older. Or import from another browser. Import favorites[Review Topics][References]Some fuel-efficient hybrid cars are rated at 55.0 miles per gallon of gasoline. Calculate the energy used to drive 9.00 miles ifgasoline produces 48.0 kJ/g and the density of gasoline is 0.737 g/cm. (1.00 gal = 3.785 L)Energy =kJ%3DSubmit AnswerRetry Entire Group3 more group attempts remaining640 PM

The amount of gasoline (V) is required to drive the car 9.00 miles is calculated as shown below…

Answered: older. Or import from another browser.…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 123QRT

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Methane, CH4, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy level diagram shown here presents relationships between energies of the fuels and their oxidation products. Use the information in the diagram to answer the following questions. (The energy terms are per mol-rxn.) (a) Which fuel, methanol or methane, yields the most energy per mole when burned? (b) Which fuel yields the most energy per gram when burned? (c) What is the enthalpy change for the conversion of methane to methanol by reaction with O2(g)? (d) Each arrow on the diagram represents a chemical reaction. Write the equation for the reaction that converts methane to methanol.
The Sun supplies about 1.0 kilowatt of energy for each squaremeter of surface area (1.0 kW/m2, where a watt = 1 J/s).Plants produce the equivalent of about 0.20 g of sucrose(C12H22O11) per hour per square meter. Assuming that thesucrose is produced as follows, calculate the percentage ofsunlight used to produce sucrose.12 CO2(g)+ 11 H2O(l)-----> C12H22O11 + 12 O2(g)ΔH = 5645 kJ
Describe chemistry of petrol and diesel ?
The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. 1. What is qH2O in Joules? A. +146.4 B. -146.4 C. -3661 D. +3661 2. What is qdissolution in Joules? A. +146.4 B. -146.4 C. -3661 D. +3661 3. What is the ΔHdissolution in kilojoules per mole? A. +44.866 B. -44.866 C. +1.794 D. -1.794 4. Is the reaction endothermic or exothermic? A. Endothermic B. Exothermic
The costs of petroleum and natural gas have increased dramatically since the early 1970s, and there is some question about their continued long-term availability. List as many alternative energy sources as you can think of, being as creative as you can, and then go back and suggest possible drawbacks to each one.
A 1.0−g sample of a candy bar (which contains lots of sugar and fats!) was burned in a bomb calorimeter. A 3.0°C temperature increase was observed for 1.00 × 103 g of water. The entire candy bar weighed 3.0 ounces (oz). Calculate the fuel value (in Cal) of the sample.
b) Cyclohexene, C6H10 undergoes hydrogenation to produce cyclohexane, C6H12 according to the equation given below : C6H10 (l) + H2 (g)  C6H12 (l) ∆???(C6H10) = -30 kJ/mol ∆???(C6H12) = -3930 kJ/mol i. Calculate the standard enthalpy of hydrogenation, ∆Ho of cyclohexene. ii. Sketch the enthalpy diagram of this reaction
The air has a dry ball temperature of 32 °C and a wet bulb temperature of 24 °C is heated in a heater so that the temperature of the dry ball increases to 90 °C. The air is then passed through the corn kernels pile to dry. air that comes out of the pile of corn kernels to dry. The air that exits the corn kernels is at a dry bulb temperature of 60 °C. then this air is passed to the dehumidifier to reduce its RH to 10 %. Draw the course of the process of changing the air on the psychometric diagram. The airflow rate through the corn kernels pile and dehumidifier was 3.0 m/s and the pile cross-sectional diameter was 0.5 m a. determine the amount of water lost from the pile of corn kernels (in grams of water / second) b. determine the amount of water lost from the air when passing through the dehumidifier (in grams of water / second)
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 was7581.62 kWh over the last calendar year. What mass of carbon dioxide did this solar systemkeep out of the atmosphere during that time, assuming that the energy consumed by this home would otherwise have been supplied solely by coal-burning power plants (note that this isn’t agreat 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 find the heat of combustion of coal:2 C(s) + O2(g)  2 CO(g) H = -222 kJCO(g) + H2(g) + O2(g) …
1. Determine the mass of CO2 produced by burning enough of octane to produce 1.00×10^2kJ of heat. C8H18(l)+25/2O2(g)→8CO2(g)+9H2O(g) ΔH∘rxn=−5074.1kJmol− Express your answer using three significant figures. 2.Which fuel contributes least to the increase in atmospheric CO2 per kJ of heat produced? propane methane octane
The general balanced equation for the combustion reaction of CH4 + O2 -----> CO2 + 2H20 is CH4 (g)+ 2 O2 (g) -> CO2 (g) + 2 H2O (g) what are the bond energies of the balanced equation, draw their lewis structure, then the enthalpy value you get for the equation is the KJ for the balanced equation. This then has to be calculated per gram of fuel.
How many grams of CO2 are produced from burning one gallon of biodiesel(3,311 g of biodiesel)?C19H36O2 + 27O2 ---> 19 CO2 + 18 H2O

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