7. Chemical reactions Flashcards

1
Q

physical and chemical changes

A

formation of a new substance
difficult to reverse
properties different to reactant

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2
Q

Describe collision theory

A

number of particles per unit volume

frequency of collisions between particles

kinetic energy of particles

activation energy, Ea

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3
Q

Factors affecting rate of reaction

A

temperature- kinetic energy of particles increases, foc between particles increases, higher percentage of particles have energy greater than/ equal to activation energy

pressure- gas particles are pushed closer together, more particles per unit volume, more foc

concentration- more particles per unit volume so foc between particles increases

surface area- more particles exposed to reactants so more foc

adding or removing a catalyst, including enzymes

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4
Q

Catalyst

A

increases the rate of a reaction and is unchanged at the end of a reaction.
It decreases the activation energy, Ea, of a reaction. (by providing alternative pathway requiring lower AE).

mass remain same, are specific to a reaction, required in small amounts

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5
Q

a reversible reaction in a closed system is at equilibrium when

A

the rate of the forward reaction is equal to the rate of the reverse reaction

the concentrations of reactants and products are no longer changing

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6
Q

Effect of temperature, pressure, concentration and catalyst on equilibrium

A

inc temperature- endothermic direction equilibrium shifts to

inc pressure- fewer moles of gas

inc concentration- moves to right (product)

using a catalyst- does not affect

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7
Q

how changing the conditions can change the direction of a reversible reaction for:

(a) the effect of heat on hydrated compounds
(b) the addition of water to anhydrous compounds

A

add water- hydrated- exothermic- contain water of crystallization
heat- anhydrous- endothermic- dehydrated

CuSO4.5H2O reversible- white to blue
CoCl2.6H2O reversible- blue to pink

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8
Q

Haber process- equation, reactants, conditions

A

N2(g) + 3H2(g) ⇌ 2NH3(g)
CH4 (g) + H2O(g) ⇌ 3H2(g)+ CO(g)

hydrogen (methane)- steam reforming
nitrogen (liquid air)- fractional distillation

450°C, 20000kPa /200atm and an iron catalyst

CH4(g)+ H2O(l) ⇌ 3H2 (g)+ CO(g)

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9
Q

contact process- equation, reactants, conditions

A

S+ O2 → SO2
2SO2(g) + O2(g) ⇌ 2SO3(g)

(burning sulfur or roasting sulfide ores) and oxygen (air) in the Contact process

450°C, 200kPa /2atm and a
vanadium(V) oxide catalyst

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10
Q

Define oxidation no., redox reactions, oxidation and reduction, oxidising agent and reducing agent

A

Use a Roman numeral to indicate the oxidation number of an element in a compound.

involving simultaneous oxidation and reduction

oxidation- gain of oxygen, loss of electron, loss of hydrogen, inc in oxidation no.

reduction- loss of oxygen, gain of electron, gain of hydrogen, dec in oxidation no.

oxidising agent- a substance that oxidises another substance and is itself reduced

reducing agent- a substance that reduces another substance and is itself oxidised

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11
Q

Identify redox reactions by the colour changes involved when using acidified aqueous potassium manganate(VII) or aqueous potassium iodide

A

acidified potassium manganate(VII) is an oxidising agent which, when added to a reducing agent its colour changes from purple to colourless.

Potassium iodide, KI, is a reducing agent, turns from colourless to red-brown when added to an acidified solution of an oxidising agent

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