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

${\mathrm{CaCO}}_3\left(\mathrm{s}\right)+2\mathrm{HCl} \left(\mathrm{aq}\right)\to {\mathrm{CaCl}}_2 \left(\mathrm{aq}\right)+{\mathrm{CO}}_2 \left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$

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:

${\mathrm{CaCO}}_3\left(\mathrm{s}\right)+2\mathrm{HCl}\left(\mathrm{aq}\right)\to {\mathrm{CaCl}}_2\left(\mathrm{aq}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

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

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

${\mathrm{CaCO}}_3\left(\mathrm{s}\right)+2\mathrm{HCl}\left(\mathrm{aq}\right)\to {\mathrm{CaCl}}_2\left(\mathrm{aq}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

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

Zinc and iodine solution react like this:

$\mathrm{Zn}\left(\mathrm{s}\right)+ {\mathrm{I}}_2\left(\mathrm{aq}\right) \to {\mathrm{ZnI}}_2\left(\mathrm{aq}\right)$

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?

Zinc and iodine solution react like this:

$\mathrm{Zn}\left(\mathrm{s}\right)+ {\mathrm{I}}_2\left(\mathrm{aq}\right) \to {\mathrm{ZnI}}_2\left(\mathrm{aq}\right)$

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.

Zinc and iodine solution react like this:

$\mathrm{Zn}\left(\mathrm{s}\right)+ {\mathrm{I}}_2\left(\mathrm{aq}\right) \to {\mathrm{ZnI}}_2\left(\mathrm{aq}\right)$

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?

Zinc and iodine solution react like this:

$\mathrm{Zn}\left(\mathrm{s}\right)+{\mathrm{I}}_2\left(\mathrm{aq}\right)\to {\mathrm{ZnI}}_2 \left(\mathrm{aq}\right)$

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 $\mathrm{y}$ axis, and time on the $\mathrm{x}$ axis.

Zinc and iodine solution react like this:

$\mathrm{Zn}\left(\mathrm{s}\right)+ {\mathrm{I}}_2\left(\mathrm{aq}\right) \to {\mathrm{ZnI}}_2\left(\mathrm{aq}\right)$

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.

How will the graph change if the temperature of the iodine solution is increased by $10°\mathrm{C}$?

Zinc and iodine solution react like this:

$\mathrm{Zn}\left(\mathrm{s}\right)+ {\mathrm{I}}_2\left(\mathrm{aq}\right) \to {\mathrm{ZnI}}_2\left(\mathrm{aq}\right)$

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.

How will the graph between concentration of zinc and time changes, if the temperature of the iodine solution is increased by ${10}^{\mathrm{o}}\mathrm{C}$ ? Explain your answer using the idea of collisions between particles.