How many moles of O2 will be formed from 2.00 moles of KCIO, for the followingreaction? Answer to 2 decimal places. The unit for mole is mol.2 KCIO3→ 2 KCI + 3 O2Your Answer:Answerunits

Given balanced reaction: 2 KClO3 → 2 KCl + 3 O2 The number of moles of KClO3 reacted = 2.00 moles.…

Answered: How many moles of O2 will be formed…

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 4.72PAE: 4.72 The picture shown depicts the species present at the start of a combustion reaction between...

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You have seven closed containers, each with equal masses of chlorine gas (Cl2) . You add 10.0 g of sodium to the first sample, 20.0 g of sodium to the second sample, and so on (adding 70.0 g of sodium to the seventh sample). Sodium and chlorine react to form sodium chloride according to the equation 2Na(s)+Cl22NaCl(s) After each reaction is complete, you collect and measure the amount of sodium chloride formed. A graph of your results is shown below. Answer the following questions: a. Explain the shape of the graph. b. Calculate the mass of NaCl formed when 20.0 g of sodium is used. c. Calculate the mass of Cl2 in each container. d. Calculate the mass of NaCl formed when 50.0 g of sodium is used. e. Identify the leftover reactant, and determine its mass for parts b and d above.
You have seven closed containers each with equal masses of chlorine gas (Cl2). You add 10.0 g of sodium to the first sample, 20.0 g of sodium to the second sample, and so on (adding 70.0 g of sodium to the seventh sample). Sodium and chloride react to form sodium chloride according to the equation :math>2Na(s)+Cl2(g)2NaCl(s) ter each reaction is complete, you collect and measure the amount of sodium chloride formed. A graph of your results is shown below. mg src=Images/HTML_99425-9-18ALQ_image001.jpg alt="" align="top"/> swer the following questions: l type='a'> Explain the shape of the graph. lculate the mass of NaClformed when 20.0 g of sodium is used.Calculate the mass of Cl2 , in each container. lculate the mass of NaClformed when 50.0 g of sodium is used. Identify the leftover reactant and determine its mass for parts b and d above.
3.81 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients.
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.
Magnesium ribbon reacts with acid to produce hydro- gen gas and magnesium ions. Different masses of magnesium ribbon are added to 10 mL of the acid. The volume of the hydrogen gas obtained is a measure of the number of moles of hydrogen produced by the reaction. Various measurements are given in the table below. (a) Draw a graph of the results by plotting the mass of Mg versus the volume of the hydrogen gas. (b) What is the limiting reactant in experiment 1? (c) What is the limiting reactant in experiment 3? (d) What is the limiting reactant in experiment 6? (e) Which experiment uses stoichiometric amounts of each reactant? (f) What volume of gas would be obtained if 0.300 g of Mg ribbon were used? If 0.010 g were used?
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.
4.72 The picture shown depicts the species present at the start of a combustion reaction between methane, CH4 and oxygen, O2 (a) What is the limiting reactant? (b) Draw the resulting state after this set of reactants has reacted as far as possible.
Glucose oxidation is a chemical process that provided energy for an organism to carry out all of its regular activities. The equation for the oxidation of glucose (C6H12O6) is: C6H12O6(aq) + 6O2(aq) →6CO2(aq) + 6H2O(ℓ) How many moles of O2 are needed to completely react with 31.94 g of C6H12O6 ? Answer to 2 decimal places.
Given (8.79x10^6) moles of glucose, C6H12O6, calculate the mole of carbon dioxide, CO2, formed upon complete oxidation of the glucose. C6H12O6 + 6 O2 → 6 CO2 + 6 H2O Express your answer in three significant digits as moles. Note: Your answer is assumed to be reduced to the highest power possible.
Propylene is burned with oxygen gas to form carbon dioxide and water vapor. If 20 kg/hr of propylene is reacted, how much oxygen gas in kg/hr is needed (2 decimal places)? Reaction is: C3H6(g)+O2(g)=CO(g)+H2O(g)
1. How many grams of water, H2O, are present in 7.50x1024 molecules of water, H2O? 2. The correct coefficients for the reaction below? ____ N2H4 + _____H2O2 → ____N2 + ____H2O Please type the answer eg; 1 2 3 4 space between the numbers.
Nitric oxide, NO, is made from the oxidation of NH3 as follows: 4NH3 + 5O2 → 4NO + 6H2O When 6.0 moles of NH3 is mixed with 11.1 moles of O2, how many moles of O2 is in excess when the reaction is over? Do not include unit. Keep 1 decimal place in your answer.

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How many moles of O2 will be formed from 2.00 moles of KCIO, for the following reaction? Answer to 2 decimal places. The unit for mole is mol. 2 KCIO3 2 KCl + 3 O2 Your Answer: Answer units