ethanol(C2H5OH)and gasoline(assumed to be octane,C8H18) are both used as automobile fuel.if gasoline is selling for $4.50/gal,what...

ethanol(C2H5OH)and gasoline(assumed to be octane,C8H18) are both used as automobile fuel.if gasoline is selling for $4.50/gal,what would the price of ethanol have to be in order to provide the same amount of heat per dollar?The density and ?Hf of octane are 0.7025g/ml and -249.9kJ/mol,respectively and of ethanol are 0.7894g/ml and -277.0 kJ/mol,respectively(1 gal =3.785L)

Expert Solution

queen_honey_blossom answered 2 years ago

Ethanol (C2H5OH) and gasoline (assumed to be all octane, C8H18) are both used as automobile fuel....

Ethanol (C2H5OH) and gasoline (assumed to be all octane, C8H18) are both used as automobile fuel. If gasoline is selling for $2.25/gal, what would the price of ethanol have to be in order to provide the same amount of heat per dollar? The density and ΔH f of octane are 0.7025 g/mL and −249.9 kJ/mol and the density and ΔH f of ethanol are 0.7894 g/mL and −277.0 kJ/mol, respectively. Assume that the products of combustion are CO2(g) and H2O(l)....

Ethanol (C2H5OH) and gasoline (C8H18) are both used as automobile fuel. If gasoline is selling for...

Ethanol (C2H5OH) and gasoline (C8H18) are both used as automobile fuel. If gasoline is selling for $2.50/gal, what would the price of ethanol have to be in order to provide the same amount of heat per dollar? Necessary ΔH°f values are found in the table below. The density of octane is 0.7025 g/mL and the density of ethanol is 0.7894 g/mL. 1 gal = 3.785 L. C8H18(l) + 25/2 O2(g) → 8CO2(g) + 9H2O(g) C2H5OH(l) + 3O2(g) → 2CO2(g) +...

Enter your answer in the provided box. Ethanol (C2H5OH) and gasoline (assumed to be all octane,...

Enter your answer in the provided box. Ethanol (C2H5OH) and gasoline (assumed to be all octane, C8H18) are both used as automobile fuel. If gasoline is selling for $3.19/gal, what would the price of ethanol have to be in order to provide the same amount of heat per dollar? The density and ΔH o f of octane are 0.7025 g/mL and −249.9 kJ/mol and the density and ΔH o f of ethanol are 0.7894 g/mL and −277.0 kJ/mol, respectively. Assume...

Consider four possible liquid fuels used in vehicles. • C8H18 Octane - gasoline • C12H26 Dodecane...

Consider four possible liquid fuels used in vehicles. • C8H18 Octane - gasoline • C12H26 Dodecane - diesel • CH3OH ethanol - gasoline additive • CH3NO2 nitromethane - racing fuel Determine the heat released upon combustion with O2 for 15 gallons of each fuel. Hint: Perform the following. 1. Balance the combustion reaction for each fuel. The products are CO2(g), H2O(g); for nitromethane, N produces N2(g) as one of the products. 2. Determine the enthalpy of each combustion reaction. 3....

The combustion of octane C8H18 (a component in gasoline) in the presence of oxygen proceeds according...

The combustion of octane C8H18 (a component in gasoline) in the presence of oxygen proceeds according to the following balanced equation: 2 C8H18 (l) + 25 O2 (g) ----> 16CO2 (g) + 18H2O (l) 0.0500 L of octane (density 0.702 g/mL) was allowed to burn in the presence of 155 g of oxygen gas. The actual yield of water produced in this reaction was 38.4 grams. a. Determine the theoretical yield for the water. b. Determine the percent yield. c....

INTERACTIVE EXAMPLE Constant Volume Calorimetry Octane, C8H18, a primary constituent of gasoline, burns in air: C8H18(ℓ)...

INTERACTIVE EXAMPLE Constant Volume Calorimetry Octane, C8H18, a primary constituent of gasoline, burns in air: C8H18(ℓ) + 12 1/2 O2(g) → 8 CO2(g) + 9 H2O(ℓ) A 1.00-g sample of octane is burned in a constant volume calorimeter. The calorimeter is in an insulated container with 1.20 kg of water. The temperature of the water and the bomb rises from 25.00 °C (298.15 K) to 33.21 °C (306.36 K). The heat required to raise the bomb’s temperature (its heat capacity),...

Octane, C8H18, a primary constituent of gasoline, burns in air: C8H18(ℓ) + 12 1/2 O2(g) →...

Octane, C8H18, a primary constituent of gasoline, burns in air: C8H18(ℓ) + 12 1/2 O2(g) → 8 CO2(g) + 9 H2O(ℓ) A 1.00-g sample of octane is burned in a constant volume calorimeter. The calorimeter is in an insulated container with 1.20 kg of water. The temperature of the water and the bomb rises from 25.00 °C (298.15 K) to 33.21 °C (306.36 K). The heat required to raise the bomb’s temperature (its heat capacity), Cbomb, is 837 J/K. The...

The complete combustion of octane, a component of gasoline, proceeds as follows: 2 C8H18+25 O2 produces...

The complete combustion of octane, a component of gasoline, proceeds as follows: 2 C8H18+25 O2 produces 16 CO2+18 H20 How many moles of O2 are needed to burn 1.50mol of C8H18? Octane has a density of 0.692g/ml at 20 degrees celsius . How many grams of O2 are required to burn 15.0gal of C8H18?

A gasoline mixture containing 60.0% by weight octane (C8H18) and 40.0% by weight hexane (C6H14) has...

A gasoline mixture containing 60.0% by weight octane (C8H18) and 40.0% by weight hexane (C6H14) has a density of 0.660 g mL–1. Calculate the number of cubic meters of air at STP drawn through the carburetor when one imperial gallon of this gasoline is combusted in an automobile engine, assuming complete combustion of the fuel to carbon dioxide and water vapor. Air contains 21.0% by volume of oxygen. One pound (lb) = 453.59 g; one imperial gallon (IG) of water...

The automobile fuel called E85 consists of 85% ethanol and 15% gasoline. E85 can be used...

The automobile fuel called E85 consists of 85% ethanol and 15% gasoline. E85 can be used in so-called flex-fuel vehicles (FFVs), which can use gasoline, ethanol, or a mix as fuels. Assume that gasoline consists of a mixture of octanes (different isomers of C8H18 ), that the average heat of combustion of C8H18(l) is 5400 kJ/mol , and that gasoline has an average density of 0.70 g/mL . The density of ethanol is 0.79 g/mL . A. How many gallons...

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