C5 - shit from gizmo idk

Question 1

what is molar volume at room temperature and pressure?

Answer 1

24dm^3

Question 2

what is room pressure?

Answer 2

1 atmosphere

Question 3

how do you calculate the volume of gas at RTP?

Answer 3

volume (dm^3) = number of moles * 24

Question 4

what does increasing pressure do to the position of equilibrium in a dynamic reversible reaction?

Answer 4

favours the side with fewer moles of gas

Question 5

what does increasing the concentration of reactants do to the position of equilibrium in a dynamic reversible reaction?

Answer 5

shifts the equilibrium to the right

Question 6

what is le chatelier’s principle?

Answer 6

states that when a system at equilibrium experiences a change (in temperature, pressure or concentration), the system will respond by shifting the equilibrium position to counteract or minimise that change

Question 7

if the temperature is increased in an endothermic equilibrium, what will happen?

Answer 7

the equilibrium will shift to the right to absorb the extra heat

Question 8

if the temperature is increased in an exothermic equilibrium, what will happen?

Answer 8

the equilibrium will shift to the left to release heat

Question 9

if the pressure is increased in an equilibrium, what will happen?

Answer 9

the equilibrium will shift towards the side with less moles

Question 10

what is the equation for the Haber process?

Answer 10

N2+3H2 <-> 2NH3

Question 11

what temperature is the Haber process reacted at and why?

Answer 11

-450 degrees celsius (moderate)
-favours product formation
-compromise between:
-reaction rate needing heat
-equilibrium position preferring lower
temperature

Question 12

what pressure is the Haber process reacted at?

Answer 12

-200-300 atmospheres
-shifts equilibrium to the right (fewer gas
molecules on product side)
-increases ammonia yield

Question 13

why is the Haber process important?

Answer 13

produces fertilisers, which increases agricultural productivity

Question 14

describe concentration in the industrialised Haber process

Answer 14

-excess hydrogen shifts equilibrium right
-increases ammonia production
-reduces unreacted nitrogen waste

Question 15

describe homogenous catalysts

Answer 15

-intimately mixed with reactants
-easier to control reaction conditions

Question 16

describe heterogeneous catalysts

Answer 16

-separate solid phase from reactants
-can be reused more easily

Question 17

what state are homogenous catalysts typically?

Answer 17

aqueous

Question 18

what state are heterogenous catalysts typically?

Answer 18

solid with liquid/gas reactants

Question 19

in the Haber process for making ammonia, which metal acts as a catalyst?

Answer 19

iron

Question 20

name 3 reasons why catalysts are important industrially

Answer 20

-reduce energy costs
-increase reaction rates
-improve economic efficiency

Question 21

describe catalytic converters

Answer 21

-used in cars
-uses platinum and palladium catalysts
-converts harmful exhaust gases into less
harmful emissions
-reduces environmental pollution

Question 22

what are heterogenous catalysts used in?

Answer 22

catalytic converters

Question 23

what are homogenous catalysts used in?

Answer 23

chemical synthesis and polymer production

Question 24

what is the contact process and why is it important?

Answer 24

-S+O2 > SO2
-2So2 + O2 > 2SO3
(same conditions as Haber process)
-SO3 + H2O > H2SO4
-sulfuric acid is essential for fertilisers