Study Question - Chapter 4 (Stoichiometry)10A. Copper will react with nitric acid (HNO3) to produce copper(II) nitratemolar mass / g.mol-¹(Cu(NO3)2), nitrogen dioxide (NO₂) and water:Cu63.55NO₂46.01Cu(s) + 4HNO3(aq) → Cu(NO3)2 (aq) + 2NO₂(g) + 2H₂O(1)Suppose NO₂ is produced at a percent yield of 85%. What mass (in g) of copper needs to be usedin an excess of HNO3 to experimentally produce 10.0 g of NO₂?(A) 5.9 g Cu(B) 8.1 g Cu(C) 12 g Cu(D) 16 g Cu100

Given,The reaction:percent yield of NO2 = 85 %experimentally produced mass of NO2 = 10.0 g

Study Question - Chapter 4 (Stoichiometry) 10A. Copper will react with nitric acid (HNO3) to produce copper(II) nitrate (Cu(NO3)2), nitrogen dioxide (NO₂) and water: Cu(s) + 4HNO3(aq) → Cu (NO3)2(aq) + 2NO₂(g) + 2H₂O(1) Suppose NO₂ is produced at a percent yield of 85%. What mass (in g) of copper needs to be used in an excess of HNO3 to experimentally produce 10.0 g of NO₂? (A) 5.9 g Cu (B) 8.1 g Cu (C) 12 g Cu molar mass / g-mol-¹ Cu 63.55 NO₂ 46.01 (D) 16 g Cu

Study Question - Chapter 4 (Stoichiometry) 10A. Copper will react with nitric acid (HNO3) to produce copper(II) nitrate (Cu(NO3)2), nitrogen dioxide (NO₂) and water: Cu(s) + 4HNO3(aq) → Cu (NO3)2(aq) + 2NO₂(g) + 2H₂O(1) Suppose NO₂ is produced at a percent yield of 85%. What mass (in g) of copper needs to be used in an excess of HNO3 to experimentally produce 10.0 g of NO₂? (A) 5.9 g Cu (B) 8.1 g Cu (C) 12 g Cu molar mass / g-mol-¹ Cu 63.55 NO₂ 46.01 (D) 16 g Cu

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter6: Chemical Calculations: Formula Masses, Moles, And Chemical Equations

Section: Chapter Questions

Problem 6.75EP: The catalytic converter that is standard equipment on American automobiles converts carbon monoxide...

See similar textbooks

Similar questions

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.
Boron forms an extensive series of compounds with hydrogen, all with the general formula BxHy. To analyze one of these compounds, you burn it in air and isolate the boron in the form of B2O3 and the hydrogen in the form of water. You find that 0.1482 g BxHy gives 0.4221 g B2O3 when burned in excess O2. Determine the empirical I formula of BxHy.
A solution of scandium chloride was treated with silver nitrate. The chlorine in the scandium compound was converted to silver chloride, AgCl. A 58.9-mg sample of scandium chloride gave 167.4 mg of silver chloride. What are the mass percentages of Sc and Cl in scandium chloride? What is its empirical formula?
Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.
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.
Potassium permanganate (KMnO4) solutions are used for the determination of Fe2+ in samples of unknown concentration. As a laboratory assistant, you are supposed to prepare 500 mL of a 0.1000 M KMnO4 solution. What mass of KMnO4, in grams, do you need?
Silicon is produced for the chemical and electronics industries by the following reactions. Give the balanced equation for each reaction. a. SiO2(s)+C(s)arefurnaceElectricSi(s)+CO(g) b. Liquid silicon tetrachloride is reacted with very pure solid magnesium, producing solid silicon and solid magnesium chloride. c. Na2SiF6(s) + Na(s) Si(s) + NaF(s)
The catalytic converter that is standard equipment on American automobiles converts carbon monoxide (CO)to carbon dioxide (CO2) by the reaction 2CO + O2 2CO2 What mass of O2, in grams, is needed to react completely with 25.0 g of CO?
The balanced equation for the reduction of iron ore to the metal using CO is Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g) (a) What is the maximum mass of iron, in grams, that can be obtained from 454 g (1.00 lb) of iron(III) oxide? (b) What mass of CO is required to react with 454 g cot Fe2O3?
You are given a solid mixture of NaNO2 and NaCl and are asked to analyze it for the amount of NaNO2 present. To do so, you allow the mixture to react with sulfamic acid, HSO3NH2, in water according to the equation NaNO2(aq) + HSO3NH2(aq) NaHSO4(aq) + H2O() + N2(g) What is the weight percentage of NaNO2 in 1.232 g of the solid mixture if reaction with sulfa-mic acid produces 295 mL of dry N2 gas with a pressure of 713 mm Hg at 21.0 C?
3.92 Many chemical reactions take place in the catalytic con- verter of a car. In one of these reactions, nitric oxide (NO) reacts with ammonia (NH3) to give nitrogen (N2) and water. Write a balanced equation for this reaction.