Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows: CaCO 3 ( s ) + 2 HCl ( aq ) → CaCl 2 ( aq ) + CO 2 ( g ) + H 2 O ( l ) Describe a laboratory method that could be used to investigate the rate of the reaction.

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows: CaCO 3 ( s ) + 2 HCl ( aq ) → CaCl 2 ( aq ) + CO 2 ( g ) + H 2 O ( l ) For a reaction involving a solid reactant or catalyst, the greater is the surface area, the faster is the reaction. Place the marble in the flask and add the acid. Quickly plug the flask with cotton wool to stop any liquid splashing out. Then weigh it, starting the clock at the same time. Note the mass at regular intervals until the reaction is complete. Carbon dioxide is a heavy gas. It escapes through the cotton wool, which means that the flask gets lighter as the reaction proceeds. So by weighing the flask at regular intervals, you can follow the rate of reaction.

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows: CaCO 3 ( s ) + 2 HCl ( aq ) → CaCl 2 ( aq ) + CO 2 ( g ) + H 2 O ( l ) Describe a laboratory method that could be used to investigate the rate of the reaction.

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows: CaCO 3 ( s ) + 2 HCl ( aq ) → CaCl 2 ( aq ) + CO 2 ( g ) + H 2 O ( l ) For a reaction involving a solid reactant or catalyst, the greater is the surface area, the faster is the reaction. Place the marble in the flask and add the acid. Quickly plug the flask with cotton wool to stop any liquid splashing out. Then weigh it, starting the clock at the same time. Note the mass at regular intervals until the reaction is complete. Carbon dioxide is a heavy gas. It escapes through the cotton wool, which means that the flask gets lighter as the reaction proceeds. So by weighing the flask at regular intervals, you can follow the rate of reaction.

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows: CaCO 3 ( s ) + 2 HCl ( aq ) → CaCl 2 ( aq ) + CO 2 ( g ) + H 2 O ( l ) How will this affect the rate of the reaction on increasing the temperature.

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows: CaCO 3 ( s ) + 2 HCl ( aq ) → CaCl 2 ( aq ) + CO 2 ( g ) + H 2 O ( l ) The rate of a reaction can be defined as the change in concentration of reactant or a product in unit time. Most of the chemical reactions are accelerated by increase in temperature. Thus, the rate of reaction increases with increase in temperature.

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows: CaCO 3 ( s ) + 2 HCl ( aq ) → CaCl 2 ( aq ) + CO 2 ( g ) + H 2 O ( l ) How will this affect the rate of the reaction on adding water to the acid.

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows: CaCO 3 ( s ) + 2 HCl ( aq ) → CaCl 2 ( aq ) + CO 2 ( g ) + H 2 O ( l ) Rate of reaction depends upon the experimental conditions such as concentration of reactants (pressure in case of gases), temperature and catalyst. The rate of the reaction decreases on adding water to the acid.

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows: CaCO 3 ( s ) + 2 HCl ( aq ) → CaCl 2 ( aq ) + CO 2 ( g ) + H 2 O ( l ) If the lumps of marble are crushed first, will the reaction rate change? Explain your answer.

The rate of a reaction increases, as the surface area of a solid reactant is increased. When we use crushed marble chips the size of the chips decreases there by increase in the surface area of reactant and, the more surface area that is available for reacting particles to collide, the faster the reaction will occur.

EASY

Upper Secondary: IGCSE

IMPORTANT

Earn 100

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows:

${CaCO}_{3} (s) + 2 HCl (aq) \to {CaCl}_{2} (aq) + {CO}_{2} (g) + H_{2} O (l)$

Describe a laboratory method that could be used to investigate the rate of the reaction.

Important Questions on The Speed of a Reaction

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 10 - The Speed of a Reaction>Checkup on Chapter 10>Q 6

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows:

${CaCO}_{3} (s) + 2 HCl (aq) \to {CaCl}_{2} (aq) + {CO}_{2} (g) + H_{2} O (l)$

How will this affect the rate of the reaction on increasing the temperature.

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 10 - The Speed of a Reaction>Checkup on Chapter 10>Q 6

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows:

${CaCO}_{3} (s) + 2 HCl (aq) \to {CaCl}_{2} (aq) + {CO}_{2} (g) + H_{2} O (l)$

How will this affect the rate of the reaction on adding water to the acid.

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 10 - The Speed of a Reaction>Checkup on Chapter 10>Q 6

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows:

${CaCO}_{3} (s) + 2 HCl (aq) \to {CaCl}_{2} (aq) + {CO}_{2} (g) + H_{2} O (l)$

Explain each of the effects in increasing the temperature and adding water to the acid in terms of collisions between reacting particles.

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 10 - The Speed of a Reaction>Checkup on Chapter 10>Q 6

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows:

${CaCO}_{3} (s) + 2 HCl (aq) \to {CaCl}_{2} (aq) + {CO}_{2} (g) + H_{2} O (l)$

If the lumps of marble are crushed first, will the reaction rate change? Explain your answer.

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 10 - The Speed of a Reaction>Checkup on Chapter 10>Q 7

Zinc and iodine solution react like this:

$Zn (s) + I_{2} (aq) \to {ZnI}_{2} (aq)$

The rate of reaction can be followed by measuring the mass of zinc metal at regular intervals, until all the iodine has been used up.

What will happen to the mass of the zinc, as the reaction proceeds?

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 10 - The Speed of a Reaction>Checkup on Chapter 10>Q 7

Zinc and iodine solution react like this:

$Zn (s) + I_{2} (aq) \to {ZnI}_{2} (aq)$

The rate of reaction can be followed by measuring the mass of zinc metal at regular intervals, until all the iodine has been used up.

Which reactant is in excess? Explain your choice.

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 10 - The Speed of a Reaction>Checkup on Chapter 10>Q 7

Zinc and iodine solution react like this:

$Zn (s) + I_{2} (aq) \to {ZnI}_{2} (aq)$

The rate of reaction can be followed by measuring the mass of zinc metal at regular intervals, until all the iodine has been used up.

The reaction rate slows down with time. Why?

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 10 - The Speed of a Reaction>Checkup on Chapter 10>Q 7

Zinc and iodine solution react like this:

$Zn (s) + I_{2} (aq) \to {ZnI}_{2} (aq)$

The rate of reaction can be followed by measuring the mass of zinc metal at regular intervals, until all the iodine has been used up.

Sketch a graph showing the mass of zinc on the $y$ axis, and time on the $x$ axis.

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows: CaCO3(s)+2HCl (aq)→CaCl2 (aq)+CO2 (g)+H2O (l) Describe a laboratory method that could be used to investigate the rate of the reaction.

Important Questions on The Speed of a Reaction

Learn and Prepare for any exam you want !

Marble chips (lumps of calcium carbonate) react with hydrochloric acid as follows:

${CaCO}_{3} (s) + 2 HCl (aq) \to {CaCl}_{2} (aq) + {CO}_{2} (g) + H_{2} O (l)$

Describe a laboratory method that could be used to investigate the rate of the reaction.