ENGR_400_Module_5_Assignment

Coal-fired power plants emit CO2, which is one of the gases that is of concern with regard to global warming. A technique that power plants can adopt to keep most of the CO2 from entering the air is called CO2 capture and storage (CCS). If the incremental cost of the sequestration process is $0.019 per kilowatt-hour, what is the present worth of the extra cost over a 3-year period to a manufacturing plant that uses 100,000 kWh of power per month? The interest rate is 12% per year compounded quarterly.

From 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?

Consider the balanced reaction 4 A + 4 B → 5C+ 6 D. If 5.577 moles of C (MW = 36.53) are produced, how many grams of A (MW%3D 47.16) are consumed? Report your answer to three decimal places (ignore significant figures).

(a) The atomic weight of carbon is 12, hydrogen is 1 and oxygen is 16, and the formula for the combustion of methane (CH4) is given by : CH4 + 2 O2 –→ CO2 + 2 H2O + energy A mole of methane releases 810 KJ of energy on burning. Calculate the weight of carbon dioxide produced by burning 5kg of methane. Identify an alternative gas for combustion that produces less carbon dioxide than methane and state how it is generated.

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Assume that producing 1 unit of calcium requires 0.2 units of calcium, 0.1 units of hydrogen, and 0.2 units of sea salt; that producing 1 unit of hydrogen requires 0.2 units of calcium, 0.2 units of hydrogen, and 0.1 units of sea salt; and that producing 1 unit of sea salt requires 0.2 units of calcium, 0.1 units of hydrogen, and 0.1 units of sea salt. Find the production schedule that satisfies an external demand for 50 units of calcium, 38 units of hydrogen, and 17 units of sea salt. X = 出 田 曲

The sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area (1 watt=1 J/s). The plants in an agricultural field produce the equivalent of 18 kg of sucrose (C12H22O11) per hour per hectare (1 ha=10,000meters squared). Assuming that sucrose is produced by the reaction 12CO2(g)+11H2O(l)>>>C12H22O11(s)+12O2(g) ?H= 5640kJ calculate the percentage of sunlight used to produce the sucrose – that is, determine the efficiency of photosynthesis in this field. Percent efficiency = %

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A number of companies currently lease solar panels to homeowners to offset the home’s energy use. The total energy production of a certain residential solar system in suburban Maryland was 7581.62 kWh over the last calendar year. What mass of carbon dioxide did this solar system keep out of the atmosphere during that time, assuming that the energy consumed by this home Chapter 5 Worksheet "Chapter 5 Worksheet" by Montgomery College is licensed under CC BY 4.0 would otherwise have been supplied solely by coal-burning power plants (note that this isn’t a great assumption, as Maryland also has a nuclear power plant, solar and wind farms, and Montgomery County incinerates waste to generate electricity)? Keep in mind that power plants are inefficient, and are able to convert on average 33% of the heat generated by the combustion of coal into electricity. Assume that coal can be approximated as C(s) (again, not a great assumption, but sufficient for this problem). Use the following data to…

A large sport utility vehicle has a mass of 2500 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 (C8H18) with 30% efficiency. (Hint: Use KE = ½ mv2 to calculate the kinetic energy required for the acceleration and pay attention to units).

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n 17 of 41 > Consider a cloudless day on which the sun shines down across the United States. If 2751 kJ of energy reaches a square meter (m²) of the United States in one hour, how much total solar energy reaches the entire United States per hour? The entire area of the United States is 9,158,960 km². solar energy per hour: kJ/h 1037 10 A átv

How much oxygen is needed to produce 105.2 kJ via the following reaction?2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l) ΔH=-3120 kJ/molMolar masses: C2H6: 30.07 g/mol; O2: 32.00 g/mol; CO2: 44.01 g/mol; H2O: 18.02 g/mol

It is estimated that the net amount of carbon dioxide fixed by photosynthesis on the landmass of earth is 5.5*1016 g/yr of CO2. Assume that all this carbon is converted into glucose. Calculate the energy stored by photosynthesis on land per year, in KJ. Calculate the average rate of conversion of solar energy into plant energy in megawatts, MW. A large nuclear power plant produces about 103 MW. The energy of how many such nuclear power plants is equivalent to the solar energy conversion?

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Calculate the heat energy (ΔHreaction) produced when 1 mole of ethanol burns to produce CO2 and H2O C2H5H(l) + 3O2 (g) ---> 2CO2 (g) +3H2O (l)

Reaction; CH4 + 2O2→CO2 +2H2O + 806 kJ A) what amount of energy is produced when 250 moles of methane is combusted? B) How many moles of methane will be used to produce 25000 kJ?

What is Eºcell in volts? (C) || (aq) | 12 (s) || Cl₂ (g) | CI (aq) | (C) I₂ (s) + 2 e² → 2 I¯ (aq) Cl₂ (g) + 2 e → 2 C1 (aq) O +0.824 O -0.824 O -1.896 O +1.648 O -1.648 O +1.896 Eº = +0.536 V Eº = +1.360 V

Information collected: Fireworks need a colorant (to make the pretty colors), a propellant (to shoot the firework into the sky), a burst charge (to blow the firework apart), and an oxidizer (provides oxygen for the burst charge reaction). The burst charge can be any of a number of available explosive chemicals. Oxidizers provide oxygen for the fuel to burn. Common oxidizers are chlorate (CIO3¬), carbonate (CO32-), sulfate (SO42–) and nitrate (NO3¬) ions. Usually the colorants are hot, glowing metals. In the flame test for elemental identity, compounds containing strontium ions yield a bright red flame. Copper (II) ion flames are blue. If we mix strontium chlorate with copper (II) chlorate, the firework will be purple! Common propellants used in fireworks contain carbon and sulfur. The "glue" is often dextrin, a cellulosic polymer made from connected units of C6H1206. The Problem In a blue-burst firework, copper (II) chlorate reacts with carbon to make copper (II) chloride and carbon…

_engine.html?ClassID=D1087757335# Caculate the standard enthalpy for the following reaction conducted at 25°C: MgCl2(s) + 2Na(s) → 2NACI(s) + Mg(s) MgCl2(s) -641.8 kJ/mol NaCl -411.0 kJ/mol AH (kJ/mol) Enter

2. Complete the tables from the data saved in your lab book. Use only a sampling of the data for pressures at 1, 3, 6, and 9 atm. Ideal Gas 1 MW=4 g/mol Volume (L) Pressure (atm) PV Product (P x V) Ideal Gas 8 MW= 222 g/mol Volume (L) Pressure (atm) PV Product (P x V) 3. What conclusions can you make about the PV product with Ideal Gas 1, MW = 4 g/mol? please ! I need it on the basis of Boyles law. this is a lab question thankyou.. neeed ans for part 2 and 3

why is lcoe misleading in the comparison of different energy generation technologies