl}\) in the presence of excess water and \(\mathrm{CO}_{2} ?\) c. Phosgenite can be considered a mixture of two lead compounds. Which compounds appear to be combined to make phosgenite?

Do the empirical and molecular formulas of a compound have the same percent composition values?

A reaction vessel contains \(10.0 \mathrm{g} \mathrm{CO}\) and \(10.0 \mathrm{g} \mathrm{O}_{2},\) which combine to form \(\mathrm{CO}_{2}\) : $$2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g)$$ a. Which reactant is limiting? b. How many grams of \(\mathrm{CO}_{2}\) could be produced? c. How many grams of the nonlimiting reactant are left over?
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