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17 Nov 2019
A student studying the decomposition of hydrogen peroxide noticed that the rate at which oxygen gas collected was noticably slower after the reaction had been running for several minutes than it was when the reaction was first started. Select the best answer from the list of statements. The lower rate of oxygen collection is likely due to an error in making the measurement. There is no reason for the rate to be different than it was at the beginning of the reaction. After the reaction has been running for several minutes the concentration of hydrogen peroxide will be lower because it is being decomposed. This lower concentration is the reason the rate of oxygen production is slower. The lower rate of oxygen collection is likely due to a change in atmospheric pressure during the experiment. Oxygen is a gas and the volume of a gas depends on atmospheric pressure. After the reaction has been running for several minutes the concentration of the catalyst will be lower because it is being used up. This lower concentration is the reason the rate of oxygen production is slower. Match the chemical with the statement that best describes the observed change in the rate of the reaction when the concentration of that chemical was changed. the H_2O_2 concentration is doubled the rate of oxygen collected is approximately half as fast the KCl concentration is doubled the rate of oxygen collected is approximately four times faster the Kl concentration is doubled the rate of oxygen collected is approximately twice as fast the Fecl_3 concentration is doubled the rate of oxygen collected is approximately four times slower there is little or no effect on the rate of oxygen collection Select the statement that describes the relationship between the rate of a reaction and the length of time needed to produce a given quantity of a product of the reaction. The time required to produce a given quantity of a product is directly proportional to the rate of the reaction. For a reaction that runs twice as fast, the given quantity of product will be produced in twice the time. The time required to produce a given quantity of a product is inversely proportional to the rate of the reaction. For a reaction that runs twice as fast, the given quantity of product will be produced in half the time. There is a relationship between the rate of a reaction and the time required to produce a given quantity of a product. It is not possible to know what that relationship is without running experiments. There is no relationship between the rate of the reaction and the time required to produce a given amount of product.
A student studying the decomposition of hydrogen peroxide noticed that the rate at which oxygen gas collected was noticably slower after the reaction had been running for several minutes than it was when the reaction was first started. Select the best answer from the list of statements. The lower rate of oxygen collection is likely due to an error in making the measurement. There is no reason for the rate to be different than it was at the beginning of the reaction. After the reaction has been running for several minutes the concentration of hydrogen peroxide will be lower because it is being decomposed. This lower concentration is the reason the rate of oxygen production is slower. The lower rate of oxygen collection is likely due to a change in atmospheric pressure during the experiment. Oxygen is a gas and the volume of a gas depends on atmospheric pressure. After the reaction has been running for several minutes the concentration of the catalyst will be lower because it is being used up. This lower concentration is the reason the rate of oxygen production is slower. Match the chemical with the statement that best describes the observed change in the rate of the reaction when the concentration of that chemical was changed. the H_2O_2 concentration is doubled the rate of oxygen collected is approximately half as fast the KCl concentration is doubled the rate of oxygen collected is approximately four times faster the Kl concentration is doubled the rate of oxygen collected is approximately twice as fast the Fecl_3 concentration is doubled the rate of oxygen collected is approximately four times slower there is little or no effect on the rate of oxygen collection Select the statement that describes the relationship between the rate of a reaction and the length of time needed to produce a given quantity of a product of the reaction. The time required to produce a given quantity of a product is directly proportional to the rate of the reaction. For a reaction that runs twice as fast, the given quantity of product will be produced in twice the time. The time required to produce a given quantity of a product is inversely proportional to the rate of the reaction. For a reaction that runs twice as fast, the given quantity of product will be produced in half the time. There is a relationship between the rate of a reaction and the time required to produce a given quantity of a product. It is not possible to know what that relationship is without running experiments. There is no relationship between the rate of the reaction and the time required to produce a given amount of product.
Keith LeannonLv2
7 Jun 2019