• endothermic
• exothermic

• + 160 kJ
• -63 kJ
• - 160 kJ
• -217 kJ
• #### 3.  Which is an example of an endothermic physical reaction?

• a) Ice melting
• b) Combustion
• c) Steam condensing
• d) Photosynthesis
• #### 4.  The following equation shows the formation of magnesium oxide from magnesium metal. Which statement is correct for this reaction?2Mg(s) + O2(g) → 2MgO(s) ΔH = -1204 kJ

• 1204 kJ of energy are released for every mole of magnesium reacted
• 602 kJ of energy are absorbed for every mole of magnesium oxide formed
• 602 kJ of energy are released for every mole of oxygen reacted
• 1204 kJ of energy are released for every two moles of magnesium oxide formed

• 2x + y - 2z
• 4z - 2x - y
• 2x + y - 4z
• 2z - 2x - y

• endothermic
• exothermic
• #### 7.  Does breaking bonds require energy, release energy, or not involve energy at all?

• requires energy to break
• releases energy when broken
• No energy involved

• 1
• 2
• 3

• endothermic
• exothermic
• isothermic
• what?
• #### 10.  How much energy is required to break all of the bonds in the first molecule depicted in the reaction above? (you must include the proper sign for credit)

• +2,826 kJ
• -2826 kj
• +2826
• None of these

• exothermic
• endothermic
• #### 12.  Use the chart to calculate the ΔE\Delta EΔE for the reaction below (include unit): C2H4 + F2 → C2H4F2C_2H_4\ +\ F_2\ \rightarrow\ C_2H_4F_2C2​H4​ + F2​ → C2​H4​F2​

• 549 kJ
• 549k
• -549 kJ
• None of these

• Piper
• Chloe
• Rex
• Fido
• #### 14.  Kuppler went to college to become a teacher. What college did Kuppler attend?

• Rowan University
• University of Pennsylvania
• The College of NJ (TCNJ)
• Stockton College
• #### 15.  Using the reaction & table above, determine the change in energy and whether or not the reaction is endothermic or exothermic:

• -2054 kJ endothermic
• 2045 kJ endothermic
• -2045 kJ exothermic
• 2045 kJ exothermic

• -102
• +102
• +350
• +394

• 3 years
• 5 years
• 9 years
• 10 years
• 15 years
• #### 18.  On the chart reaction diagram above, #4 represents:

• the energy of the reactants
• the energy of the products
• the energy of the intermediates
• the energy change for the reaction
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