Rate of reaction：练习题

Which change will increase the rate of reaction between marble chips (calcium carbonate) and dilute hydrochloric acid?

What is the effect of adding a catalyst to a chemical reaction?

The reaction \(N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)\) is carried out in a closed container. If the volume of the container is halved while keeping the temperature constant, what happens to the rate of reaction?

A student reacts excess zinc with dilute \(HCl\). The volume of hydrogen gas produced is recorded over time and plotted on a graph. Which change results in a steeper initial gradient on the graph but the same final volume of gas?

How does a \(10^{\circ}C\) increase in temperature affect the particles in a reaction mixture?

State what happens to the mass and chemical properties of a catalyst at the end of a chemical reaction.

When marble chips (\(CaCO_3\)) react with dilute hydrochloric acid (\(HCl\)) in an open conical flask, the mass of the flask and its contents decreases over time. Identify the product responsible for this change and explain why the mass decreases.

Explain, using collision theory, why an increase in temperature increases the rate of a chemical reaction.

The reaction between marble chips (calcium carbonate) and dilute hydrochloric acid is used to study the rate of reaction. The equation is:

\(\text{CaCO}_3\text{(s)} + 2\text{HCl(aq)} \rightarrow \text{CaCl}_2\text{(aq)} + \text{H}_2\text{O(l)} + \text{CO}_2\text{(g)}\)

A student performs the experiment twice. In the first experiment, large marble chips are used. In the second experiment, the same mass of marble is used, but in the form of small chips.

(a) Describe a practical method to measure the rate of this reaction by collecting the gas.
(b) Predict and explain how the rate of reaction changes when using small chips instead of large chips.
(c) Explain your prediction in part (b) using collision theory.

A student investigates the effect of temperature on the rate of reaction between sodium thiosulfate (\(\text{Na}_2\text{S}_2\text{O}_3\)) and hydrochloric acid. The reaction produces a sulfur precipitate which makes the solution cloudy.

(a) State the word equation for this reaction.
(b) Describe how the student can determine the rate of reaction using a piece of paper with a cross marked on it.
(c) Using collision theory, explain why the rate of reaction increases significantly with a small increase in temperature. Refer to kinetic energy and activation energy in your answer.