Question #11:
Which of the following potential energy diagrams represents equation #1? - Equation 1 (Thumbnail One).
- Question 11 Option A (Thumbnail Two).
- Question 11 Option B (Thumbnail Three).
- Question 11 Option C (Thumbnail Four).
- Question 11 Option D (Thumbnail Five).
Question #12:
Use the following information to answer the next question.
1. Methane
2. Ethene
3. Butane
4. Methanol
The order of the compounds shown above when they are listed from least thermally stable to most thermally stable is:
A) 1, 2, 4, 3
B) 2, 1, 3, 4
C) 3, 4, 2, 1
D) 4, 3, 1, 2
Question #13:
Based on the enthalpy of formation of MgO, the energy required to decompose 48.6 g of MgO is: A) 60.3 kJ
B) 301 kJ
C) 603 kJ
D) 725 kJ
Question #14:
Air bags are designed to deploy when a car moving in excess of 18 km/h undergoes a sudden decrease in speed. During the deceleration, an electrical circuit ignites a small amount of explosive powder to cause sodium azide, NaN3(s), to react inside the air bag. The sodium azide rapidly decomposes, producing nitrogen gas, which fills the bag. The equation for this reaction is (Thumbnail Six). The molar enthalpy of formation of sodium azide is:
A) -43.5 kJ/mol
B) -21.8 kJ/mol
C) +21.8 kJ/mol
D) +43.5 kJ/mol
Question #15:
The amount of energy involved when 100 g of This is NaN3(s) decomposes is:
A) 43.5 kJ
B) 1.54 kJ
C) 33.5 kJ
D) 66.8 kJ
Question #16:
Ammonia is produced by the Haber process. This process involves injecting hydrogen and nitrogen into a heated reaction vessel. The overall reaction involved is (Thumbnail Seven). The enthalpy of reaction for the production of ammonia shown above is:
A) +45.9 kJ
B) +91.8 kJ
C) -45.9 kJ
D) -91.8 kJ
Question #17:
An equation that represents an endothermic change is:
A) C2H5OH(l) + 2O2(g) > 2CO2(g) + 3H2O(g)
B) 2C(s) + H2(g) > C2H2(g)
C) C(s) + O2(g) > CO2(g)
D) C2H4(g) > 2C(s) + 2H2(g)
Question #18:
Sulfuric acid is used to dissolve copper ore in many mining operations. Sulfuric acid may be produced on site by burning sulfur and dissolving the products in water. The overall equation for this reaction is (Thumbnail Eight). In this process, the enthalpy of reaction for one mole of sulfuric acid is:
A) +4225.6 kJ
B) +528.2 kJ
C) -528.2 kJ
D) -4225.6 kJ
Question #20:
(Thumbnail Nine)
The (delta)rH for the combustion reaction shown in the graph above is:
A) -951.9 kJ
B) +951.9 kJ
C) -802.3 kJ
D) +802.3 kJ
Question #21:
Use information from your Table of Standard Molar Enthalpies of Formation in your Data Booklet to determine which of the following compounds has the strongest intramolecular bonds. A) HBr (g)
B) HCl (g)
C) HF (g)
D) HI (g)
Question #22:
(Thumbnail Ten)
Use the following information to answer the next question. The reaction between phosphoric acid and lithium hydroxide is shown below. The reaction above can best be described as:
A) endothermic with a negative enthalpy
B) exothermic with a negative enthalpy
C) endothermic with a positive enthalpy
D) exothermic with a positive enthalpy
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