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(a)
Interpretation: The positive factors and concerns of the technique fracking should be given.
Concept introduction:
Fracking or Hydraulic fracturing: The process is a high pressure technique and it is proved to be an unconventional natural gas technology. Using a high pressurized liquid, cracks are created in the rocks which results in the ejection of natural gas and oil.
(b)
Interpretation: The use of ethanol as a fuel is whether a wise choice should be explained. The arguments for and against for this has to be listed.
Concept introduction:
Different forms of energy sources: Renewable energy source and Non-renewable energy source.
Renewable energy resources: The resources which occur by natural process and can be recyclable or replaced. They will be much useful to human beings.
Non-renewable energy resources: The resources which are once used and which cannot be available again within a given amount of time. Energy derived from fossil fuel is an example for non-renewable resource.
Water, food and air are the major examples for renewable energy resources. The use of renewable sources contributes less pollution in the atmosphere and this is the reason for their increase use. Ethanol in gasoline is a renewable form of energy.
Gasoline, coal, diesel, fossil fuel, plastic.. are examples for non-renewable energy resources. The major disadvantages of these resources are they are not renewed and cannot be recycled.
(c)
Interpretation: The development of electric cars and cars using natural gas should be encouraged or not. The advantages and disadvantages to owning this cars has to be explained.
Concept introduction:
Different forms of energy sources: Renewable energy source and Non-renewable energy source.
Renewable energy resources: The resources which occur by natural process and can be recyclable or replaced. They will be much useful to human beings.
Non-renewable energy resources: The resources which are once used and which cannot be available again within a given amount of time. Energy derived from fossil fuel is an example for non-renewable resource.
Water, food and air are the major examples for renewable energy resources. The use of renewable sources contributes less pollution in the atmosphere and this is the reason for their increase use. Ethanol in gasoline is a renewable form of energy.
Gasoline, coal, diesel, fossil fuel, plastic.. are examples for non-renewable energy resources. The major disadvantages of these resources are they are not renewed and cannot be recycled.
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Chapter 20 Solutions
Chemistry & Chemical Reactivity
- A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forwardWhat is incomplete combustion of fossil fuels? Why can this be a problem?arrow_forward4.60 Why are fuel additives used?arrow_forward
- The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forwardAlthough the gas used in an oxyacetylene torch (Figure 5.7) is essentially pure acetylene, the heat produced by combustion of one mole of acetylene in such a torch is likely not equal to the enthalpy of combustion of acetylene listed in Table 5.2. Considering the conditions for which the tabulated data are reported, suggest an explanation.arrow_forwardDefine the terms renewable and nonrenewable as applied to energy resources. Which of the following energy resources are renewable: solar energy, coal, natural gas, geothermal energy, wind power?arrow_forward
- (a) Write the chemical equation for the complete combustion of butane. (b) Why is it not advisable to use a butane stove inside a tent?arrow_forwardThe citizens of the world burn the fossil fuel equivalent of 7 * 1012 kg of petroleum per year. Assume that all of this petroleum is in the form of octane (C8H18) and calculate how much CO2 (in kg) the world produces from fossil fuel combustion per year. (Hint: Begin by writing a balanced equation for the combustion of octane.) If the atmosphere currently contains approximately3 * 1015 kg of CO2, how long will it take for the world’s fossil fuel combustion to double the amount of atmospheric carbon dioxide?arrow_forwardFrom the discussion question from Module 5, recall the chemical equation for the combustion of gasoline (iso-octane, C8H18) is: 2C8H18 + 25O2 ---> 16CO2 + 18H2O This means that 2 moles of iso-octane combine with 25 moles of CO2 to produce 16 moles of CO2 and 18 moles of water. This is important for understanding the impact of fossil fuel use on the atmosphere because burning one mole of fuel adds a lot of CO2. Thinking about this in terms of the stoichiometry, and change in concentration, suppose we had 1.0 mole of iso-octane dissolved in 1.0 m3 of atmosphere. That means the concentration of carbon-containing molecules would be 1 mole per cubic meter. However, ff we burned all that iso-octane and convert the C8H18 into CO2 the concentration of carbon-containing molecules increases. How much does the concentration of carbon-containing molecules increase if 1.0 mole of C8H18 in 1.0 m3 of air is converted into CO2 as shown in the chemical equation above?arrow_forward
- A large sport utility vehicle has a mass of 2.5 * 103 kg. Calculate the mass of CO2 emitted into the atmosphere upon accelerating the SUV from 0.0 mph to 65.0 mph. Assume that the required energy comes from the combustion of octane with 30% efficiency. (Hint: Use KE = 1/2 mv2 to calculate the kineticenergy required for the acceleration.)arrow_forwardWhat are the practices that are considered waste minimization and pollution prevention?arrow_forwardWhat is the role of environmental chemistry in the development of sustainable technologies?arrow_forward
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