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General Education Common Graded Assignment Chemistry 107
Name
Fundamentals of Chemistry (CHEM 107)
Institution
Date
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You must show all relevant work clearly and completely. Sentences must be used to state
answers on the lines provided. Appropriate use of significant figures and units is required
in order to receive full credit.
1.Write a balanced thermochemical equation with phase labels for the Haber process with
the heat energy as part of the equation. (3 pts)
N (g) + 3H (g) → 2NH (g) + Heat
H= -92.0 kJ
ΔH = -92.6 kJ
2.What is the theoretical yield of ammonia (in grams) if 16.55 grams of nitrogen gas and
10.15 grams of hydrogen gas are allowed to react? (9 pts)
Molecular weight of N
2
28 g/mol
Molecular weight H2 2.016 g/mol
Molecular weight NH
3
17.031 17 g/mol
No of weight of N
2
Mass/ Molar mass
No of weight of N
2
=16.55/ 28.01= 0.59 mol N
2
No of weight of H
2
Mass/ Molar mass
No of weight of H
2
=10.15/ 2.016 = 5.02 mol H
2
of N
2
is the limiting reagent
28 g of N
2
2*17 grams of NH
3
Theoretical yield of ammonia = (16.55*2*17)/28 = 20.0964 grams
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3.Based on your theoretical yield, what is the percent yield of ammonia if only 8.33 grams
of ammonia is produced? (3 pts)
Percentage Yield= actual yield/ theoretical yield
Percentage Yield= (8.33/ 20.0964) * 100= 41.45%
4. How much heat energy (in kJ) will be absorbed or released if 8.33 grams of ammonia is
produced? State whether the energy will be absorbed or released. (4 pts)
Mass, ½ N
2
(g) + 3/2H
2
(g) Nh
3
(g) ∆H° =-46 kj mol-
1
Moles, n= w (g) / Mg (g mol
-1
) 8.33 g/ 17.031 g = 0.4891 mole
Moles= Mass or weight / Molar mass and Mass= moles * molar mass
46 kj mol-
1
* 0.4891 mole= -22.5 kj
Heat energy is released
5. Ammonia gas reacts with aqueous nitric acid to form aqueous ammonium nitrate, a
fertilizer. (a) Write the balanced chemical equation for the reaction, including the physical
states. (2 pts)
NH
3
+ HNO
3
(aq)NH
4
NO
3
(aq)
(b) Write the complete ionic and the net ionic equations for the reaction. (7 pts)
The full ionic equation would be: NH
3
+ H
+
+ NO
3
(aq) NH
4
(aq)
+
+NO
3
(aq)
the net ionic equation would be: NH
3
(g) NH
4
+
(aq)
6. Compare and contrast the positive and negative effects that result from the use of the
Haber process. Discuss the controversy that followed the awarding of the Nobel Prize in
Chemistry to Haber. Based on this discussion, do you think Haber should have been
awarded this prestigious award for his work? Explain. (22 pts)
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In the Haber-Bosch process, there is the synthesis of ammonia from hydrogen and
nitrogen. The Haber process is crucial to making nitrogen fertilizers and was helpful in the 20th
century. There was increased food production from arable land that becomes less fertile.
Increased food supply is crucial to feed the world’s population, and food supply partly explains
the growth in the global population. Nitrogen fertilizers stimulate plant growth in nitrogen-
deficient soils, which improved crop yield and increased soil nitrate levels.
Nitrogen fertilizers cause eutrophication, with water bodies becoming enriched with
nitrates as these fertilizers are soluble in water and eutrophication can cause harmful algae
blooms (Ahmed et al., 2017). Nitrogen fertilizers seep into ground-drinking water, which is one
reason for oxygen deprivation among babies, which causes the “Blue Baby Syndrome” and heart
problems. The Haber process requires heavy use of fossil fuel as well as high pressures and
temperatures.
Haber received the Nobel Prize in Chemistry for the synthesis of ammonia, but he was
involved in Germany’s poison-gas program during WWI. Although Haber was involved in
chemical warfare research, influential in making ammonia produce fertilizers, and deserved the
Nobel.
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References
Ahmed, M., Rauf, M., Mukhtar, Z., & Saeed, N. A. (2017). Excessive use of nitrogenous
fertilizers: an unawareness causing serious threats to environment and human health.
Environmental Science and Pollution Research, 24(35), 26983-26987.

Unformatted Attachment Preview

General Education Common Graded Assignment Chemistry 107 Name Fundamentals of Chemistry (CHEM 107) Institution Date You must show all relevant work clearly and completely. Sentences must be used to state answers on the lines provided. Appropriate use of significant figures and units is required in order to receive full credit. 1.Write a balanced thermochemical equation with phase labels for the Haber process with the heat energy as part of the equation. (3 pts) N ₂ (g) + 3H ₂ (g) → 2NH ₃ (g) + Heat ∆H= -92.0 kJ ΔH = -92.6 kJ 2.What is the theoretical yield of ammonia (in grams) if 16.55 grams of nitrogen gas and 10.15 grams of hydrogen gas are allowed to react? (9 pts) Molecular weight of N2→ 28 g/mol Molecular weight H2→ 2.016 g/mol Molecular weight NH3→ 17.031 17 g/mol No of weight of N2→ Mass/ Molar mass No of weight of N2=16.55/ 28.01= 0.59 mol N2 No of weight of H2→ Mass/ Molar mass No of weight of H2=10.15/ 2.016 = 5.02 mol H2 of N2 is the limiting reagent 28 g of N2→ 2*17 grams of NH3 Theoretical yield of ammonia = (16.55*2*17)/28 = 20.0964 grams 3.Based on your theoretical yield, what is the percent yield of ammonia if only 8.33 grams of ammonia is produced? (3 pts) Percentage Yield= actual yield/ theoretical yield Percentage Yield= (8.33/ 20.0964) * 100= 41.45% 4. How much heat energy (in kJ) will be absorbed or released if 8.33 grams of ammonia is produced? State whether the energy will be absorbed or released. (4 pts) Mass, ½ N2 (g) + 3/2H2 (g)→ Nh3 (g) ∆H° =-46 kj mol-1 Moles, n= w (g) / Mg (g mol-1)→ 8.33 g/ 17.031 g = 0.4891 mole Moles= Mass or weight / Molar mass and Mass= moles * molar mass 46 kj mol-1 * 0.4891 mole= -22.5 kj Heat energy is released 5. Ammonia gas reacts with aqueous nitric acid to form aqueous ammonium nitrate, a fertilizer. (a) Write the balanced chemical equation for the reaction, including the physical states. (2 pts) NH3 + HNO3 (aq)→NH4NO3 (aq) (b) Write the complete ionic and the net ionic equations for the reaction. (7 pts) The full ionic equation would be: NH3 + H+ + NO3− (aq) → NH4 (aq)+ +NO3− (aq) the net ionic equation would be: NH3 (g) →NH4+(aq) 6. Compare and contrast the positive and negative effects that result from the use of the Haber process. Discuss the controversy that followed the awarding of the Nobel Prize in Chemistry to Haber. Based on this discussion, do you think Haber should have been awarded this prestigious award for his work? Explain. (22 pts) In the Haber-Bosch process, there is the synthesis of ammonia from hydrogen and nitrogen. The Haber process is crucial to making nitrogen fertilizers and was helpful in the 20th century. There was increased food production from arable land that becomes less fertile. Increased food supply is crucial to feed the world’s population, and food supply partly explains the growth in the global population. Nitrogen fertilizers stimulate plant growth in nitrogendeficient soils, which improved crop yield and increased soil nitrate levels. Nitrogen fertilizers cause eutrophication, with water bodies becoming enriched with nitrates as these fertilizers are soluble in water and eutrophication can cause harmful algae blooms (Ahmed et al., 2017). Nitrogen fertilizers seep into ground-drinking water, which is one reason for oxygen deprivation among babies, which causes the “Blue Baby Syndrome” and heart problems. The Haber process requires heavy use of fossil fuel as well as high pressures and temperatures. Haber received the Nobel Prize in Chemistry for the synthesis of ammonia, but he was involved in Germany’s poison-gas program during WWI. Although Haber was involved in chemical warfare research, influential in making ammonia produce fertilizers, and deserved the Nobel. References Ahmed, M., Rauf, M., Mukhtar, Z., & Saeed, N. A. (2017). Excessive use of nitrogenous fertilizers: an unawareness causing serious threats to environment and human health. Environmental Science and Pollution Research, 24(35), 26983-26987. Name: Description: ...
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