Combustion of hydrocarbons such as pentane (C5H₁2) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid pentane into gaseous carbon dioxide and gaseous water. x10 X 5 ? 2. Suppose 0.460 kg of pentane are burned in air at a pressure of exactly 1 atm and a temperature of 20.0 °C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits. Explanation Check Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A ES

Combustion of hydrocarbons such as pentane (C5H₁2) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid pentane into gaseous carbon dioxide and gaseous water. x10 X 5 ? 2. Suppose 0.460 kg of pentane are burned in air at a pressure of exactly 1 atm and a temperature of 20.0 °C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits. Explanation Check Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A ES

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 84QRT: Oxygen is not normally found in positive oxidation states, but when it is combined with fluorine in...

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Oxygen is not normally found in positive oxidation states, but when it is combined with fluorine in the compound oxygen difluoride, oxygen is in a +2 oxidation state. Oxygen difluoride is a strong oxidizing agent that oxidizes water to produce O2 and HF. OF2(g) + H2O(g) → 2 HF(g) + O2(g) The standard formation enthalpy of oxygen difluoride is 24.5 kJ/mol. Using this information and data from Appendix J, calculate the standard reaction enthalpy for the reaction of oxygen difluoride with water. Table 4.2 Selected Standard Formation Enthalpies, ΔfH°, at 25°C
The combustion of liquid ethanol (C2H5OH)(C2H5OH) produces carbon dioxide and water. After 4.63 mLmL of ethanol (density=0.789g/ml)(density=0.789g/ml) was allowed to burn in the presence of 15.50 gg of oxygen gas, 3.70 mLmL of water (density=1.00g/ml)(density=1.00g/ml) was collected. Determine the theoretical and percent yeild of h2o in the reaction.
Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients.A precipitate forms when aqueous solutions of chromium(II) iodide and potassium carbonate are combined.Be sure to include states such as (s) or (aq).
During photosynthesis, plants convert carbon dioxide and water to glucose (C6H12O6) and oxygen gas. a. Is photosynthesis a source or a sink of a GHG? Explain. b. Write and balance the chemical equation for the photosynthesis c. It is estimated that the amount of CO2 sequestered (removed from the air) by an urban tree is 60.0 kg.4 How much glucose can be produced from 60.0 kg CO2 during photosynthesis?
4.4g KMnO4 is mixed with water and 1.3 of iodine powder is added to the mixture 0.14g of potassium iodide and a few little grams of potassium hydroxide what are the chemical equations of this reaction and the limiting reagent
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C3H5NO33) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. 2. Suppose 67.0L of carbon dioxide gas are produced by this reaction, at a temperature of −6.0°C and pressure of exactly 1atm. Calculate the mass of nitroglycerin that must have reacted. Round your answer to 3 significant digits. = g
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin ( C3H5NO33 ) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. 2. Suppose 10.0L of carbon dioxide gas are produced by this reaction, at a temperature of −11.0°C and pressure of exactly 1atm . Calculate the mass of nitroglycerin that must have reacted. Be sure your answer has the correct number of significant digits.
The reaction of solid calcium fluoride and sulfuric acid produces calcium sulfate solids and gaseous HF. The gas product is dissolved in water to form hydrofluoric acid. Fluorite ore, a source of calcium fluoride, contains 95%wt CaF2 and 5%wt SiO2. In a certain process, the ore is reacted with 93%wt aqueous sulfuric acid, supplied 15% in excess. From this, 95% of the ore dissolves in the acid. Some of the HF formed reacts with the dissolved silica in the reaction: HF reacts with SiO2 to produce H2SiF6 and liquid water. If 60%wt of hydrofluoric acid was formed when hydrogen fluoride (which exits the reactor) is dissolved in water, determine the amount of ore needed to produce one metric ton of acid. Report your answers to one decimal place only.
Cinnabar, (or Cinnabarite) HgSHgS is the common ore of mercury. Because of its mercury content, cinnabar can be tpxoc to human beings; however, because of its red color, it has also been used since ancient times as a pigment. Alchemists produced elemental mercury by roasting cinnabar ore in air: HgS(s)+O2(g) → Hg(l) + SO2(g) The votality and toxicity of mercury make this a hazardous procedure, which likely shortened the life span of many alchemists. Given 100g of cinnabar, a. How much elemtal mercury can be produced from this reaction? b. How much oxygen is required to completely react with the given amount of cinnabar?
(write a balanced chemical equation with accurate states) Liquid methanol (CH3OH) undergoes complete combustion in racecar engines.
Life support systems of spaceships and submarines are designed assuming that averageconsumption of oxygen for 1 person is 1 kg per day. To obtain oxygen, reaction of sodiumperoxide with carbon dioxide exhaled by people is used (RbO2 + CO2 =>). Calculate the mass of sodium peroxide which must be taken on an expedition to provide oxygen to a crew of 4 people for a week.
The manufacture of nitrogen trifluoride is a growing industry, due to its use as a plasma etchant in the semiconductor industry. Nitrogen trifluoride can be synthesized by passing a currentthrough a high-temperature mixture of ammonium fluoride and hydrogen fluoride, withhydrogen gas as a byproduct. In one synthesis, 1.20x103g ammonium fluoride is reacted with1.20x103g hydrogen fluoride to produce 5.00x102g nitrogen trifluoride. What is the limitingeactant, excess reactant, theoretical yield of nitrogen trifluoride, percent yield, and mass ofxcess reactant remaining after the reaction?

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