Chemical Reactions

Dissolve in the liquid

Escape from the flask

React with the catalyst

Turn back into a solid

Increasing the temperature

Adding a catalyst

Increasing the particle size of a solid reactant

Increasing the concentration of a solution

The rate increases

The rate decreases

The rate remains constant

The rate fluctuates

It acts as a catalyst

It has a very large surface area and can cause explosions

It removes oxygen from the air

It lowers the activation energy of fire

A straight line passing through the origin

An exponential increase in rate with temperature

A horizontal line indicating rate is independent of temperature

A decreasing curve as temperature increases

The kinetic energy of the particles will increase

The concentration of the reactants will increase

The activation energy will decrease

The reaction rate will decrease

It acts as a chemical reactant that binds to silver

It provides the energy to move electrons from $Br^-$ to $Ag^+$

It increases the pressure within the film layer

It acts as a biological catalyst

The reaction is highly exothermic, and the thermal energy released increases the frequency of successful collisions.

The $Mn^{2+}$ ions produced act as a catalyst, providing an alternative reaction pathway with a lower activation energy.

The produced $CO_2$ gas increases the pressure within the reaction vessel, increasing the concentration of the reactants.

The ethanedioic acid dissociates more completely as the reaction proceeds, increasing the frequency of collisions between $H^+$ ions.

All collisions result in products if the kinetic energy is high enough

Only collisions with the correct geometry allow the necessary bonds to break and form

Orientation only matters for spherical atoms like noble gases

Increasing the temperature improves the orientation of the molecules

$\text{s}^{-1}$

$\text{mol}^{-1}\text{ dm}^3\text{ s}^{-1}$

$\text{mol}^{-2}\text{ dm}^6\text{ s}^{-1}$

$\text{mol dm}^{-3}$

They increase.

They decrease.

They stay the same.

They both turn into solids.

It shifts the equilibrium to the right.

It shifts the equilibrium to the left.

It increases the rate at which equilibrium is reached.

It decreases the yield of the products.

Fuel for cars

Making plastics

Making fertilizers

Purifying water

Equilibrium shifts to the left.

Equilibrium shifts to the right.

Equilibrium remains unchanged.

The reaction stops.

It is also exothermic.

It is endothermic with the same magnitude of enthalpy change.

It is endothermic with a much larger magnitude of enthalpy change.

It cannot occur without a catalyst.

The time taken to reach equilibrium.

The activation energy of the forward reaction.

The position of equilibrium.

The rate of the forward reaction.

Increase.

Decrease.

Stay the same.

Initially increase, then decrease.

The reaction is exothermic with $\Delta H = -20\,kJ/mol$.

The reaction is endothermic with $\Delta H = +20\,kJ/mol$.

Increasing the temperature will decrease the value of $K_c$.

The reaction will reach equilibrium faster if $\Delta H$ is increased.

Increases more than the rate of the forward reaction.

Decreases because the reaction is exothermic.

Increases by the same amount as the forward reaction.

Remains constant while the forward rate decreases.

$K_p = P_{NH3} \cdot P_{HCl}$

$K_p = (P_{NH3} \cdot P_{HCl}) / P_{NH4Cl}$

$K_p = P_{NH3} + P_{HCl}$

$K_p = (P_{NH3} \cdot P_{HCl})^2$

0 to -1

0 to +1

+1 to 0

-1 to 0

Fluorine

Chlorine

Bromine

Iodine

-1

+1

+3

+5

$Mg$

$H^{+}$ ions

$Cl^{-}$ ions

$MgCl_{2}$

Iron is oxidized because it loses electrons to the aluminum.

Aluminum is the reducing agent because its oxidation state increases from 0 to +3.

The oxidation state of iron increases from 0 to +3 as it is reduced.

Oxygen is the oxidizing agent because it is transferred from iron to aluminum.

Gain of hydrogen

Loss of hydrogen

Gain of electrons

Loss of oxygen

$Cu^{2+}$

$I^{-}$

$CuI$

$I_{2}$

-3

-1

-1/3

+3

1:1

1:2

2:1

4:1

+4

+2

-2

-4