T6 the rate and extent of chemical change

Question 1

how is rate of reaction calculated

Answer 1

= amount of reactant used or product formed / time

(mol/s) = moles of reactant used or product formed / time

Question 2

what are the various units for rate of reaction

Answer 2

g/s or cm3/s or mol/s

generally, mass/time, volume/time, moles/time

Question 3

name 3 common ways of measuring rate of reaction

Answer 3

loss in mass of reactants
volume of gas produced
time for a solution to become opaque

Question 4

describe measuring the rate by monitoring mass loss

Answer 4

• place the reaction flask on a balance
• in these reactions a gas is given off, so record the decrease in mass in time intervals
• plot a graph of mass vs time

Question 5

describe measuring the rate by monitoring the volume of a gas

Answer 5

• connect a gas syringe to a reaction flask and measure the volume of a gas formed in time intervals
• plot a graph of volume vs time

Question 6

describe measuring the rate by monitoring the disappearance of a cross

Answer 6

• take a piece of paper and mark a X on it
• put the reaction flask on this cross
• mix the reagents, and measure how long it takes for a cloudy mixture to conceal a cross

Question 7

how to find a rate of reaction at some time, t, from a graph of amount of reactant vs time

Answer 7

• pick a point corresponding to the time, t, and find the tangent to the curve at this point
• the tangent is the gradient of this graph, tells you how fast the reaction proceeds at this point
• the steeper the tangent line, the faster the rate
• gradient of tangent can be expressed in change in y values over change in x values

Question 8

state 5 factors affecting the rate of a chemical reaction

Answer 8

concentration of reactants
pressure of gases (volume)
surface area
temperature
catalysts

Question 9

what is collision theory

Answer 9

chemical reactions can occur only when reacting particles collide with each other with sufficient energy (more than or equal to activation energy)

Question 10

describe and explain the effect of increasing temperature on the rate of reaction

Answer 10

T increases = faster reaction
as T increases, kinetic energy of particles increases (more energetic collisions)

also, they move faster so collide more frequently

there is no straight line relationship between the rate and temperature, not directly proportional to one another

Question 11

describe and explain the effect of increasing concentration on the rate of reaction

Answer 11

conc increases = faster reaction

more reactants = more frequent collisions

Question 12

describe and explain the effect of increasing pressure of a gas on the rate of reaction

Answer 12

increases the number of gas molecules in the same volume and so increases the frequency of collisions and therefore increases the rate of the reaction

volume and pressure are inversely proportional to each other
increasing the volume retards the reaction

Question 13

describe and explain the effect of increasing surface area

Answer 13

if solid reactants are in smaller pieces, they have a greater surface area

increasing the surface area of solid reactants increases the frequency of collisions and so increases the rate of reaction

Question 14

what is a catalyst and how does it work

how does it affect the reaction profile

Answer 14

• changes the rate of reaction but is not used up
• increases rate by providing a different pathway for the reaction that has a lower activation energy
• reaction profile for a catalysed reaction will have a lower maximum of the curve (lower activation energy)

Question 15

what is an enzyme

Answer 15

molecule that acts as a catalyst in a biological system

Question 16

what is a reversible reaction

Answer 16

occurs when the products of a reaction can react backwards to produce the original reactants

Question 17

when is dynamic equilibrium reached

Answer 17

in a closed system, when the forward and reverse reactions occur at the same rate and the concentrations of reactants and products remain constant

Question 18

describe Le Chatelier’s principle

Answer 18

if a system is at equilibrium and a change is made to any of the conditions, then the system responds to counteract change and restore the equilibrium

Question 19

describe the effect of changing the concentration of reactant and product on the position on the equilibrium

Answer 19

if the concentration of one of the reactants or products is changed, the system is no longer at equilibrium and the concentrations of all the substances will change until equilibrium is reached again

if the concentration of a reactant is increased, more products will be formed until equilibrium is reached again

if the concentration of a product is decreased, more reactants will react until equilibrium is reached again

Question 20

describe the effect of changing temperature on the position of the equilibrium

Answer 20

if the temperature of a system at equilibrium is increased:

• the relative amount of products at equilibrium increases for an endothermic reaction
• the relative amount of products at equilibrium decreases for an exothermic reaction

Question 21

describe the effect of changing pressure on the position of the equilibrium

Answer 21

this applies to equilibria that involve gases

increase in pressure causes the equilibrium position to shift towards the side with the smaller number of molecules as shown by the symbol equation for that reaction

decrease in pressure causes the equilibrium position to shift towards the side with the larger number of molecules as shown by the symbol equation for that reaction

pressure has no effect on the reactions where the numbers of gas molecules are equal on both sides of the equation

Question 22

describe the effect of a catalyst on the position of the equilibrium

Answer 22

no effect
speeds up both forward and backward reactions equally
equilibrium is achieved faster