Energy/Phases of Matter /Equilibrium Review Game

Pick A Number 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40

Question 1 2 SO2 (g) + O2 (g) ) 2 SO3 (g) + heat   Adding what compound would shift the equilibrium to the left? a. SO2 b. O2 c. SO3 d. none of the above

Question 1 2 SO2 (g) + O2 (g) ) 2 SO3 (g) + heat   Adding what compound would shift the equilibrium to the left? Answer: c. SO3 Adding a compound on the right will make the equilbrium shift in the opposite direction. Return

Question 2 Which of the following best describes sublimation? F A solid melting to a liquid G A solid melting to a liquid, which then evaporates H The movement of gaseous particles so that they fill the space they occupy J A solid forming a gas

Question 2 Which of the following best describes sublimation? Answer: J A solid forming a gas Sublimation is the direct conversion of solid to gas. Return

Question 3 Standard atmospheric pressure is 101.3 kPa. According to the graph, which of these four liquids boils at the lowest temperature? A 1 B 2 C 3 D 4

Question 3 Standard atmospheric pressure is 101.3 kPa. According to the graph, which of these four liquids boils at the lowest temperature? Answer: A 1 The boiling point is the temperature where vapor pressure = atmospheric pressure. At any pressure, line 1 is at the lowest temperature Return

Question 4 Between points 2 and 3, energy is being used to — A melt ice B heat water C evaporate water D heat water vapor

Question 4 Between points 2 and 3, energy is being used to — Answer: A melt ice When energy is being added with no change in temperature, a phase change is occuring. This is at 0oC, so this is melting ice. Return

Question 5 The amount of energy needed to raise one gram of a substance one degree Kelvin is a characteristic property known as — A heat of formation B heat of vaporization C molar heat of fusion D specific heat capacity

Question 5 The amount of energy needed to raise one gram of a substance one degree Kelvin is a characteristic property known as — Answer: D specific heat capacity Return

Question 6 The energy required to melt a solid into a liquid is called — A heat of vaporization B heat of fusion C cooling curve D triple point

Question 6 The energy required to melt a solid into a liquid is called — Answer: B heat of fusion The energy required to melt a solid into a liquid is heat of fusion The energy required to boil a liquid to gas is heat of vaporization Return

Question 7 Free Point 

Question 7 Free Point  Return

Question 8 Solid magnesium has a specific heat of 1.01 J/g·°C. How much heat is given off by a 20.0 gram sample of magnesium when it cools from 70.0°C to 50.0°C? F 202 J G 404 J H 808 J J 1010 J

Question 8 Solid magnesium has a specific heat of 1.01 J/g·°C. How much heat is given off by a 20.0 gram sample of magnesium when it cools from 70.0°C to 50.0°C? Answer: G 404 J The formula for specific heat capacity is : Energy / (mass x temperature change) 1.01 = Energy / (20.0 g x 20 degrees) Energy = 404 J Return

Question 9 At 100oC, what phase change occurs when the pressure drops from 105 kPa to 5 kPa? A solid to liquid B liquid to vapor C solid to vapor D vapor to liquid

Question 9 At 100oC, what phase change occurs when the pressure drops from 105 kPa to 5 kPa? Answer: B liquid to vapor When plotting the first point (105 kPa, 100oC), it is in the liquid area. The second point (5 kPa, 100oC) is in the vapor area. Return

Question 10 2HCl(g) ↔ H2(g) + Cl2(g) Which condition will cause a shift in the equilibrium of the above reaction? A Double the concentration of reactants and products B Increase the reaction temperature C Reduce the concentration of products and reactants by 10% D Keep the reaction temperature constant

Question 10 2HCl(g) ↔ H2(g) + Cl2(g) Which condition will cause a shift in the equilibrium of the above reaction? Answer: B Increase the reaction temperature The choices with changes in concentration had equal changes in concentration. To shift the equilibrium, one compound would have to be added in a different amount. Keeping the temperature the same wouldn’t change anything. Return

Question 11 What is true about the chemical reaction shown below? C (s) + H2O (l) + 113 k J  CO (g) + H2 (g) A It is a spontaneous reaction B It is an exothermic reaction C It is a synthesis reaction D It is an endothermic reaction

Question 11 What is true about the chemical reaction shown below? C (s) + H2O (l) + 113 k J  CO (g) + H2 (g) Answer: D It is an endothermic reaction Energy (113 kJ) is a reactant. When energy is added to the reaction, the reaction is endothermic. Return

Question 12 The diagram above is a potential energy curve for a reaction. Which number represents the effect of a catalyst on the reaction? A 1 B 2 C 3 D 4

Question 12 The diagram above is a potential energy curve for a reaction. Which number represents the effect of a catalyst on the reaction? Answer: B 2 A catalyst lowers the activation energy , which is the hump in the middle of the reaction coordinate Return

Question 13 The diagram above is a potential energy curve for a reaction. Which number represents the enthalpy of the reaction? A 1 B 2 C 3 D 4

Question 13 The diagram above is a potential energy curve for a reaction. Which number represents the enthalpy of the reaction? Answer A 1 The net energy of the reaction is 1 Return

Question 14 S

Question 14 The reaction is exothermic, so the energy at the end is lower than at the beginning. Return

Question 15 Which of the following occurs when a reaction in a solution is at equilibrium and more product is added to the solution? F Equilibrium shifts to produce more product G Equilibrium shifts to produce more reactant H No change will occur J The reaction will stop

Question 15 Which of the following occurs when a reaction in a solution is at equilibrium and more product is added to the solution? Answer: G Equilibrium shifts to produce more reactant Whenever you add something to one side, the equilibrium shifts the other direction. Return

Question 16 H2O(l) ↔ H2O(g) Water molecules in a sealed jar are in a state of dynamic equilibrium because water vapor molecules — A are condensing at the same rate that others are evaporating B cease to form when the air in the jar becomes saturated C are evaporating faster than they are condensing D form only at high temperatures

Question 16 H2O(l) ↔ H2O(g) Water molecules in a sealed jar are in a state of dynamic equilibrium because water vapor molecules — Answer: A are condensing at the same rate that others are evaporating The amount of water in the jar is not changing. As a result, if water is evaporating, it must be condensing at the same rate. Return

Question 17

Question 17 Answer: G Iron Crystals Iron has the highest melting point. To melt a solid, the intermolecular forces must be broken. As a result, iron has the strongest intermolecular forces. Return

Question 18

Question 18 Answer: B an exothermic reaction Heat is a product, so the overall energy decreased during the reaction. This would be exothermic Return

Question 19 If the heat of fusion of water is 80 cal/g, the amount of heat energy required to change 15.0 grams of ice at 0°C to 15.0 grams of water at 0°C is— A 80 cal B 560 cal C 1200 cal D 2400 cal

Question 19 If the heat of fusion of water is 80 cal/g, the amount of heat energy required to change 15.0 grams of ice at 0°C to 15.0 grams of water at 0°C is— Answer: C 1200 cal 80 cal/g x 15 g = 1200 cal Return

Question 20 Which numbered process represents condensation? F 1 G 2 J 4

Question 20 Which numbered process represents condensation? Answer: G 2 Condensation is gas to liquid 1-evaporation 3-melting 4-freezing Return Return Return

Question 21 Water molecules have the greatest kinetic energy in — A ice at 0°C B water at 373 K C water at 98°C D steam at 150°C

Question 21 Water molecules have the greatest kinetic energy in — A ice at 0°C = 273 K B water at 373 K C water at 98°C =371 K Answer: D steam at 150°C = 423 K Temperature is a measure of average kinetic energy. The highest temperature has the highest kinetic energy Return

Question 22 The total disorder of a system is: A temperature B entropy C enthalpy D vapor pressure

Question 22 The total disorder of a system is: Answer B entropy Return

Question 23 What phase of matter has the highest entropy? A gas B liquid C solid D cannot be determined

Question 23 What phase of matter has the highest entropy? Answer A gas Gas has no fixed volume or shape, so the molecules have the greatest amount of freedom. Return

Question 24 As heat is added to a substance undergoing a phase change, the temperature remains constant because the energy is being used to- a. break covalent bonds b. lower the specific heat capacity c. overcome intermolecular forces d. oppose electron cloud repulsions

Question 24 As heat is added to a substance undergoing a phase change, the temperature remains constant because the energy is being used to- Answer c. overcome intermolecular forces Intermolecular forces must be broken to change phases and this takes energy. The kinetic energy doesn’t increase until the phase change is complete Return

Question 25 Which of the following will have the highest melting point based on intermolecular forces? A H2O B CH4 C CO2 D LiCl

Question 25 Which of the following will have the highest melting point based on intermolecular forces? A H2O (hydrogen bonds) B CH4 (London dispersion) C C2H6 (London dispersion) D LiCl (Answer – Ionic networks – strongest) Return

Question 26 According to the graph above, what happens at the triple point of water? F Only ice and liquid water exist in equilibrium. G Water exists only as a solid. H Water exists only as a gas. J Ice, water vapor, and liquid water exist in equilibrium.

Question 26 According to the graph above, what happens at the triple point of water? Answer: J Ice, water vapor, and liquid water exist in equilibrium. Return

Question 27 Water has several unique properties such as high boiling point, high surface tension, and low vapor pressure. The type of attraction that best accounts for these unique properties is — A dispersion forces B coordinate covalent bonding C hydrogen bonding D ionic bonding

Question 27 Water has several unique properties such as high boiling point, high surface tension, and low vapor pressure. The type of attraction that best accounts for these unique properties is — Answer: C hydrogen bonding Anytime a question is asked about the properties of water, it’s hydrogen bonding Return

Question 28 The intermolecular force caused by temporary dipoles is known as: A London dispersion B Ionic networks C Hydrogen bonding D Covalent bonding

Question 28 The intermolecular force caused by temporary dipoles is known as: Answer A London dispersion Return

Question 29 Which of the following describes a catalyst? a. speeds up a chemical reaction b. is not consumed during a chemical reaction c. lowers the activation energy d. all of the above

Question 29 Which of the following describes a catalyst? Answer d. all of the above Return Return

Question 30 The transfer of energy between objects at different temperatures is known as: A entropy B enthalpy C exothermic D heat

Question 30 The transfer of energy between objects at different temperatures is known as: Answer D heat Return

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