Masteringchemistry With Pearson Etext -- Valuepack Access Card -- For Introductory Chemistry: Concepts And Critical Thinking
8th Edition
ISBN: 9780134473130
Author: CORWIN
Publisher: PEARSON
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Chapter 9, Problem 12E
Interpretation Introduction
Interpretation:
The numbers of moles of barium metal and nitrogen gas which are required to form
Concept introduction:
A mole of atoms or molecules is described as an amount whose mass corresponds to its gram
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of a catalyst, to produce ammonia.
N2(g)+3H2(g)⟶2NH3(g)
There are four molecules of nitrogen and nine molecules of hydrogen present in the diagram.
When the reaction is complete, how many molecules of NH3 are produced?
molecules of NH3:______
What is the limiting reactant?
-nitrogen
-hydrogen
2NO(g) + O2(g) → 2NO2(g)
You are provided with 4.12 molmol of nitrogen monoxide gas. Using the balanced chemical equation completed in Part A, determine how many moles of oxygen gas are needed to completely react with the nitrogen monoxide gas and how many moles of nitrogen dioxide are formed as a result?
Ammonia and oxygen react to form nitrogen monoxide and water. Construct your own balanced equation to determine the amount of NO and H2O that would form when 2.80 molmol NH3 and 4.64 mol O2 react.
Express the amounts in moles to two decimal places separated by a comma.
Given the chemical equation C4H10 + O2
⟶
⟶
CO2 + H2O, what coefficient is needed in front of C4H10 to produce a balanced equation?
Chapter 9 Solutions
Masteringchemistry With Pearson Etext -- Valuepack Access Card -- For Introductory Chemistry: Concepts And Critical Thinking
Ch. 9 - Prob. 1CECh. 9 - Prob. 2CECh. 9 - Prob. 3CECh. 9 - Prob. 4CECh. 9 - Prob. 5CECh. 9 - Prob. 6CECh. 9 - Prob. 7CECh. 9 - Prob. 8CECh. 9 - Prob. 9CECh. 9 - Prob. 10CE
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- 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.arrow_forward3.50 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?arrow_forwardCarbon disulfide burns in air, producing carbon dioxide and sulfur dioxide. CS2(l)+3O2(g)CO2(g)+2SO2(g);H=1077kJ What is H for the following equation? 12CO2(g)+SO2(g)12CS2(l)+32O2(g)arrow_forward
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- You react nitrogen and hydrogen in a container to produce ammonia, NH3(g). The following figure depicts the contents of the container after the reaction is complete. a Write a balanced chemical equation for the reaction. b What is the limiting reactant? c How many molecules of the limiting reactant would you need to add to the container in order to have a complete reaction (convert all reactants to products)?arrow_forward4.27 Copper reacts with sulfuric acid according to the following equation: 2H2SO4+CuCuSO4+2H2O+SO2 How many grams of sulfur dioxide are created by this reaction if 14.2 g of copper reacts with 18.0 g of sulfuric acid?arrow_forwarda. Write die balanced equation for the combustion of isooctane (C8H18) to produce water vapor and carbon dioxide gas. b. Assuming gasoline is 100.% isooctane, with a density of 0.692 g/mL, what is the theoretical yield of carbon dioxide produced by the combustion of 1.2 1010 gal of gasoline (the approximate annual consumption of gasoline in the United States)?arrow_forward
- One way to remove nitrogen oxide (NO) from smoke-stack emissions is to react it with ammonia. 4NH3(g)+6NO(g)5N2(g)+6H2O(l) Calculate (a) the mass of water produced from 0.839 mol of ammonia. (b) the mass of NO required to react with 3.402 mol of ammonia. (c) the mass of ammonia required to produce 12.0 g of nitrogen gas. (d) the mass of ammonia required to react with 115 g of NO.arrow_forwardUsing each of the following balanced chemical equations, calculate the number of moles of the first listed reactant needed to produce 5.00 moles of CO2. a. C7H16+11O27CO2+8H2O b. CS2+O22SO2+CO2 c. Fe3O4+CO3FeO+CO2 d. 2HCl+CaCO3CaCl2+CO2+H2Oarrow_forward4.8 In an experiment carried out at very low pressure, 13x1015 molecules of H2 are reacted with acetylene, C2H2, to form ethane, C2H6, on the surface of a catalyst. Write a balanced chemical equation for this reaction. How many molecules of acetylene are consumed?arrow_forward
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