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General Chemistry

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Chemical Reactions

Question
13 out of 15
 

Passage 1

Information regarding the amounts of substances that actually react to form the products are of extreme help. Analyzing reactions and having the balanced equations help chemists to determine the correct and optimum proportions of reactants to be used. There are various other factors besides the amount of reactants, which determine the efficiency of reactions.

Experiment 1

Student 1 used 40.5 g of aluminum and 80 g of Fe2O3 for Reaction I. A second student conducted the same reaction with a different amount for one of the reactants. The second student used 40.5 g of aluminum, and 90 grams of Fe2O3. A third student also conducted the same reaction with 54 g of aluminum and the same amount of Fe2O3 used by the first student.

Experiment 2

Reaction II involved the production of Al2O3 from aluminum hydroxide This was done by heating aluminum hydroxide.


Experiment 3


Roughly 80 g of Fe2O3 was present in Experiment 3, and upon completion of the reaction, it was measured that 22 g of CO2 was formed. If this is true, how much CO must have reacted before reaching completion of the reaction?

A 14 grams
B 28 grams
C 56 grams
D 84 grams

Ans. A In the question, we are given that 80 g of Fe2O3 is used in the reaction mixture. How much of this actually reacted is another story. That is to be found out from the yield data. The amount of CO2 produced is 22 g. Based on the balanced equation, we can infer that for every 3 moles of CO reacted, 3 moles of CO2 are produced. So CO and CO2 have a 1:1 ratio. If 22 g or 0.5 moles of CO2 is produced, 0.5 moles of CO must have reacted.

Chemical Reactions Flashcard List

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