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 11E
Interpretation Introduction
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The moles of chlorine gas that will react with
Concept introduction:
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Industrial production of nitric acid, which is used in many products including fertilizers and explosives, approaches 10 billion kg per year worldwide. The first step in its production is the exothermic oxidation of ammonia, represented by the following equation.
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
ΔH⁰rxn
= −902.0 kJ
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X.3H2O + Heat --->
X can be any element.
4.Given the balanced chemical equation below, determine the mass of AgCl produced when 11g of Silver nitrate reacts with 15g of Sodium chloride.
AgNO3 + NaCl --> AgCl + NaNO3
_________g AgCl
How many grams of excess reactant remain after the reaction_________ g
Blank 1:
Blank 2:
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Chapter 9 Solutions
Masteringchemistry With Pearson Etext -- Valuepack Access Card -- For Introductory Chemistry: Concepts And Critical Thinking
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- 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.arrow_forwardCarbon 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.arrow_forward3.81 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_forward
- Insoluble AgCl(s) precipitates when solutions of AgNO3(aq) and NaCl(aq) are mixed. AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) rH = ? To measure the energy evolved in this reaction, 250. mL of 0.16 M AgNO3(aq) and 125 mL of 0.32 M NaCl(aq) are mixed in a coffee-cup calorimeter. The temperature of the mixture rises from 21.15 C to 22.90 C. Calculate the enthalpy change for the precipitation of AgCl(s), in kJ/mol. (Assume the density of the solution is 1.0 g/mL and its specific heat capacity is 4.2 J/g K.)arrow_forward4-77 To convert 1 mol of iron(III) oxide to its elements requires 196.5 kcal: How many grams of iron can be produced if 156.0 kcal of heat is absorbed by a large-enough sample of iron(III) oxide?arrow_forwardA rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forward
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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 -hydrogenarrow_forwardCamels store the fat tristearin (C57H110O6) in the hump. As well as being a source of energy the fat is a source of water, because when it is used the reaction below takes place. What mass of water is available from 1000 g of fat? Balance the equation. C57H110O6 (s) + O2(g) → CO2(g) + H2O(l)arrow_forwardWhen in danger, bombardier beetles can fire a hot, toxic mixture of chemicals at their attacker. This mixture contains quinone, C6H4O2, a compound that is formed by the reaction of hydroquinone, CH4(OH)2, with hydrogen peroxide, H2O2. The equation for the overall reaction is: CH4(OH)2(aq) + H2O2(aq) → C6H4O2(aq) + 2H2O(ℓ) Use the following data to calculate the enthalpy change, in kJ mol-1 , for the above reaction. CH4(OH)2(aq) → C6H4O2 (aq) + H2(g) ΔH = +177.4 kJ mol−1 H2(g) + O2(g) → H2O2(aq) ΔH = −191.2 kJ mol−1 H2(g) + ½O2(g) → H2O(g) ΔH = −241.8 kJ mol−1 H2O(g) → H2O(ℓ) ΔH = −43.8 kJ mol−1arrow_forward
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