CHEM 101 Lecture Notes - Lecture 6: Reagent, Molar Mass, Sodium Hydroxide

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coffeegoat117

21 Mar 2016

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This experiment was conducted in order to determine how the ratio of reactants determines the ratio of products using stoichiometry. Stoichiometry was used to determine how many moles of each reactant are needed to force at least one of the reactants to be completely used up in the reaction. This experiment was done by using one reactant as a limiting reagent and the other reactant as an excess reagent. Theoretical yield was used to determine about how many moles it would take to force the reaction to completion and was calculated by balancing the chemical equation for the reaction. The percent yield was determined by how much was actually yielded in comparison to how much was theoretically yielded in order to determine the accuracy of the experiment. The calculations that were performed were in order to determine how much. Ca(oh)2 could possibly be formed in the reaction.

Related Questions

A weighed sample of iron (Fe) is added to liquid bromine (Br₂) and allowed to react completely. The reaction produces a single product which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below).

(a) What mass of Br₂ is used when the reaction consumes 2.0 g of Fe?

(b) What is the mole ratio of Br₂ to Fe in the reaction?

(d) Write the balanced chemical equation for the reaction of iron and bromine.

(e) What is the name of the reaction product?

(f) Which statement of statements best describe the experiments summarized by the graph?

(i) When 1.00 g of Fe is added to the Br₂, Fe is the limiting reagent.

(ii) When 3.50 g of Fe is added to the Br₂, there is an excess of Br₂.

(iii) When 2.50 g of Fe is added to the Br₂, both reactants are used up completely.

(iv) When 2.00 g of Fe is added to the Br₂, 10.8 g of product is formed. The percent yield must therefore be 20.0%

salmonjellyfish398

A weighed sample of iron (Fe) is added to liquid bromine (Br₂) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below).

(a) What mass of Br₂ is used when the reaction consumes 2.0 g of Fe?

(b) What is the mole ratio of Br₂ to Fe in the reaction?

(d) Write the balanced chemical equation for the reaction of iron and bromine.

(e) What is the name of the reaction product?

(f) Which statement or statements best describe the experiments summarized by the graph?

(i) When 1.00 g of Fe is added to the Br₂, Fe is the limiting reagent.

(ii) When 3.50 g of Fe is added to the Br₂, there is an excess of Br₂.

(iii) When 2.50 g of Fe is added to the Br₂, both reactants are used up completely.

(iv) When 2.00 g of Fe is added to the Br₂, 10.8 g of product is formed. The percent yield must therefore be 20.0%.

jadegiraffe875

Chemistry Help: Very Bottom of Page are the questions and thedata is above the Data Analysis Questions #1 #2 #3 #4 ? Help pleaseshow work so I could understand how you solved the questions.

CHEM 101 Lecture Notes - Lecture 6: Reagent, Molar Mass, Sodium Hydroxide

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