Problem is attached!Please and thank you An unknown contagion made of Carbon, Hydrogen, Nitrogen, and Oxygen needs to be identified. A combustion analysis of a 25.00 gsample produced 35.03 g CO:, 4.30 g H:O g, and 7.32 g NO2. Using combustion analysis, determine the correct subscripts and enterthem here, in the order C__H__N_O.type your answer...type your answer..type your answer.type your answer.

Given : The compound is made up of Carbon i.e C, Nitrogen i.e N, oxygen i.e O and hydrogen i.e H.…

An unknown contagion made of Carbon, Hydrogen, Nitrogen, and Oxygen needs to be identified. A combustion analysis of a 25.00 g sample produced 35.03 g CO:, 4.30 g H:O g, and 7.32 g NO:. Using combustion analysis, determine the correct subscripts and enter them here, in the order C_ H_ _N___0_ type your answer. type your answer.. type your answer. type your answer.

An unknown contagion made of Carbon, Hydrogen, Nitrogen, and Oxygen needs to be identified. A combustion analysis of a 25.00 g sample produced 35.03 g CO:, 4.30 g H:O g, and 7.32 g NO:. Using combustion analysis, determine the correct subscripts and enter them here, in the order C_ H_ _N___0_ type your answer. type your answer.. type your answer. type your answer.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section3.9: Composition And Empirical Formulas

Problem 3.22CE: Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a...

See similar textbooks

Similar questions

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.
What is true about the chemical properties of the product? a. The properties are more like chemical A. b. The properties are more like chemical B. c. The properties are an average of those of chemical A and chemical B. d. The properties are not necessarily like either chemical A or chemical B. e. The properties arc more like chemical A or more like chemical B, but more information is needed. Justify your choice, and for choices you did not pick, explain what is wrong with them.
A 100.0-g mixture made up of NaCl03, Na2CO3, NaCl, and NaHCO3 is heated, producing 5.95 g of oxygen, 1.67 g of water, and 14.5 g of carbon dioxide. NaCl does not react under the conditions of the experiment. The equations for the reactions that take place are: 2NaClO3(s)2NaCl(s)+3O2(g)Na2CO3(s)2Na2O(s)+CO2(g)2NaHCO3(s)Na2O(s)+2CO2(g)+H2O Assuming 100% decomposition of NaClO3, Na2CO3, and NaHCO3, what is the composition of the mixture in grams?
Carbon dioxide from the atmosphere weathers, or dissolves, limestone (CaCO3) by the reaction CaCO3(s)+CO2(g)+H2O(l)Ca2(aq)+2HCO3(aq) Obtain H for this reaction. See Table 6.2 for the data.
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
A newspaper article states that biomass has actually been used as an energy source throughout human history. Do you agree or disagree with this statement? Defend your answer.
hat happens to the weight of an iron bar when it rusts? l type='a'> There is no change because mass is always conserved. i>The weight increases. i>The weight increases, hut it the rust is scraped off, the bar has the original weight. i>The weight decreases. stify your choice and, for choices you did not pick, explain what is wrong with them. Explain what it means for something to rust.
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.
Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?
3.50 A test of an automobile engine's exhaust revealed that g of NO2 was emitted in 10 minutes of operation. How many moles of NO2 would this engine release if it were used for a 45-minute commute, assuming that this mea- sured number is representative of the emission under all circumstances?
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.
The space shuttle environmental control system handles excess CO2 (which the astronauts breathe out; it is 4.0% by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets to form lithium carbonate, Li2CO3, and water. If there are seven astronauts on board the shuttle, and each exhales 20. L of air pee minute, how long could clean air be generated if there were 25,000 g of LiOH pellets available for each shuttle mission? Assume the density of air is 0.0010 g/mL.