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Final exam Revision-G11 chemistry

Total questions: 112

Worksheet time: 19hrs 40mins

Name
Class
Date
1.

When heat flows from system to the surroundings that is an example of an ________________ process.

a)

exothermic

b)

endothermic

2.

What is calorimetry?

a)

process of measuring kinetic and potential energy

b)

process of measuring heat flow of chemical reactions

c)

process of measuring pressure and temperature of a substance

3.

What area of study in chemistry is concerned with the heat transfers that occur during chemical reactions?

a)

stoichiometry

b)

thermochemistry

c)

inorganic chemistry

d)

physical chemistry

4.

1 food calorie = _______ chemistry calories

a)

1000

b)

1

c)

500

d)

4.184

5.

What is the SI unit of heat and energy?

a)

calorie

b)

celsius

c)

joule

6.

The law of conservation of energy states that

a)

in any chemical or physical change, energy cannot be created or destroyed, only changed in form.

b)

heat changes occur during chemical and physical changes.

c)

energy is the capacity to do work or to supply heat

d)

there are two types of energy, kinetic and potential

7.

What is the vocab term for the quantity of heat needed to raise the temperature of 1g of a substance by 1°C?

a)

Joule

b)

Specific Heat

c)

Heat Capacity

d)

calorie

8.

How much ammonia (NH3) can be melted by the addition of 2 kJ of heat (ΔHfus = 5.66 kJ/mol)

a)

.66 g

b)

3.6 g

c)

79.2 g

d)

6.0 g

9.

How many calories of heat are required to raise the temperature of 225g of Al from 20°C to 100°C? (specific heat of Al = 0.21 cal/g°C)

a)

590 calories

b)

3800 calories

c)

38000 calories

d)

85000 calories

10.

A 100 g piece of heated steel cools from 50°C to 20°C. How much heat is released to the surroundings?

a)

300 J of heat are released

b)

300 cal of heat are released

c)

The amount cannot be calculated because the heat capacity isn't known

d)

The amount cannot be calculated because the system isn't closed

11.

What process is exothermic?

a)

condensation

b)

melting

c)

baking a cake

d)

boiling

12.

The specific heat of copper is 0.39 J/g °C. What is the temperature change when 100 Joules of heat is added to 20 grams?

a)

12.82 °C

b)

24.12°C

c)

351 °C

13.

Calculate the ∆H for the following reaction: 2H2O2 → 2H2O + 1 O2

You are given these two equations:

2H2 + O2 → 2H2O ∆H = -572 kJ

H2 + O2 → H2O2 ∆H = -188 kJ

a)

∆H = -948 kJ

b)

∆H = -196 kJ

c)

∆H = -384 kJ

d)

∆H = -188 kJ

14.

Refer the the following question:

2N2 + 3H2 --> 2NH3 + 46 kJ

How much energy would be produced if only 14.0 g of nitrogen was reacted?

a)

92 kJ

b)

0.143 kJ

c)

23 kJ

d)

15 kJ

15.

A + B + heat ---> AB; Delta H, enthalpy is

a)

negative

b)

positive

c)

not enough information given

16.

A reaction that releases heat is

a)

endothermic

b)

exothermic

c)

exotic

d)

a combustion reaction

17.

How many calories are found in 516 Joules of energy?



   (1cal = 4.184 J) Use correct sig figs

a)

123.3 cal

b)

123 cal

c)

2158 cal

d)

2160 cal

18.

Match the definition below to the correct term.

The enthalpy change that takes place when one mole of a compound is formed from its elements in their standard states under standard conditions.

a)

The enthalpy of neutralisation

b)

The enthalpy of combustion

c)

The enthalpy of formation

d)

The enthalpy of reaction

19.

How do you calculate Enthalpy of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

20.

The enthalpy change for the reaction

C(s, graphite) + 1⁄2O2(g) --> CO(g) cannot be measured directly since some carbon dioxide is always formed in the reaction.

It can be calculated using Hess’s Law and the enthalpy changes of combustion of graphite and of carbon monoxide.

C(s, graphite) + O2(g) --> CO2 ΔH=-394 kJmol–1

CO(g) + 1⁄2O2(g) --> CO2 ΔH=-283 kJmol–1

The enthalpy change for the reaction of graphite with oxygen to give carbon monoxide is

a)

-677 kJmol–1

b)

-111 kJmol–1

c)

+111 kJmol–1

d)

+677 kJmol–1

21.

Study the reaction below. Is it exothermic or endothermic?

H2 + Cl2 --> 2 HCl + 1845 kJ

a)

Exothermic Reaction

b)

Endothermic Reaction

22.

ΔH value in an endothermic reaction is negative.

a)

True

b)

False

23.

 HfinalH_{final}   >  HinitialH_{initial}  means _____

a)

change of enthalpy is positive and system absorbs heat

b)

change of enthalpy is negative and system absorbs heat

c)

change of enthalpy is positive and system loses heat

d)

change of enthalpy is negative and system loses heat

24.

Which of the following equations is enthalpy change of formation of carbon dioxide?

a)

C(s) + O2(g) --> CO2(g)

b)

CO(g) + 1/2O2 --> CO2(g)

25.

Calculate the heat of RXN using the listed heats of formation.

NOTE: Fluorine gas = 0 kJ/mol

a)

-1934.59 kJ

b)

-1934.6 kJ

c)

-1935 kJ

d)

-1934 kJ

26.

Use the given standard enthalpies of formation to determine the heat of reaction of the given chemical RXN.

NOTE: Na and hydrogen gas = 0 kJ

a)

-282 kJ

b)

-282.0 kJ

c)

282 kJ

d)

282.0 kJ

27.

Calculate the standard enthalpy of formation for the RXN from the listed standard enthalpies of the substances involved.

a)

-410.8 kJ

b)

-411 kJ

c)

410.8 kJ

d)

411 kJ

28.

The standard enthalpy of formation of propene is +20.6 kJ/mole. Calculate the heat of combustion of one mole of propene. The heats of formation of carbon dioxide gas and water liquid are -394 kJ/mole and -285.8 kJ/mole respectively.

NOTE: Diatomic molecule present in the RXN has 0 kJ standard enthalpy of formation.

a)

-4120 kJ

b)

-4120.0 kJ

c)

4120 kJ

d)

4120.0 kJ

29.

Using Hess law, compute the thermochemical equation to know the total heat of RXN.

a)

-3216.8 kJ

b)

-136.8 kJ

c)

3216 kJ

d)

-136.8 J

30.

Is the following exothermic or endothermic?

a)

Endothermic

b)

Exothermic

31.

Calculate ΔH when 2 moles of ethanol (C2H5OH) reacts with excess oxygen according to the following thermochemical equation?

C2H5OH + 3O2 → 2CO2 + 3H2O ΔH = −1366.7 kJ

a)

-2733.4 kJ

b)

-683.35 kJ

c)

-1366.7 kJ

d)

-910.67 kJ

32.

What will ΔH be if there is 1 mole of oxygen?

4Fe(s) + 3O2(g) --> 2Fe2O3(s) ΔH = –1500 kJ

a)

-500 kJ

b)

500 kJ

c)

-750 kJ

d)

-4500 kJ

33.
What mass of P4 must be reacted to produce 5905 kJ of energy?
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
a)
25.43 g
b)
563.0 g
c)
2.421 g
d)
300.0 g
34.
C+ O2 --> CO2 + 60kJ, what is the value for ΔH for the reaction?
a)
+60
b)
-60
c)
there is no way to know
35.

which of the following enthalpy changes represent the enthalpy change of formation?

a)

Mg(s) + Cl2(g) → MgCl2(s)

b)

Mg2+(g) + 2 Cl -(g) → MgCl2(aq)

c)

O2(g) → 2 O(g)

d)

2Mg (s) + O2(g) → 2MgO(S)

36.
a)

202.9 kJ

b)

1256.3 kJ

c)

363.1 kJ

37.

Calculate ΔH° for the following reaction. The standard enthalpies of formation for the two reactants and two products are, in order, -1118, -110.5, -272, -393.5 (all in kJ/mol)


Fe3O4(s) + CO(g) →3FeO(s) + CO2(g)

a)

-263 kJ

b)

54 kJ

c)

19 kJ

d)

-50 kJ

38.

Calculate the enthalpy of reaction (ΔH).

4CO2 (g) + 6H2O (g) → 2C2H6 (g) + 7O2 (g)


ΔHfo [CO2(g)] = -393.5 kJ

ΔHfo [H2O(g)] = -241.8 kJ

ΔHfo [C2H6(g)] = -84.7 kJ

a)

550.6 kJ/mol

b)

2855.4 kJ/mol

c)

-550.6 kJ/mol

d)

-3194.2 kJ/mol

39.

Which would have the highest positional entropy?

a)

Solid CO2

b)

Liquid CO2

c)

Gaseous CO2

40.

If a process generates heat and is not spontaneous, which of the following is true?  \   

a)

 Δ G < 0\Delta\ G\ <\ 0  

b)

 Δ H > 0\Delta\ H\ >\ 0  

c)

 Δ S < 0\Delta\ S\ <\ 0  

d)

 Δ G = 0\Delta\ G\ =\ 0  

41.
A reaction has a positive ΔH and a positive ΔS. Which of the following is true?
a)
It will be spontaneous at all temperatures.
b)
It will be nonspontaneous at all temperatures.
c)
It will be spontaneous at low temperatures.
d)
It will be spontaneous at high temperatures.
42.

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

43.

1. Given the following information, calculate ΔG0 for the reaction below at 250C: (K = 0C + 273)

SnCl4(l) + 2 H20(l) → SnO2(S) + 4HCl(g),

ΔH0=133.0 kJ and ΔS0 =401.5 J/K

a)

-252.6 kJ

b)

-13.4 kJ

c)

13.4 kJ

d)

252.6 kJ

44.

The thermodynamic quantity that expresses the degree of disorder in a system is _

a)

entropy

b)

internal energy

c)

heat flow

d)

enthalpy

e)

bond energy

45.

ΔS will be positive for the reaction

a)

2H2 (g) + O2 (g) -> 2H2O (g)

b)

2NO2 (g) -> N2O4 (g)

c)

BaF2 (s) ->Ba2+ (aq) + 2F- (aq)

d)

2Hg (l) + O2 (g) ->2HgO (s)

46.

Which one of the following processes produces a decrease in the entropy of the system?

a)

dissolution of solid KCl in water

b)

mixing of two gases into one container

c)

freezing water to form ice

d)

melting ice to form water

47.

For a reaction to be spontaneous under standard conditions at all temperatures, the signs of ΔHΟ and ΔSΟ must be __________ and __________, respectively.

a)

+, +

b)

+, -

c)

-, +

d)

-, -

e)

+, 0

48.

What does Gibbs Free Energy tell us?

a)

How much energy is given off by a reaction.

b)

The tendency of a reaction to become "random"

c)

How spontaneous a reaction is.

49.

Predict the signs of ΔH , ΔS and ΔG for the reaction:

Mg(s) --> Mg(g)

a)

Δ H = - , Δ S = + and Δ G = - (all temperature)

b)

Δ H = + , Δ S = + and Δ G = - (At all temperature)

c)

Δ H = + , Δ S = + and Δ G = - (At low temperature)

d)

Δ H = + , Δ S = + and Δ G = - (At high temperature)

50.

Using the equations below:


C(s) + O2(g) → CO2(g) ∆H = –390 kJ

Mn(s) + O2(g) → MnO2(s) ∆H = –520 kJ


what is ∆H (in kJ) for the following reaction?


MnO2(s) + C(s) → Mn(s) + CO2(g)

a)

910

b)

130

c)

-130

d)

-910

51.

Using the equations below


Cu(s) + 1/2O2(g) → CuO(s) ∆H = –156 kJ

2Cu(s) + O2(g) → Cu2O(s) ∆H = –170 kJ


what is the value of ∆H (in kJ) for the following reaction?


2CuO(s) → Cu2O(s) + 1/2O2(g)

a)

142

b)

15

c)

-15

d)

-142

52.

Consider the following equations.


Mg(s) + O2(g) → MgO(s) ∆H = –602 kJ

H2(g) + O2(g) → H2O(g) ∆H = –242 kJ


What is the ∆H value (in kJ) for the following reaction?


MgO(s) + H2(g) → Mg(s) + H2O(g)

a)

-844

b)

-360

c)

+360

d)

+844

53.

Hess' Law makes use of which principle to calculate the enthalpy change of a reaction?

a)

The law of conservation of energy

b)

The law of conservation of matter

c)

The law that you will always find a lost item in the last place you look for it

d)

Murphy's law

54.

In order to find the enthalpy of combustion of C3H8 how must the enthalpy changes be arranged?

a)

ΔH3 = ΔH1 + ΔH2

b)

ΔH2 = ΔH3 - ΔH1

c)

ΔH1 = ΔH2 - ΔH3

d)

0 = ΔH1 + ΔH2 + ΔH3

55.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

56.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

57.
What is the rate of reaction?
a)
How fast a reaction is 
b)
How big a reaction is
c)
How loud a reaction is
d)
How much gas a reaction produces
58.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
59.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

60.
The rate of a chemical reaction is NOT affected by which of the following:
a)
temperature
b)
concentration
c)
particle size (surface area)
d)
All of these affect reaction rates
61.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
62.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
63.

Table 4 shows the total volume of gas evolved at different intervals for the dissociation of hydrogen peroxide.


What is the average rate of reaction in the second minute?

a)

14.0 cm3 min-1

b)

16.0 cm3 min-1

c)

18.0 cm3 min-1

d)

28.0 cm3 min-1

64.

An experiment is carried out to study the effect of concentration on the rate of reaction between sodium thiosulphate and hydrochloric acid.


Graph of the concentration of sodium thiosulphate against 1/time is as shown.


Based on the graph, what is the value of t if the experiment is repeated using sodium

thiosulphate solution 0.025 mol dm-3.

a)

32.3 s

b)

50.0 s

c)

0.020 s

d)

0.031s

65.

Diagram 4 shows the graph of volume of carbon dioxide gas against time when 5 g of marble chips is added to

50 cm3 of 0.2 mol dm-3 hydrochloric acid.


At what time the rate of reaction the highest?

a)

t1

b)

t2

c)

t3

d)

t4

66.

Diagram 12 shows an energy profile diagram. Ea is the activation energy for the decomposition of hydrogen peroxide.

P

Which of the following is the activation energy for the dissociation of hydrogen peroxide when manganese(IV) oxide is added?

a)

P

b)

Q

c)

R

d)

S

67.

Which of the following explains the meaning of effective collision?

a)

The collision where its energy is less than the activation energy

b)

The collision that has a low energy

c)

The collision which takes place before a reaction

d)

The collision that causes a reaction

68.

Which of the following is the meaning of activation energy?

a)

The maximum energy that the particles need to produce effective collision

b)

The amount of energy used by the particles during a collision

c)

The minimum amount of energy that particles must have in order to react

d)

The amount of kinetic energy of molecules during a collision

69.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

70.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
71.

What is the energy of the activated complex?

a)

75 kJ

b)

225 kJ

c)

300 kJ

d)

50 kJ

72.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
73.

What is the name given to a catalyst in the human body?

a)

Biology

b)

Catalyst

c)

Chemical

d)

Enzyme

74.

The collisions which bring about a chemical reaction are called:

a)

Consistent collisions

b)

Normal collisions

c)

Effective collisions

75.
The equation and energy profile for combustion of methane is shown. 
According to the information provided on this profile, the activation energy for the reaction:
0.5CO2(g) + H2O(g) → 0.5CH4(g) + O2(g)
would be
a)
1635 kJ
b)
2135 kJ
c)
2490 kJ
d)
4270 kJ
76.
A reaction has the rate law: Rate = k [A][B].
What is the order of reaction with respect to A?
a)
1st
b)
2nd
c)
3rd
d)
4th
77.
A reaction has the rate law: Rate = k [A][B].
What is the overall order of reaction?
a)
1st
b)
2nd
c)
3rd
d)
4th
78.
A possible rate law for a third overall order of a reaction is __________________
a)
Rate = k [A]2[B]2
b)
Rate = k [A][B]3
c)
Rate = k [A]3 [B]
d)
Rate = k [A]2[B]
79.
Write the rate law for the reaction aA → bB if the reaction is third order in A. [B] is not part of the rate law.
a)
Rate =k[A]
b)
Rate =3[A]
c)
Rate =k[3A]
d)
Rate =k[A]3
80.
A reaction has the rate law: Rate = k [A][B].
What will happen to the rate of reaction if the concentration of A is doubled and the concentration of B is tripled?
a)
increases by a factor of 3
b)
increases by a factor of 4
c)
increases by a factor of 5
d)
increases by a factor of 6
81.
The rate law for the reaction 2NO(g) + O2(g) → 2NO2(g) is first order in O2 and third order overall. What is the rate law for the reaction?
a)
Rate = k [NO]2[O2]2
b)
Rate = k [NO]1[O2]2
c)
Rate = k [NO]2[O2]1
d)
Rate = k [2NO]2[O2]1
82.
Which two trials would you use to find the rate exponent for A?
a)
trials 1 and 2
b)
trials 1 and 3
c)
trials 2 and 3
83.
What two trials would you use to find the rate exponent for B?
a)
trials 1 and 2
b)
trials 1 and 3
c)
trails 2 and 3
84.
What is the rate exponent for A?
a)
0
b)
1
c)
2
85.
The rate law of any chemical reaction 
a)
must be determined experimentally
b)
can be deduced based on the stoichiometry of the reaction
c)
changes based on the condition of the experiment
d)
I don't know
86.
Find the order for F2 and CIO2 using data shown below.
a)
(F2 - 2nd order) (CIO2 - 1st order)
b)
(F2 - 1st order) (CIO2 - 1st order)
c)
(F2 - 1st order) (CIO2 - 2nd order)
d)
(F2 - 2nd order) (CIO2 - 2nd order)
87.
The only factor that can change the value of k is:
a)
concentration
b)
a catalyst
c)
surface area
d)
temperature
88.

The rate constant for a second-order reaction is 0.15 M-1s-1. If the initial concentration of the reactant is 0.30 M, how long does it take for the concentration to decrease to 0.15 M? (2 sig figs with unit)

(a)  

89.

A compound decomposes by a first-order process. If 25.0% of the compound decomposes in 60.0 minutes, find the rate constant. (3 sig figs with unit)

(a)  

90.

Cyclopentane is unstable and decomposes by a first order reaction. The rate constant for this reaction is 9.5 s-1. What is the half-life of the reaction? (2 sig figs and unit)

(a)  

91.

The rate of the reaction 2A + B → C was measured at different concentrations of the reactants. Find the rate law if the results are as follows:

a)

rate = k[A][B]

b)

rate = k[A]2[B]

c)

rate = k[A][B]2

d)

rate = k[A]2[B]0

92.

The rate law for a reaction is rate = k[Al2O3]2[NaOH]. What is the rate constant for this reaction if the reaction proceeds at an initial rate of 0.005 M/s when all of the reactants have initial concentrations of 0.02M? (3 sig figs and NO unit)

(a)  

93.

What is the rate law for the following?

A + 2B + C → D

a)

rate = k[A][B][C]2

b)

rate = k[B][C]

c)

rate = k[A][B]2[C]

d)

rate = k[B][C]2

94.

Given the following information.

a)

Rate = k[NH4+][NO2-]

b)

Rate = k[NH4+]2[NO2-]2

c)

Rate = k[NH4+]2[NO2-]

d)

Rate = k[NH4+][NO2-]2

e)

none of the above

95.

What is collision theory?

a)

Molecules must collide in the correct orientation with enough energy to bond.

b)

Molecules need enough energy to collide and react.

c)

Atoms constantly collide and react.

d)

The minimum energy needed for atoms to react

96.
The collisions which bring about a chemical reaction are called: 
a)
Consistent collisions
b)
 Normal collisions 
c)
Effective collisions 
d)
None of the above
97.

The factor that will slow down the rate of a chemical reaction.

a)

Manual stirring of the substance.

b)

Placing substance in a hot water.

c)

Placing products in iced water.

d)

Placing reactants in an ice bath.

98.

What does Gibbs Free Energy tell us?

a)

How much energy is given off by a reaction.

b)

The tendency of a reaction to become "random"

c)

How spontaneous a reaction is.

99.

What information do we need to perform a calculation of Gibbs Free Energy?

a)

Enthalpy of the reaction.

b)

Entropy of the reaction.

c)

The temperature of the reaction in Kelvin.

d)

All of the above are needed.

100.

Which of the following would most likely lead to a spontaneous reaction.

a)

A high negative enthalpy.

b)

A low negative enthalpy.

c)

A high positive enthalpy.

d)

A low positive enthalpy.

101.
A reaction has a positive ΔH and a positive ΔS. Which of the following is true?
a)
It will be spontaneous at all temperatures.
b)
It will be nonspontaneous at all temperatures.
c)
It will be spontaneous at low temperatures.
d)
It will be spontaneous at high temperatures.
102.

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

103.

For the process at 250C : I2(g) →I2(s). What are the signs for ΔG, ΔH and ΔS?

a)

ΔG + ΔH - ΔS -

b)

ΔG - ΔH - ΔS -

c)

ΔG - ΔH + ΔS +

d)

ΔG - ΔH + ΔS +

104.

At what temperature would a given reaction become spontaneous if ΔH =+119kJ and ΔS=+263J/K.mol

a)

452 K

b)

2210 K

c)

382 K

d)

363 K

105.

Which reaction has a +ΔS ?

a)

AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

b)

H2O(g) + CO2(g) → H2CO3(aq)

c)

H2(g) + I2(g) → 2Hl(g)

d)

C2H2O2(g) → 2CO(g) + H2(g)

106.

Which sample has the lowest entropy?

a)

1 mole of KNO3(l)

b)

1 mole of KNO3(s)

c)

1 mole of H2O(l)

d)

1 mole of H2O(g)

107.

Entropy increases from solid, liquid to gas. Why?

a)

Molecular disorder increases

b)

Molecules increase in number from solid to gas

c)

Molecules are heavier in solid

d)

Molecules are more reactive

108.
Entropy always increases when
a)
enthalpy decreases.
b)
temperature decreases.
c)
temperature increases.
d)
volume increases.
109.

Given the change of phase:  CO2(g) →\rightarrow  CO2(s)

As CO2(g) changes to CO2(s), the entropy of the system

a)

decreases

b)

increases

c)

remains the same

110.

Entropy of a system increases when a reaction increases the number of particles.

a)

True

b)

False

111.

Predict the entropy change for this reaction 

  N2O4(g)N_2O_4\left(g\right)   →  2NO2(g)2NO_2\left(g\right)   

a)

ΔS = +ve and non spontaneous

b)

ΔS = -ve and spontaneous

c)

ΔS = -ve and non spontaneous

d)

ΔS = +ve and spontaneous

112.

Which of the reactions below has a negative ∆S?

a)

CuCO3 (s) + 2HCl (aq) → CuCl2 (aq) + CO2 (g) + H2O (l)

b)

C (s) + O2 (g) → CO2 (g)

c)

CuO (s) + H2SO4 (aq) → CuSO4 (aq) + H2O (l)

d)

BaCl2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaCl (aq)

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