chapter 1

Question 1

what are the three states of matter?

Answer 1

solid, liquid, gas

Question 2

what is a mixture?

Answer 2

a mixture contains two or more elements that are not chemically bonded so they retain individual properties

Question 3

what are the two types of mixtures?

Answer 3

homogenous and heterogenous

Question 4

what is the mole?

Answer 4

The mole is a fixed number of particles and refers to the amount, n, of substance.

Question 5

how are masses of an atom compared?

Answer 5

compared on a scale relative to 12DC

Question 6

what are the units of molar mass (M)?

Answer 6

g mol-1

Question 7

what are the two things a reactant can be?

Answer 7

in excess or limiting

Question 8

what is a homogenous mixture?

Answer 8

a homogenous mixture is where all elements have uniform composition so there is only one phase

Question 9

what is a heterogenous mixture?

Answer 9

a heterogenous mixture is where elements do not have uniform compositions so there are seperate phases

Question 10

how do you separate heterogenous mixtures?

Answer 10

mechanical means

Question 11

give an example of a homogenous mixture?

Answer 11

a solution

Question 12

give an example of a heterogenous mixture?

Answer 12

sand in a beaker of water

Question 13

what is the equation for calculation the number of moles?

Answer 13

moles = mass / Mr

Question 14

what is avogadros constant?

Answer 14

6.02 x 10E23

Question 15

equation to calculate number of particles?

Answer 15

moles x avogadros constant

Question 16

what is empirical formula?

Answer 16

formula of a compound give the simplest ratio

Question 17

what is molecular formula?

Answer 17

actual number of atoms present in a molecule

Question 18

what is yield?

Answer 18

the desired amount of product

Question 19

equation for calculation % yield?

Answer 19

(actual yield / theoretical yield) x 100

Question 20

what happens when a limiting reactant is used up?

Answer 20

the reaction stops

Question 21

what is a standard solution?

Answer 21

one of known concentration

Question 22

what are normal/standard conditions?

Answer 22

0 degrees Celsius, 100kPa

Question 23

what assumptions are made for defining ideal gas?

Answer 23

• the molecules have no volume

- there are no forces between volumes

Question 24

what causes gases to deviate from ideal behaviour?

Answer 24

high pressure and low temperature

Question 25

what does avogadros law enable

Answer 25

Avogadro’s law enables the mole ratio of reacting gases to be determined from volumes of the gases

Question 26

what is the equation that links number of moles and volume?

Answer 26

volume = number of moles x molar volume

Question 27

what is boyles law?

Answer 27

at a constant temperature the volume of a mixed mass of an ideal gas is inversely proportional to pressure

Question 28

why can an ideal gas not liquify?

Answer 28

because there are no forces between molecules

Question 29

what is the ideal gas equation?

Answer 29

PV = nRT

Question 30

equation to work out concentration (mol dm3) ?

Answer 30

concentration = moles / volume

Question 31

equation to work out concentration (g dm3) ?

Answer 31

concentration = mass / volume

Question 32

equation to work out concentration (ppm)

Answer 32

concentration = (mass of solute x 10E6) / mass of solution

Question 33

when is ppm notation used?

Answer 33

when talking about pollution

Question 34

how is molar concentration determined?

Answer 34

The molar concentration of a solution is determined by the amount of solute and the volume of solution