Chapter 19

Question 1

The partial pressure of a gas in a mixture is

Answer 1

the pressure that the gas would have if it alone occupied the volume occupied by the whole mixture.

Question 2

If a mixture of gases contains 3 different gases then the total pressure will equal the 3 partial pressure added together
equation

Answer 2

P =p1 + p2 + p3

Question 3

partial pressure =
word and symbol

Answer 3

mole fraction x total pressure of gas 1
p1 = x1 P

Question 4

mole fraction =

Answer 4

number of moles of a gas/ total number of moles of all gases

Question 5

moles of reactant at equilibrium =

Answer 5

initial moles – moles reacted

Question 6

moles of product at equilibrium =

Answer 6

initial moles + moles formed

Question 7

the techniques and procedures used to
determine quantities present at equilibrium

Answer 7

titrations and using colorimeter

Question 8

expressions for Kc and Kp for homogeneous and heterogeneous equilibria

Answer 8

homogenous equilibrium-> involved reactants are in the same state
heterogenous equilibrium-> molar concentrations for solids and pure liquids do not change because volume is constant. so concentrations of pure solids and liquids are not included in Kc

Question 9

The larger the Kc the greater the

Answer 9

amount of products.
If Kc is small we say the equilibrium favours the reactants

Question 10

if K is… =,> or <

Answer 10

K= 1, position of equilibrium halfway between products and reactants
K>1= product side is favoured
K<1= reactant side is favoured

Question 11

Kc and Kp only change with

Answer 11

temperature

Question 12

Changing concentration would shift the position of equilibrium but

Answer 12

the value of Kc would not change.

Question 13

Catalysts have no effect on the value of Kc or Kp or the position of equilibrium because

Answer 13

they speed up both forward and backward rates by the same amount.

Question 14

exothermic reaction, increasing temperature will mean

Answer 14

less yield as equilibrium moves to the left(reactants) to lower temperature

Question 15

endothermic reaction, increasing temperature will mean

Answer 15

more yield as equilibrium shifts to the right(products) to increase temperature

Question 16

Increasing pressure does

Answer 16

not change Kc.

Question 17

The position of equilibrium will change if(kp and pressure)

Answer 17

pressure is altered but the value of Kp stays constant as Kp only
varies with temperature

Question 18

Kp expressions only contain

Answer 18

gaseous substances. Any substance with another state is left out

Question 19

mole fraction definition

Answer 19

is a measure of how much of a given substance is present in a reaction mixture