1.0 Reversible reactions and equilibria summing up (Quizizz)

Which of these is a reversible process?

• Burning firewood

• Dissolving magnesium in acid

• Reacting an acid with an alkali

• Heating hydrated copper (I) sulfate

Which of these statements about dynamic equilibrium is true

• All product molecules are used up

• All reactant molecules are used up

• There is no net change in products or reactants

• There are no forward or backwards reactions

What is special about the forward and backwards reaction at dynamic equilibrium?

• They are zero

• They proceed at the same rate

• The forward reaction is greater

• The backward reaction is greater

If the pressure of a reaction involving gases is increased, in which direction will the equilibrium be shifted

• There will be no shift

• Towards the side with the fewest molecules

• Towards the side with the most molecules

• Towards the side with the greater amount of product

What factors can change the position of the equilibrium?

• Temperature only

• Temperature and pressure only

• Temperature, pressure and concentration

• Temperature, pressure and the use of a catalyst

What effect will increased temperature have on this reaction (forward reaction is exothermic)?
N2(g) + 3H2(g)    <-->    2NH3(g)

• There will be no effect

• The reaction will slow down

• More nitrogen and hydrogen will be produced

• More ammonia will be produced

What effect will increased pressure have on this reaction (forward reaction is exothermic)?
N2(g) + 3H2(g)    <-->    2NH3(g)

• There will be no effect

• The reaction will slow down

• More nitrogen and hydrogen will be produced

• More ammonia will be produced

Why is a pressure not greater than 200 atm used in the Haber process?

• There will be no effect

• It reduces the yield

• It is too expensive

• It is impossible

Why does the Haber process take place at a higher temperature even though this reduces the yield?

• Smaller amounts of reactants are needed

• It produces purer ammonia

• It speeds up the reaction

• It slows down the reaction