Butane, C4H10, burns to completion with 110% theoretical air. 4.1) What is the actual air-fuel ratio on mass basis. 4.2) What is the actual air-fuel ratio on mole basis. 4.3) What is theoretical air-fuel ratio (mass basis) 4.4) What is theoretical air-fuel ratio (mole basis) 4.5 Determine the equivalence ratio.

Butane, C4H10, burns to completion with 110% theoretical air. 4.1) What is the actual air-fuel ratio on mass basis. 4.2) What is the actual air-fuel ratio on mole basis. 4.3) What is theoretical air-fuel ratio (mass basis) 4.4) What is theoretical air-fuel ratio (mole basis) 4.5 Determine the equivalence ratio.

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter10: Energy

Section: Chapter Questions

Problem 38A

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1. Write the combustion equations for (a) Complete combustion in theoretical air of 1 mol of gasoline, butane C4 H10 (b) Combustion with 21% excess air (c) Combustion with 9% CO in the product 2. Determine the (d) theoretical air-fuel ratio (e) Actual air-fuel ratio
17. A fuel mixture used in the early days of rocketry consisted of two liquids, hydrazine (N2H4) and dinitrogen tetraoxide (N2O4), which ignite on contact to form nitrogen gas and water vapor. How much in grams of the excess reagent is used up when 435.0 g of N2H4 and 718.5 g of N2O4 are mixed? (, MW: N204 = 92.011g/mol, N2H4 = 32.05g/mol, N2 =28.013 g/mol 2N2H4(0) + N2O40) –> 3N2(9) + 4H2O(g)
What mass is grams of potassium chloride is produced if 2.4 moles of potassium chlorate decompose according to the following equation? heat 2KC10;(s)– 2KCI(s) + 30,(g)
The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the D-0 decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 54.0 mL of dioxygen gas are produced by this reaction, at a temperature of 50.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Round your answer to 3 significant digits. APR 24 MacBook Air
Consider the microbial conversion of glucose to L-glutamic acid, as shown below. Assume that initially the bioreactor contains 200 kg of glucose, 15 kg of ammonia and 54 kg of O2. C6H1206 + NH3 +1.5 O2 →C5H9NO4+ CO2 + 3H2O glucose ammonia glutamic acid a) Which reactant is limiting? b) What is the percentage excess of the other reactants? c) If the reaction proceeds to completion, how much of the excess reactants will be left; how much L-glutamic acid will be formed; and what is the extent of reaction ? d) If the reaction proceeds to a point where the conversion of the limiting reactant is 33%, how much of each reactant and product is present at the end, and what is the extent of reaction E ? e) If the reaction proceeds to a point where 35 kg of O2 is left, what is the fractional conversion of glucose? What is the fractional conversion of O2? What is the extent of reaction E ?
is a poisonous gas that was used in World War I and banned afterward. It causes the general destruction of body tissues, resulting in the formation of large water blisters. The chemical formula of mustard gas is C4H8C12S and the chemical equation Mustard gas below describes its production. (C2H4 - ethene), (SCI4 - sulfur dichloride) What type of chemical reaction is given in the equation below? * C2H4 + SCL2(9) - SCl2(g) C4HºC12S(g) O Combination O Combustion O Decomposition O Neutralization Which of the following statement is correct? * Coefficient tell the number of atoms of each element in a molecule Products appear on the left side of the equation O Reactants appear on the right side of the equation. The states of the reactants and products are written in parentheses to the right of each compound.
Detonation of nitroglycerin proceeds as follows:4 C3H5N3O9(l)------>12 CO2(g) + 6 N2(g) + O2(g) + 10 H2O(g)(a) If a sample containing 2.00 mL of nitroglycerin (density =1.592 g/mL) is detonated, how many moles of gas are produced?(b) If each mole of gas occupies 55 L under the conditionsof the explosion, how many liters of gas are produced?(c) How many grams of N2 are produced in the detonation?
6. In one experiment, a mixture of 0.250 mol of methane gas was burned in 1.25 mol of ogen sina sealed container. Find the limiting reactant and calculate the theoretical yield of water produced. 2.34 g of water was actually produced in the experiment, what is the percentage yield? (9) CH,(g) + 02(9) Co,(g) + H20G) Reply... :
b) Calculate the stoichiometric fuel/air mass ratio and product gas composition for the combustion of Hexane in air. (C=12, H=1, O=16, N=14)
The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(11) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(11) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 39.0 mL of dioxygen gas are produced by this reaction, at a temperature of 50.0 °C and pressure of exactly 1 atm, Calculate the mass of mercury(11) oxide that must have reacted. Round your answer to 3 significant digits. 0. 0-0 X
Be sure to amswer all parts. The reaction between alumiaam and iron(lII) axide can generate temperatures approaching 3000°C and is used in welding metaks: 2A1 - Fe;O, - Al;O, +2Fe In one process, 146 g of Al are reacted with 601 g of Fe;O. Calculate the mass (in grams) of Alo, formed, and determine the amount of excess reagent left at the end of the reaction. mass of AlO, fermed: amount of excess reagent left:
(References] Nitrobenzene, C6 H5 NO2, an important raw material for the dye industry, is prepared from benzene, C6 H6 (molar weight 78.1 g/mol), and nitric acid, HNO3 according to the following chemical equation: C6 H6 (1) + HNO3 (1) → C,H5NO2 (1) + H2 O(1) a. When 22.8 g of benzene and an excess of nitric acid are used, what is the theoretical yield of nitrobenzene (molar weight 123.1 g/mol)? Theoretical yield = b. If 32.3 g of nitrobenzene is recovered, what is the percentage yield? Percentage yield = %

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