a) b) Rate of Reaction Concentration of Acid (mol dm³) Explain, using collision theory, why the student obtained these results, and state what they could conclude about the effect of changing concentration of acid on the rate of reaction between calcium carbonate and sulfuric acid. If the student had ground up the calcium carbonate chips into a powder and run the tests again, what would you expect to happen to the rate of reaction? Briefly explain why by applying collision theory. Part 2 The student ran the same experiment, but this time changed the temperature, increasing it by 10°C each time whilst keeping the concentration and all other factors constant. They found that as the temperature increased, so did the rate of reaction, as shown in the graph below. Rate of Reaction Temperature (°C) The student had seen a Maxwell-Boltzmann distribution curve such as the one below but was unsure about how it explained his results. a) Provide an answer for the student to explain how the Maxwell- Boltzmann curve can explain the trend the student found.
a) b) Rate of Reaction Concentration of Acid (mol dm³) Explain, using collision theory, why the student obtained these results, and state what they could conclude about the effect of changing concentration of acid on the rate of reaction between calcium carbonate and sulfuric acid. If the student had ground up the calcium carbonate chips into a powder and run the tests again, what would you expect to happen to the rate of reaction? Briefly explain why by applying collision theory. Part 2 The student ran the same experiment, but this time changed the temperature, increasing it by 10°C each time whilst keeping the concentration and all other factors constant. They found that as the temperature increased, so did the rate of reaction, as shown in the graph below. Rate of Reaction Temperature (°C) The student had seen a Maxwell-Boltzmann distribution curve such as the one below but was unsure about how it explained his results. a) Provide an answer for the student to explain how the Maxwell- Boltzmann curve can explain the trend the student found.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...
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Transcribed Image Text:Part 1
A student carried out an investigation to observe the effect of changing
concentration of sulfuric acid on the breakdown of calcium carbonate
(marble) chips. They changed the concentration of the acid between
each test but kept the size of the marble chips constant. The full equation
for the reaction and a graph of the overall results can be seen below.
CaCO3(s) + H₂SO4(aq) → CaSO4(aq) + CO2(g) + H₂O (1)
a)
b)
Rate of Reaction
*
Concentration of Acid (mol dm³)
Explain, using collision theory, why the student obtained
these results, and state what they could conclude about the
effect of changing concentration of acid on the rate of reaction
between calcium carbonate and sulfuric acid.
If the student had ground up the calcium carbonate chips into
a powder and run the tests again, what would you expect to
happen to the rate of reaction? Briefly explain why by
applying collision theory.
Part 2
The student ran the same experiment, but this time changed the
temperature, increasing it by 10°C each time whilst keeping the
concentration and all other factors constant. They found that as the
temperature increased, so did the rate of reaction, as shown in the graph
below.
Rate of Reaction
Temperature (°C)
The student had seen a Maxwell-Boltzmann distribution curve such
as the one below but was unsure about how it explained his results.
a) Provide an answer for the student to explain how the Maxwell-
Boltzmann curve can explain the trend the student found.
Number of Molecules with energy
T°C
T+10°C
Kinetic Energy
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