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Pure substances can be elements or compounds. What effect do solid and liquid pure substances have on the equilibrium position when a gas is also involved?

Question 1 options:

They are denser than gases, and so shift the equilibrium away from their position as product or reactant.

They are more concentrated and so shift the equilibrium away from their position in a balanced equation.

They have no effect on the equilibrium.

They have a profound effect in determining equilibrium position, but this effect is dependent on their bond energies.

Question 2 (1 point)

Consider the reaction in which solid calcium carbonate produces calcium oxide (solid) and carbon dioxide (gas). An increase in pressure will

Question 2 options:

prevent the reaction from occurring

shift the equilibrium to the right

not shift the equilibrium position

shift the equilibrium to the left

Question 3 (1 point)

How does an increase in temperature affect the equilibrium of an endothermic reaction?

Question 3 options:

The equilibrium will shift to the right

The equilibrium will not change.

The equilibrium will shift to the centre

The equilibrium will shift to the left

Question 4 (1 point)

Sulfuric Acid is an important industrial chemical. It is used for fertilizers, detergents, dyes, and medicine. The equilibrium equation for the first step in the contact process is as follows:

2 SO2(g)  + O2(g)  <--> 2SO3(g)      delta H = -196kJ/mol

What would you do to increase the production of SO3?

Question 4 options:

Raise the temperature considerably to shift the equilibrium to the right.

Raise the temperature to shift the equilibrium to the right and increase the rate of formation.

lower the temperature considerably to shift the equilibrium to the right

Lower the temperature moderately to shift the equilibrium right while maintaining the rate of formation (collision theory)

Question 5 (1 point)

The Ksp for an ionic substance is taken into consideration when studying

Question 5 options:

thermal energy

the release of anioins and cations

the dissolving and forming of precipitates

the release of acidic and basic ions

Question 6 (1 point)

What will happen to the following equilibrium if silver ions are added to the solution?

AgNO3(s) <--> Ag(aq) + NO3(aq)  

Question 6 options:

There will be no change

The equilibrium will shift to the right

The equilibrium will shift to the left

The equilibrium will shift to the centre

Question 7 (1 point)

There are many examples of chemical reactions where the products and reactants exist in equilibrium. These include

Question 7 options:

combustion reactions

reactions where the bond energy of the reactants greatly exceeds that of the product

biochemical reactions that occur in a cell

reactions where a gas is involved and escapes to the atmosphere

Question 8 (1 point)

Nitrogen dioxide (brown) and dinitrogen tetroxide (colourless) are placed in a syringe. the syringe is depressed to half its volume. What happens to the pressure in the syringe?

2 NO2(g) <--> N2O4(g)

Question 8 options:

It will initially double, then decrease as the equilibrium shifts left (brown).

It will double, driving the reaction to the right (clear)

It will double, driving the reaction to the left (brown)

It will initially double, then decrease slightly as the equilibrium shifts right (clear)

Question 9 (1 point)

What happens when an acid is added to the following buffer system?

HA(aq) <--> H+(aq)  +  A-(aq)

Question 9 options:

The acid shifts to equilibrium to the left, removing only a few H+ ions, so the pH is decreased

The acid shifts to equilibrium to the right, producing H+ ions, so the pH is decreased

The acid shifts to equilibrium to the right, producing a few H+ ions, maintaining the pH 

The acid shifts to equilibrium to the left, removing H+ ions, maintaining the pH 

Question 10 (1 point)

What do Bronsted-Lowry acids do?

Question 10 options:

They accept electrons

They donate electrons

They accept protons

They donate protons

Question 11 (1 point)

Which of the followoing best describes an amphiprotic substance?

Question 11 options:

prevents reversible reactions

neutralizes acids and bases

proton donor and proton acceptor

consists of an anion and a cation

Question 12 (1 point)

Why is water eliminated from the equilibrium constant?

Question 12 options:

The concentration is constant

It is amphiprotic

It is polar

It does not ionize

Question 13 (1 point)

Solution A has pH of 5 and solution B has a pH of 8. Which has the greater concentration of OH- ions?

Question 13 options:

Solution B

Solution A

It depends on the percent ionization of A and B

It depends on the molarity of A and B

Question 14 (1 point)

Consider the two concentrations of H3O+ ions, 1 x 10^-3 mol/L and 3.2 x 10^-3 mol/L. Which will have the lower pH value?

Question 14 options:

3.2 x 10^-3

The pH value is equal tot h absolute value of the exponent: both have a pH of 3.

1 x 10^-3

It depends on the concentration of hydroxide ions.

Question 15 (1 point)

If pOH = 0.700 for a 0.100 mol/L solution of calcium hydroxide, what would its pH be?

Question 15 options:

13.8

14.7

14.2

13.3

Question 16 (1 point)

If Ka = 5.8 x 10^-10, then what is the value of Kb?

Question 16 options:

8.2 x 10^-4

6.3 x 10^5

9.2

1.7 x 10^-5

True and False

Question 17 (1 point)

At equilibrium the concentration of the reactants is always equal to the concentration of the products.

Question 17 options:

True

False

Question 18 (1 point)

Carbon monoxide reacts with water to form hydrogen and carbon dioxide. If the initial concentration of CO(g) is 3.5mol/L, then the expression for the equilibrium in the ICE table will be x - 3.5.

Question 18 options:

True

False

Question 19 (1 point)

In the Haber process, ammonia is produced in the reaction: N2 + 3H2 <--> 2NH3. The hydrogen molecules will decrease three times faster than nitrogen.

Question 19 options:

True

False

Question 20 (1 point)

The following reaction is an example of a homogeneous system.

CaCO3(s) <--> CaO(s) + CO2(g)

Question 20 options:

True

False

Question 21 (1 point)

Inert gases colliding with reactants and products in a container will result in a chemical reaction.

Question 21 options:

True

False

Question 22 (1 point)

In the following reaction, ammonia acts as a proton acceptor.

NH3 + H2O <--> C + D

Question 22 options:

True

False

Question 23 (1 point)

Water is only ionized when it is in a reversible reaction with another chemical

Question 23 options:

True

False

Short Answers

Question 24 (5 points)

Use an ICE table to determine the equilibrium concentrations for the following reaction if the initial concentrations of SO2 and O2 are 0.6 mol/L and 0.7 mol/L respectively. The value of the equilibrium constant is 2.45 x 10^1 at 25 degrees Celsius.

2 SO2(g)  + O2(g)  <--> 2 SO3(g)

Question 25 (5 points)

Consider the following reaction;

AgIO3(s) <--> Ag+(aq)  + IO3-(aq)

a) Using an ICE table to organize your answer, solve for the equilibrium concentrations of the reaction with a Ksp of 3.17 x 10^-8.

b) How would precipitating the silver our affect this equilibrium?

Question 26 (4 points)

In the incomplete combustion of carbon-based fuels, carbon monoxide is formed:

2C(s) + O2(g) <--> 2 CO(g)

Explain what happens if:

a) there was oxygen added

b) temperature was decreased

c)Increase in pressure

d) a catalyst was added

Question 27 (3 points)

Determine the Ksp for silver chloride if the molar solubility is 1.33 x 10^-5 at 25 degrees Celsius.

Question 28 (2 points)

Describe one example of an indicator or buffer that affects your everyday activities.

Question 29 (7 points)

Methylamine (CH3NH2) is a derivative of the weak base ammonia. Write the equation for the ionization of methylamine in water, and use the I.C.E. method to find the pH of a 3.75 M CH3NH2 solution. (Kb = 4.37 x 10−4 at 25ºC)