question is in the photo Use the following information to answer the next question.Diboron trioxide, B203(s) has many uses including being used as an additive in the production of fibre opticcables. The following reactions can be used in the synthesis of diboron trioxide.H3BO3 (aq) → HBO2(aq) + H2O(1)H2B407 (aq) + H2O(1)H, B40, (aq) → 2B2O;(s) + H2O(1) A,H=+17.9kJA,H = +0.4kJ4HBO2 (aq) A,H = -12.1kJUsing the information above, the enthalpy change for the following reaction2H3BO3 (aq) → B,0;(8) + 3H2O(1)is calculated to bekJ.Record your 3-digit answer. Include sign, do not include units.

From given data you have to calculate the enthalpy change for the reaction: 2 H3BO3 (aq) --->…

Use the following information to answer the next question. Diboron trioxide, B203(s) has many uses including being used as an additive in the production of fibre optic cables. The following reactions can be used in the synthesis of diboron trioxide. H;BO3 (aq) → HB0,(aq) + H2O(1) A,H = +0.4kJ H, B407 (aq) + H,0(1) → 4HBO2 (aq) A,H = -12.1kJ H, B40, (aq) → 2B2O3(s) + H2O(1) A,H = +17.9kJ Using the information above, the enthalpy change for the following reaction 2H3BO3 (aq) → B,0;(8) + 3H2O(1) is calculated to be kJ. Record your 3-digit answer. Include sign, do not include units.

Use the following information to answer the next question. Diboron trioxide, B203(s) has many uses including being used as an additive in the production of fibre optic cables. The following reactions can be used in the synthesis of diboron trioxide. H;BO3 (aq) → HB0,(aq) + H2O(1) A,H = +0.4kJ H, B407 (aq) + H,0(1) → 4HBO2 (aq) A,H = -12.1kJ H, B40, (aq) → 2B2O3(s) + H2O(1) A,H = +17.9kJ Using the information above, the enthalpy change for the following reaction 2H3BO3 (aq) → B,0;(8) + 3H2O(1) is calculated to be kJ. Record your 3-digit answer. Include sign, do not include units.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.87PAE

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Hydrogen peroxide is used as a cleansing agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes on contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams on contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the action of an acid on an alkaline earth metal peroxide, such as barium peroxide: BaO2(s)+2HCl(aq)H2O2(aq)+BaCl2(aq) What mass of hydrogen peroxide should result when 1.50 g barium peroxide is treated with 25.0 mL hydrochloric acid solution containing 0.0272 g HCI per mL? What mass of which reagent is left unreacted?
Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
4.61 What is actually measured by the octane ratings of different grades of gasoline?
4.13 For the following reactions, determine the value of x. 4C+S84CS2 mol S8 yields x mol CS2 CS2+3O2CO2+2SO2 mol CS2 yields x mol SO2 N2H4+3O22NO2+2H2O mol O2 yields x mol NO2 SiH4+2O2SiO2+2H2O 1.3103 mol SiH4 yields x mol H2O
89 A number of compounds containing the heavier noble gases, and especially xenon, have been prepared. One of these is xenon hexafluoride (XeF6), which can be prepared by heating a mixture of xenon and fluoride gases. XeF6 is a white crystalline solid at room temperature and melts at about 325 K. A mixture of 0.0600 g of Xe and 0.0304 g of F2 is sealed into a 100.0-mL bulb. (The bulb is heated, and the reaction goes to completion. Then the sealed bulb is cooled back to 20.0°C. What will be the final pressure in the bulb, expressed in torr?
About 5 billion kilograms of benzene, C6H6, are made each year. Benzene is used as a starting material for many other compounds and as a solvent (although it is also a carcinogen, and its use is restricted). One compound that can be made from benzene is cyclohexane, C6H12. C6H6() + 3 H2(g) C6H12() rH = 206.7 kJ/mol-rxn; rS = 361.5 J/K mol-rxn Is this reaction predicted to be product-favored at equilibrium at 25 C? Is the reaction enthalpy- or entropy-driven?
4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Write a balanced equation for the reaction between (a) dihydrogen sulfide and sulfur dioxide gases to form sulfur solid and steam. (b) methane, ammonia, and oxygen gases to form hydrogen cyanide gas and steam. (c) iron(lll) oxide and hydrogen gas to form molten iron and steam. (d) uranium(IV) oxide and hydrogen fluoride gas to form uranium(IV) fluoride and steam. (e) the combustion of ethyl alcohol (C2H5OH) to give carbon dioxide and water.
What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.
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The sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethanol and carbon dioxide gas. Balance the following equation for this reaction of sucrose. C12H22O11(aq) + H2O(l) C2H5OH(aq) + CO2(g)

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