ENGR_400_Module_5_Assignment

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?

The compound diborane (B2H6) was at one time considered for use as a rocket fuel. Its combustion reaction is B2H6(g) + 3 O2(l) → 2 HBO2(g) + 2 H2O(l) The fact that HBO2, a reactive compound, was produced rather than the relatively inert B2O3 was a factor in the discontinuation of the investigation of the diborane as a fuel. What mass of liquid oxygen (LOX) would be needed to burn 234.4 g of B2H6? Answer in units of g.

4a Assume that worldwide combustion of fossil fuel accounts for an energy use of 500 x 1015 kJ/year. Also, assume that all fossil fuels can be represented by the formula C3H5 with energy content of 32,500 kJ/kg.Finally, assume that air is 79% N2 and 21% O2 , and has a molecular weight of 29 kg/kmol. i. Estimate the annual release of CO2 to the atmosphere by burning fossil fuels, in kg/yr ii. If all that CO2 entered the atmosphere (and none was removed), estimate the increase in atmospheric concentration, in ppm by volume. Assume the atmosphere contains 6.7 x 1018 kg of air.

NIG 2 H₂(g) + O2(g) → 2 H₂O(g) IO AH°--241.8KJ, 促 ASO = -88.85. Assuming AHO=AH and AS-AS, calculate the temperature criterion for spontaneity. Indicate the min. or max temp. required for OROKA spontaneity. T₁S2T=AH HO For this ran, дно

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 = %

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…

Hydrogen gas has the potential for use as a clean fuel inreaction with oxygen. The relevant reaction is2 H2(g) + O2(g) ---->2 H2O(l)Consider two possible ways of utilizing this reaction asan electrical energy source: (i) Hydrogen and oxygengases are combusted and used to drive a generator, muchas coal is currently used in the electric power industry;(ii) hydrogen and oxygen gases are used to generate electricitydirectly by using fuel cells that operate at 85 °C.(a) Calculate ΔH° and ΔS° forthe reaction. We will assume that these values do notchange appreciably with temperature. (b) Based on thevalues from part (a), what trend would you expect forthe magnitude of ΔG for the reaction as the temperatureincreases? (c) What is the significance of the change inthe magnitude of ΔG with temperature with respect to the utility of hydrogen as a fuel? (d) Based on the analysishere, would it be more efficient to use the combustionmethod or the fuel-cell method to generate electricalenergy from…

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).

Refer to the attached photo. Thank you!

Calculate the volume of carbon dioxide gas that is collected. You can assume the pressure in the room is exactly 1atm. Round your answer to 3 significant digits.

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

Please assist me with homework question 5. Thanks in advance

Calculate the theoretical enthalpy of reaction where NH4NO3 (s)  →  NH41+ (aq) +  NO31- (aq).   ΔHrxn: Please show work. ---------------------------- ΔHf (kJ/mol): For NO31- it is  -205.0 kJ/mol For NH41+  it is -132.5 kJ/mol For NH4NO3  it is -365.56 kJ/mol

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?

Balance the following equation by selecting the coefficients in the dropdown boxes.The coefficient for C5H12 isa. 1b. 2c. 3d. 4The coefficient for O2 isa. 1b. 2c. 3d. 4e. 5f. 6g. 7h. 8i. 9j. 10The coefficient for CO2 is a. 1b. 2c. 3d. 4e. 5f. 6g. 7h. 8i. 9j. 10The coefficient for H2O is a. 1b. 2c. 3d. 4e. 5f. 6g. 7h. 8i. 9j. 10

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

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Please help me work out question 11a and 11b.