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If 21.4 g of carbon dioxide is produced in the reaction of ethyne with oxygen to form carbon dioxide and water, how many grams of water are produced in this reaction?

1. 8.76 g

2. 4.38 g

3. 17.5 g

4. 2.92 g

5. None of these

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Question 2

1 Point

What volume of 4.7 M sodium hydroxide will be needed to neutralize 2.0 L of 1.0 M hydrochloric acid?

1. 0.43 L

2. 9.4 L

3. 2.4 L

4. 4.7 L

5. 6.7 L

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Question 3

1 Point

The balanced equation 2Cu+O2->2CuO tells us that 8.0 mol of Cu

1. reacts with 8.0 mol of O2

2. produces 8.0 mol of CuO

3. must react with 256 g of O2

4. cannot react with oxygen

5. produces 16.0 mol of CuOBottom of Form

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Question 4

1 Point

Consider the following reaction: 3Fe+4H2O->Fe3O4+H2

How many grams of steam must react to produce 381 g of ferrous ferric oxide (Fe3O4)?

1. 29.6 g

2. 6.58 g

3. 1.65 g

4. 119. g

5. 7.41 g

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Question 5

1 Point

The process of using a chemical equation to calculate the absolute masses of reactants and products involved in a reaction is called stoichiometry. Is this statement true or false?

1. True

2. False

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Question 6

1 Point

According to the equation below, how many moles of oxygen are produced by decomposing 36.8 g of hydrogen peroxide(molar mass = 34.0 g/mol)?

2H2O2->2H2O+O2

1. 1.082 mol oxygen

2. 626 mol oxygen

3. 0.541 mol oxygen

4. 2.16 mol oxygen

5. None of these

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Question 7

1 Point

Tetraphosphorous hexaoxide is formed by the reaction of phosphorous (P4) with oxygen gas. If the reaction of 19.4 g of phosphorus (P4) with 68.3 g of oxygen produces 21.0 g of Tetraphosphorous hexaoxide, calculate the percent yield for the reaction.

1. 34.4

2. 156.5

3. 13.4

4. 86.6

5. 61.0

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Question 8

1 Point

In the reaction below, how many molecules of water can be produced by starting with 40.3 kilograms of sodium hydroxide and excess chlorine?

3Cl2+6NaOH->5NaCl+NaClO3+3H2O

1. 1.82 × 1027 molecules water

2. 1.01 × 1026 molecules water

3. 3.03 × 1026 molecules water

4. 6.07 × 1026 molecules water

5. None of these

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Question 9

1 Point

For the reaction of ethene, C2H4(g), with oxygen(g) to form carbon dioxide(g) and water(g), what number of moles of carbon dioxide can be produced by the reaction of 5.00 mol ethene and 10.2 mol oxygen?

1. 15.3 mol

2. 10.2 mol

3. 6.80 mol

4. 10.0 mol

5. None of these

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Question 10

1 Point

You react 16.9 g of nitrogen gas with 16.9 g of hydrogen gas. Determine the mass of ammonia that can be produced from these two reactants.

1. 10.3 g

2. 5.14 g

3. 95. g

4. 143. g

5. 20.5 g

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Question 11

1 Point

Refer to the following equation: 4NH3+7O2->4NO2+6H2O

How many molecules of water are produced if 1.76 mol of NO2 is given off?

1. 2.12 × 1024

2. 1.06 × 1024

3. 31.7

4. 1.59 × 1024

5. none of these

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Question 12

1 Point

For the reaction of ethene, C2H4(g), with oxygen(g) to form carbon dioxide(g) and water(g), how many grams of carbon dioxide could be produced from 2.0 g of ethene and 3.1 g of oxygen?

1. 6.4 g

2. 2.8 g

3. 4.3 g

4. 6.3 g

5. None of these

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Question 13

1 Point

The reactant that runs out first and limits the amounts of products that can form is called the _____.

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Question 14

1 Point

In the reaction below, how many molecules of water can be produced from 40.7 g of sodium hydroxide and excess chlorine?

1. 1.23 × 1024 molecules water

2. 3.06 × 1023 molecules water

3. 1.53 × 1023 molecules water

4. 6.13 × 1023 molecules water

5. 8.17 × 1023 molecules water

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Question 15

1 Point

Refer to the following unbalanced equation: C6H14+O2->CO2+H2O

What mass of oxygen (O2) is required to react completely with 21.4 g of C6H14?

1. 6.51 × 103 g

2. 37.7 g

3. 7.95 g

4. 75.5 g

5. 0.248 g

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Question 16

1 Point

Consider a general unbalanced reaction in which two reactants make one product: Following information you know about the reaction:

2.0 mol A (with an excess of B) can produce a maximum of 2.0 mol C.

3.0 mol B (with an excess of A) can produce a maximum of 4.0 mol C.

If you react 2.0 mol of A with 3.0 mol of B, what is the maximum amount of C that can be produced?

1. 2.0 mol

2. 4.0 mol

3. 5.0 mol

4. 6.0 mol

5. More information is needed to answer this question.

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Question 17

1 Point

When 37.1 g of CH4 reacts completely with excess chlorine yielding 52.0 g of HCl, what is the percentage yield, according to CH4(g) + Cl2(g) → CH3Cl(g) + HCl(g)

1. 84.6

2. 38.6

3. 71.3

4. 28.7

5. 61.4

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Question 18

1 Point

In the reaction below, 34.8 g of solid calcium carbonate is mixed with 51.6 g hydrochloric acid. How many grams of carbon dioxide will be produced?

CaCO3+2HCl->CaCl2+CO2+H2O

1. 12.3 g carbon dioxide

2. 30.6 g carbon dioxide

3. 7.7 g carbon dioxide

4. 31.1 g carbon dioxide

5. 15.3 g carbon dioxide

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Question 19

1 Point

Reacting 3.00 mol nitrogen gas with 3.59 mol hydrogen gas will produce how many moles of ammonia according to the following balanced chemical equation?

N2+3H2->2NH3

1. 3.59 mol NH3

2. 5.39 mol NH3

3. 2.39 mol NH3

4. 7.18 mol NH3

5. 6.00 mol NH3

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Question 20

1 Point

Consider the following reaction: 2A+B->3C+D

3.38 mol of A and 2.00 mol of B react to form 4.00 mol of C. What is the percent yield of this reaction?

1. 21.1%

2. 52.6%

3. 39.4%

4. 78.9%

5. 100.%

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Question 21

1 Point

Consider the following unbalanced equation:

C2H5OH+O2->CO2+H2O

If 1.18 g of ethanol reacts with 14.1 g of oxygen, how many moles of carbon dioxide are produced?

1. 0.0256 mol

2. 0.294 mol

3. 0.0512 mol

4. 0.441 mol

5. 0.0128 mol

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Question 22

1 Point

How many moles of oxygen will be produced by the decomposition of 7 moles of water?

1. 3.5 moles

2. 4.5 moles

3. 3.0 moles

4. 2.5 moles

5. 4.0 moles

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Question 23

1 Point

Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. If 3.75 mol of magnesium and 3.75 mol of hydrochloric acid are reacted, how many grams of excess reactant are left over?

1. 1.88 g

2. 91.2 g

3. 68.4 g

4. g

5. 45.6 g

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Question 24

1 Point

Consider the following reaction at 1.10 atm and 19°C:

2NaCL+2NH3+CO2+H2O->2NH4CL+Na2CO3

0.216 mol of sodium chloride, 2.98 L of ammonia, 2.00 L of carbon dioxide, and an unlimited amount of water react to form aqueous ammonium chloride and solid sodium bicarbonate. How many moles of ammonium chloride are formed in the reaction?

1. 0.137 mol

2. 0.274 mol

3. 0.216 mol

4. 5.96 mol

5. 0.0918 mol

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Question 25

1 Point

According to the unbalanced equation below, how many moles of antimony trichloride are formed when 4.00 mol of antimony is reacted with 5.14 mol of chlorine?

Sb+Cl2->SbCL3

1. 7.71 mol antimony trichloride

2. 5.14 mol antimony trichloride

3. 3.43 mol antimony trichloride

4. 4.00 mol antimony trichloride

5. It cannot be determined based on the information given.

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Question 26

1 Point

In the reaction

Cu+2AgNO3->2Ag+Cu(NO3)2

what number of grams of silver can be produced from the reaction of 83.7 g of copper?

1. 284 g Ag

2. 142.1 g Ag

3. 71.1 g Ag

4. 98.6 g Ag

5. 1.32 g Ag

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Question 27

1 Point

A 49.3 sample of CaCO3 was treated with aqueous H2SO4, producing calcium sulfate, 3.65 g of water and CO2(g). What was the % yield of H2O?

1. 8.9

2. 58.9

3. 7.4

4. 92.6

5. 41.1

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Question 28

1 Point

In the reaction below, how many moles of chlorine are needed to react with 23.9 g of sodium hydroxide?

2Cl2+$NaOH3NaCL+NaClO2+2H2O

1. 1.20 mol chlorine

2. 0.598 mol chlorine

3. 0.398 mol chlorine

4. 0.149 mol chlorine

5. 0.299 mol chlorine

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Question 29

1 Point

A mole ratio is used to convert the moles of a starting substance to the moles of a desired substance. Is this statement true or false?Bottom of Form

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Question 30

1 Point

Look at the reaction below:

Al(OH)3+3HCl->3H2O+AlCl3

Suppose 0.55 g of water were produced from 1.2 g of aluminum hydroxide and a certain amount of hydrochloric acid. Which of the following statements is true? Choose the best answer.

1. Aluminum hydroxide is the limiting reactant because 1.2 g of aluminum hydroxide produces 0.55 g of water.

2. Aluminum hydroxide is the limiting reactant because it has a smaller coefficient than hydrochloric acid.

3. Aluminum hydroxide is not the limiting reactant because more than 0.55 g of water could have been produced from 1.2 g of aluminum hydroxide.

4. Aluminum hydroxide is not the limiting reactant because some amount of aluminum hydroxide is left.

5. There is not enough information given to answer this question.

31. State whether the kinetic energy of the underlined object increases or decreases as a result of the change described.

a tennis ball is served

an air plane lands

a bullet is shot from a pistol

32. What is the kinetic energy of a 148 gram baseball moving at a velocity of 42.0 meters per second?

33. An automobile engine generates 2155 Joules of heat that must be carried away by the cooling system. The internal energy changes by -2736 Joules in this process. Calculate w for the engine. This represents the work available to push the pistons in this process.

34. A chemical reaction is run in which 153 Joules of heat are absorbed and the internal energy changes by +568 Joules. Calculate w for the system.

35. In the laboratory a student finds that it takes 2.21×103 Joules to increase the temperature of 10.8 grams of gaseous hydrogen from 20.5 to 36.0 degrees Celsius. The specific heat of hydrogen calculated from her data is___J/g°C.

36. The following thermochemical equation is for the reaction of CO with NO to form CO2 and N2.

2CO+2NO->2CO2+N2 ΔH° =-747kj

When 8.74 grams of CO(g) react with excess NO(g),______ kJ of energy are__________(evolved or absorbed)

37. Given the standard enthalpy changes for the following two reactions: (1) Ni(s) + Cl2(g)NiCl2(s)...... ΔH° = -305.3 kJ (2) Fe(s) + Cl2(g)FeCl2(s)......ΔH° = -341.8 kJ what is the standard enthalpy change for the reaction: (3) Ni(s) + FeCl2(s)NiCl2(s) + Fe(s)......ΔH° = ______kJ

38. The standard enthalpy change for the following reaction is 103 kJ at 298 K.

CCl4(g) C(s,graphite) + 2 Cl2(g) ΔH° = 103 kJ

What is the standard enthalpy change for this reaction at 298 K?

C(s,graphite) + 2 Cl2(g) CCl4(g)

_____kJ

39. A chemical reaction is run in which 330 Joules of work is done on the system and the internal energy changes by + 1080 Joules. Calculate q for the system. q =_____ Joules

40. Expressing amounts of energy in different energy units is necessary to solve many chemistry problems. For practice, complete the following table.

The Joule (J) is the SI unit of energy. 1 calorie (cal) = 4.184 J; 1 kcal = 1000 cal

J	kJ	kcal
676
	0.978
		0.217

41. Expressing amounts of energy in different energy units is necessary to solve many chemistry problems. For practice, complete the following table.

The Joule (J) is the SI unit of energy. 1 calorie (cal) = 4.184 J

J	cal	kJ
676
	115
		0.690

42. What is the energy change when the temperature of 11.4 grams of solid platinum is decreased from 38.6 °C to 20.5 °C ? Answer:______ Joules.

43. State whether the potential energy of the underlined object increases or decreases as a result of the change described.

a person climbs a flight of stairs	Increases or decreases
a skier skis from the top to the bottom of a hill	Increases or decreases
a magnet is pulled off of a refrigerator	Increases or decreases

44. The standard enthalpy change for the following reaction is -220 kJ at 298 K.

Cu(s) + Cl2(g) CuCl2(s) ΔH° = -220 kJ

What is the standard enthalpy change for the reaction at 298 K?

CuCl2(s) Cu(s) + Cl2(g)

________ kJ

45. An automobile engine provides 637 Joules of work to push the pistons and generates 2331 Joules of heat that must be carried away by the cooling system. Calculate the change in the internal energy of the engine. E = _______Joules

46. How much energy is required to raise the temperature of 11.0 grams of gaseous nitrogen from 20.9 °C to 39.6 °C ? Answer:_______ Joules.

47. The following thermochemical equation is for the reaction of NH4NO3 to form N2O and H2O.

NH4NO3N2O+2H2O ΔH°=-35.9kj

How many grams of NH4NO3 would have to react to produce 10.4 kJ of energy?

_________grams

48. Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H2(g)C4H10(g)...... ΔH° = -125.6 kJ (2) C2H4(g)2C(s) + 2H2(g)......ΔH° = -52.3 kJ what is the standard enthalpy change for the reaction: (3) 2C2H4(g) + H2(g)C4H10(g)......ΔH° = ? __________kJ

49. Given the standard enthalpy changes for the following two reactions:

(1) 2Pb+O22PbO ΔH° = -434.6 kj

(2) Pb+Cl2PbCl2 ΔH° =-359.4kj

what is the standard enthalpy change for the reaction:

(3) 2PbCl2+O22PbO+2Cl2 ΔH° =?

ΔH° = _______ kJ

50. An automobile engine provides 519 Joules of work to push the pistons. In this process the internal energy changes by –2745 Joules.

Calculate q for the engine. This represents the amount of heat that must be carried away by the cooling system.

Heat =_______ J

51. A chemical reaction is run in which 454 Joules of heat are generated and 790 Joules of work are done on the system.

Calculate the change in the internal energy of the chemical system.

ΔE =_______ J

52. The following thermochemical equation is for the reaction of Fe with Cl2 to form FeCl3.

2Fe+3Cl22FeCl3 ΔH=-799kj

How many grams of Fe would have to react to produce 100 kJ of energy?

________grams

53. The following thermochemical equation is for the reaction of hydrogen sulfide(g) with water(l) to form hydrogen(g) and sulfur dioxide(g).

H2S(g) + 2H2O(g)3H2(g) + SO2(g) Δ H = 207 kJ

When 10.4 grams of hydrogen sulfide(g) react with excess water(l),______kJ of energy are _________ (evolved or absorbed)

54. Given the standard enthalpy changes for the following two reactions:

(1) N2+2O2N2O4 Δ H=9.2kj

(2) 2N2O2N2+O2 Δ H=-164.2kj

What is the standard enthalpy change for the following reaction?

(3) 2N2O+3O22N2O4 Δ H=?

Standard enthalpy change = ________ kJ

55. Given the standard enthalpy changes for the following two reactions:

(1) N2+O22NO Δ H=181.8kj

(2) N2+2O2N2O4 Δ H=9.2kj

What is the standard enthalpy change for the following reaction?

(3) 2NO+O2N2O4 Δ H=?

Standard enthalpy change =_______ kJ

56. Given the standard enthalpy changes for the following two reactions:

(1) 2Ni+O22NiO Δ H=-479.4kj

(2) 2Zn+O22ZnO Δ H=-696.6kj

What is the standard enthalpy change for the following reaction?

(3) NiO+ZnNi+ZnO Δ H=?

Standard enthalpy change =_________ kJ

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