2. If, in another student's reaction, all of the Al(OH)3 did not dissolve but remained in the beakerand ended up on the filter paper, will the student's percentage yield be higher or lower than itwould have been if all of the Al(OH)3had dissolved? Explain your answer.

All of the Al(OH)3 did not dissolve but remained in the beaker and ended up on filter paper, will…

Answered: 2. If, in another student's reaction,…

Living By Chemistry: First Edition Textbook

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ISBN:9781559539418

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ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

SectionU6.2: How Backward: Reversible Reactions

Problem 7E

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I2 (aq) + CH3COCH3 (aq)  HI (aq) + ICH2COCH3 (aq)Iodine in solution has a yellow-brown color, whereas the acetone and both products are colorless. This means that we can run the reaction using iodine as the limiting reagent, and when we see that the yellow-brown color of the iodine has disappeared, we know that the reaction has stopped and all of the iodine has been consumed. Recall that to calculate a rate of reaction, we would like toknow the change in concentration of a reactant or product during a fixed amount of time. Wewill choose the reactant iodine in this case, because its brown color allows us to determinewhen its concentration has fallen to zero. Rate = –Δ[I2] / Δt = – ([I2]final – [I2]initial) / ([tfinal – tinitial) = – (0 – [I2]initial) / (tfinal – 0) = [I2]initial / tfinal Run several trials at different concentrations of reactants and use themethod of initial rates to obtain values for k, x, y, and z in the rate law. Rate = k [I2]x [acetone]y [H+]z Run the…
I2 (aq) + CH3COCH3 (aq)  HI (aq) + ICH2COCH3 (aq)Iodine in solution has a yellow-brown color, whereas the acetone and both products are colorless. This means that we can run the reaction using iodine as the limiting reagent, and when we see that the yellow-brown color of the iodine has disappeared, we know that the reaction has stopped and all of the iodine has been consumed. Recall that to calculate a rate of reaction, we would like toknow the change in concentration of a reactant or product during a fixed amount of time. Wewill choose the reactant iodine in this case, because its brown color allows us to determinewhen its concentration has fallen to zero. Rate = –Δ[I2] / Δt = – ([I2]final – [I2]initial) / ([tfinal – tinitial) = – (0 – [I2]initial) / (tfinal – 0) = [I2]initial / tfinal Run several trials at different concentrations of reactants and use themethod of initial rates to obtain values for k, x, y, and z in the rate law. Rate = k [I2]x [acetone]y [H+]z Run the…
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2. If, in another student's reaction, all of the Al(OH)3 did not dissolve but remained in the beaker and ended up on the filter paper, will the student's percentage yield be higher or lower than it would have been if all of the Al(OH)3 had dissolved? Explain your answer.