Everything should be rounded to four decimal places, and all final solutions should be boxed. Vehicle benzole is a 75 percent, 15%, and 10% combination of three lower aromatic hydrocarbons: benzene, toluene, and xylene. It has a caloric value of 41.9 MJ/kg. When benzole is used to power a motor, the exhaust gas contains 10.7 percent CO2 and 1.07 percent CO. Calculate: a. the percentage of excess air; and b. the complete exhaust gas analysis.

Everything should be rounded to four decimal places, and all final solutions should be boxed. Vehicle benzole is a 75 percent, 15%, and 10% combination of three lower aromatic hydrocarbons: benzene, toluene, and xylene. It has a caloric value of 41.9 MJ/kg. When benzole is used to power a motor, the exhaust gas contains 10.7 percent CO2 and 1.07 percent CO. Calculate: a. the percentage of excess air; and b. the complete exhaust gas analysis.

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 38E: Which is the least expensive source of energy in kilojoules per dollar: a box of breakfast cereal...

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Which is the least expensive source of energy in kilojoules per dollar: a box of breakfast cereal that weighs 32 ounces and costs $4.23, or a liter of isooctane (density, 0.69 19 g/mL) that costs $0.45? Compare the nutritional value of the cereal with the heat produced by combustion of the isooctane under standard conditions. A 1.0-ounce serving of the cereal provides 130 Calories.
an important flavor component of vanilla extract is vanillin C8H8O3 molar mass = 152.15 g/mol when vanillin burns in a bomb calorimeter with a heat capacity of 8.60 kJ/°C the temp increases from 25.97°C to 31.18°C. if the heat of combustion of vanillin is -3760 kJ/mol what mass of vanillin (in g) was combusted? answer to two decimal places
Nitrogen oxide (NO) has been found to be a key component in many biological processes. It also can react with oxygen to give the brown gas NO2. When one mole of NO reacts with oxygen, 57.0 kJ of heat is evolved.A. Write the thermochemical equation for the reaction between one mole of nitrogen oxide and oxygen.B. Is the reaction exothermic or endothermic?C. What is  H when 5.00 grams of nitrogen oxide reacts?D. How many grams of nitrogen oxide must react with an excess of oxygen to liberate ten kilojoules of heat?
Given that H2(g)+F2(g)⟶2HF(g) Δ?∘rxn=−546.6kJ 2H2(g)+O2(g)⟶2H2O(l) Δ?∘rxn=−571.6 kJ calculate the value of ΔHrxn∘ for 2F2(g)+2H2O(l)⟶4HF(g)+O2(g) Δ?∘rxn= ?kJ
When copper(II) sulfate pentahydrate (CuSO4·5 H2O) is heated, it decomposes to the dehydrated form. The waters of hydration are released from the solid crystal and form water vapor. The hydrated form is medium blue, and the dehydrated solid is light blue. The balanced equation is CuSO4·5 H2O(s) --> CuSO4(s) + 5 H2O(g) *heat above the arrow If 5.32 g CuSO4·5 H2O is decomposed to CuSO4, predict the mass of the remaining light blue solid.
Calculate the quantity of energy transferred (q), in kJ, by the combustion of 177 mL of acetone (C3H6O)? C3H6O(l) + 4 O2(g) → 3 CO2(l) + 3 H2O(g) ΔHrxn = -1790 kJ Given: The density of acetone is 0.788 g/mL and its molar mass is 58.08 g/mol IMPORTANT: Enter both the sign and the value (no units), using 3 significant figures.
The equation for the reaction of iron and oxygen gas to form rust (Fe2O3)(Fe2O3) is written as4Fe(s)+3O2(g)→2Fe2O3(s)ΔH=1.7×103kJ How many grams of rust form when 300 kJkJ are released? How many kilojoules are released when 2.10 gg of FeFe reacts?
Calculate the enthlapy of reaction (ΔH) in kJ for the reaction:2A + B → E ΔH =?Given these stepwise reactions:A + 2C → D ΔH = -436 kJE → A + D ΔH = -461.9 kJ1/2 B → C ΔH = 775.5 kJReport answer to the tenths place. Do not include units in your answer. Include the correct sign in your answer (+ or -) and do not include a space between the sign and the number.
what is the value of ΔHrxn if the reaction below is reversed? In other words, PCl5 becomes the reactant. Report your answer in kJ to 1 decimal place. PCl3(g) + Cl2(g) → PCl5(g); ΔHrxn = 618.7 kJ
The heat of combustion for C2H6 (30.07 g/mol) is -1559.5 kJ/mol. Calculate the heat of reaction (in kJ) when 8.24 g C2H6 is combusted. Be sure to include the correct sign in your answer (+ or -) and do not put a space between the sign and the number. Do not include units in your answer. Round answer to the hundredths place.
The Bunsen burner in your labs are fueled by natural gas, which is mostly methane, CH4. The thermochemical equations for the combustion of methane (burning in oxygen) is: CH4(g) + 2 O2(g)  CO2(g) + 2 H2O (g) ΔH = – 890.3 kJ Calculate ΔH when: A) 5.00 g CH4 react with an excess oxygen. B) 2 L of O2 at 49 0 C and 782 mm Hg react with an excess of methane.
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.6421 g sample of 2-naphthylacetic acid (C12H10O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.267×103 g of water. During the combustion the temperature increases from 27.50 to 30.60 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter was determined in a previous experiment to be 843.2 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 2-naphthylacetic acid based on these data. C12H10O2(s) + (27/2) O2(g) 5 H2O(l) + 12 CO2(g) + EnergyMolar Heat of Combustion = kJ/mol