SQA Higher Chemistry Area 3 Chemistry in Society overview quiz quiz

Actual mass of product divided by theoretical mass of product, times 100

Theoretical mass of product divided by the actual mass obtained, times 100

Mass of the desired product divided by the total mass of all the reactants used, times 100

Moles of the product divided by the moles of catalyst added, times 100

How quickly a reaction reaches its position of dynamic equilibrium

The proportion of the total reactant mass that ends up in the desired product

The total amount of energy released per mole of product formed

The total number of individual atoms that are present in a single molecule of the product

To slow the overall rate of the reaction down deliberately

To lower the temperature at which the reaction is carried out

To ensure the more valuable reactant is completely used up

To reduce the atom economy of the industrial process

Equilibrium constants never change, whatever conditions are applied to the system

Adding a catalyst to a reaction always increases the final yield of product obtained

Reactions always go fully to completion, leaving none of the original reactants behind at all in the flask

If a change is applied to a system at equilibrium, the position shifts to oppose that change

It does not change the position, but equilibrium is reached faster

It shifts the position of equilibrium over to the right-hand side

It shifts the position of equilibrium over to the left-hand side

It increases the final yield of the product obtained at equilibrium

The side with more moles of gas

The side with fewer moles of gas

Neither side changes

The side with the heavier molecules

$E_h = nRT$

$E_h = mc^2$

$E_h = cm\Delta T$

$E_h = \Delta H - T\Delta S$

Energy is always released to the surroundings in every chemical reaction

Every chemical reaction is reversible under the right conditions

Enthalpy changes for reactions are always positive in value

The enthalpy change for a reaction is independent of the route taken

As a bleach or antiseptic

As a nitrogen-rich fertiliser spread on crops

As a lubricant for reducing friction in engines

As a strong building material used in construction

Any solution that happens to be made up using ordinary tap water from the laboratory tap

A solution of accurately known concentration, made from a known mass of pure solute and a precise volume

A solution that always has a concentration of exactly one mole per litre, no matter what the solute happens to be

A solution that contains a dissolved catalyst to speed up the reaction being studied

more strongly attracted to the stationary phase than to the mobile phase

always the heaviest component present in the original mixture being separated

more strongly attracted to the mobile phase and less to the stationary phase

completely insoluble in the solvent used as the mobile phase

To make the whole titration procedure run more quickly

To use up less of the standard solution during the experiment

Concordance is not really needed at all, because a single rough titre is enough on its own

To ensure the results are reliable, agreeing within a small range