Question

Please calculate the net (LHV) and gross (HHV) heat of combustion in kWh/gal for gasoline a....

Please calculate the net (LHV) and gross (HHV) heat of combustion in kWh/gal for gasoline a. Gasoline (C8H18, l), density 6.1 lb/gal

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
What volume of CO2 is produced from combustion of 1.00 gal of gasoline (2.65 kg) during...
What volume of CO2 is produced from combustion of 1.00 gal of gasoline (2.65 kg) during a hot day in August (35 °C) at sea level (1.00 atm barometric pressure)? What volume of O2 from the air was consumed? Assume gasoline is pure isooctane (C8H18).
Gasoline consists primarly of octane, C8H18. Calculate the mass of water, in kilograms, coming from the...
Gasoline consists primarly of octane, C8H18. Calculate the mass of water, in kilograms, coming from the exhaust of a car that takes a trip of 257 miles, in a car that gets 28.2 miles/gallon. Assume complete combustion of the gasoline (octane) with excess O2. 3.97 L = 1.00 galln density of octane = 0.756 g/mL combustion = combustion with oxygen Equation must be displayed as one step, not broken into parts.
1. The combustion of gasoline (C8H18) with excess oxygen produces carbon dioxide and water. -Write a...
1. The combustion of gasoline (C8H18) with excess oxygen produces carbon dioxide and water. -Write a balanced chemical reaction for the combustion of gasoline to yield carbon dioxide and water. -Presuming that a tank of gasoline contains 80 liters and that its density is 0.77 kg/liter, determine how many kg of CO2 are produced for each tank of gasoline burned. Also, the products for octane + O2 should be carbon dioxide and water. Now, you have to write it in...
Calculate the number of grams and pounds of CO2 that result from thecombustion of 1 gallon...
Calculate the number of grams and pounds of CO2 that result from thecombustion of 1 gallon of gasoline (we will assume that gasoline is mostly octane,C8H18). Gasoline has a density of about 0.7g/mL. Hint - Remember to balance thechemical reaction and that combustion uses oxygen gas and heat to generate CO2and water.
Question 4 Part A Using the following equation for the combustion of octane, calculate the heat...
Question 4 Part A Using the following equation for the combustion of octane, calculate the heat of reaction for 100.0 g of octane. The molar mass of octane is 114.33 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ Using the following equation for the combustion of octane, calculate the heat of reaction for 100.0 g of octane. The molar mass of octane is 114.33 g/mole. 2 C8H18 + 25 O2 → 16...
Calculate heat of combustion reaction of 1.0 g of octane: 2 C8H18 + 25 O2 -->...
Calculate heat of combustion reaction of 1.0 g of octane: 2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O The calorimeter contains 1200 g water, and the temperature changes from 25.00 deg C to 33.20 deg C. Heat capacity of bomb is 837 J/deg C.
Using the following equation for the combustion of octane, calculate the heat of reaction for 100.0...
Using the following equation for the combustion of octane, calculate the heat of reaction for 100.0 g of octane. The molar mass of octane is 114.33 g/mole. 2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O   ,deltaH°rxn = -11018 kJ I got- 4820kJ but the answer is 4820kJ. why is the answer positive when the delta h is negative?
Calculate the number of pounds of CO2 released into the atmosphere when a 21.0-gallon tank of...
Calculate the number of pounds of CO2 released into the atmosphere when a 21.0-gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, C8H18, and that the density of gasoline is 0.692 g·mL–1 (this assumption ignores additives). Also assume complete combustion.
The value for the standard heat of combustion, ΔH°combustion, for sucrose, C12H22O11, is -5.65 × 103...
The value for the standard heat of combustion, ΔH°combustion, for sucrose, C12H22O11, is -5.65 × 103 kJ·mol-1. Enter the thermochemical equation for the combustion of 1 mol of sucrose and calculate the value of ΔHf° for this compound (express your answer in scientific notation). The sole products of combustion are CO2(g) and H2O(l).
Using Hess’ Law, compare the heat of combustion of one liter of ethanol with the heat...
Using Hess’ Law, compare the heat of combustion of one liter of ethanol with the heat of combustion of one liter of octane. The density of ethanol is 0.789 g/mL and that of octane is 0.703 g/mL. how do you calculate the number -343.909 kj for CO2 or -241.101 of H2O.. or 200.447kj/mol for C2H4OH? thank you!
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT