Homework 1due 9/4/241. You are studying a reaction in which compounds A and B react to make compoundC (A+B C). You have measured the change in each compound over the sametime period and in the same reaction conditions. Using this, give the balancedchemical equation for the reaction.A[C]A[B]=A[A] -0.833 M/s= -0.278 M/s= 1.111 M/sAtAtAt

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Answered: Homework 1 due 9/4/24 1. You are…

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter9: Chemical Reactions

Section: Chapter Questions

Problem 9.57EP: The characteristics of four reactions, each of which involves only two reactants, are given. For...

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The characteristics of four reactions, each of which involves only two reactants, are given. For each of the following pairs of the preceding reactions, compare the reaction rates when the two reactants are first mixed by indicating which reaction is faster. a. 1 and 2 b. 1 and 3 c. 1 and 4 d. 2 and 3
Classify each of the reactions according to one of the four reaction types summarized in Table 18.1. (a) C6H12O6(s) + 6 O2(g) 6 CO2(g) + 6 H2O() rH = 673 kj/mol-rxn rS = 60.4 j/K mol-rxn (b) MgO(s) + C(graphite) Mg(s) + CO(g) rH = 490.7 kJ/mol-rxn rS = 197.9 J/K mol-rxn TABLE 18.1 Predicting Whether a Reaction Will Be Spontaneous Under Standard Conditions
Classify each of the reactions according to one of the four reaction types summarized in Table 18.1. (a) Fe2O3(s) + 2 Al(s) 2 Fe(s) + Al2O3(s) rH = 851.5 kj/mol-rxn rS = 375.2 J/K mol-rxn (b) N2(g) + 2 O2(g) 2 NO2(g) rH = 66.2 kJ/mol-rxn rS = 121.6 J/K mol-rxn TABLE 18.1 Predicting Whether a Reaction Will Be Spontaneous Under Standard Conditions
The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative molecular picture that shows what this system looks like after the reactants are mixed in one of the boxes and the system reaches equilibrium. Support your answer with calculations. Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the foll owing equation: A+BC+D a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. b. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
I Review | Constants | Periodic Table The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: Submit Previous Answers v Correct ?NH3(9)+?O2(9)–→?NO(g)+?H2O(g) Correct answer is shown. Your answer 443.34 L was either rounded differently or used a different number of significant figures than required for this part. You have calculated the theoretical volume of O2 needed to produce 18.0 mol of NO. However, in the industrial production of NO, oxygen is added in excess of this amount. Part B What volume of H20(g) is produced by the reaction under the same conditions? Express your answer numerically in litres. • View Available Hint(s) volume of H20 = L
What is true for this chemical reaction: 2SO₂(g) + O₂(g) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. b C d AHrxn > 0; ASrxn > 0 AHrxn 0; ASrxn 0
Directions: Inspect the given reactions very carefully, follow the given step- by-step procedure to balance the equation. 1. I2(g) + Clz(g) + H2O) → HIO3(aq) + HCl(ag) 2. Sn(e) + HNO3(aq) → SnO2(s) + NO21) + H2O«) 3. Al(s) + Ag*(aq) → Al³+ + Ag(s) 4. K(s) + Cr3* (aq) → Cr(s) + K*(aq) 5. Zn(s) + Sn2*(aq) → Zn2*(aq) + Sn(s)
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The same amounts of moles of substance that go into a reaction come out of a reaction. F ostly sunny F1 F2 True F3 11 F4 2 C3 F5 % F6 ☆ Q F7 4- F8 & F9 ★ O False F10 F11 9 F12 A
AB --> A + B is called a decomposition reaction. True False
& 76°F Rain Which is the balanced equation for: Al2O3 + Fe → Fe3O4 + Al 4Al2O3 +9Fe→3Fe3O4 + 8AI 8A1203 + Fe → 2 Fe3O4 + Al O 9Al2O3 + 4Fe → 8Fe304 + 3 Al O 3Al2O3 + 4Fe → Fe304 +8AI O O O Search H
C6H12O6 O + 6O2 →→ 6CO2 + 6H2O + Energy Determine the limiting reactant and how much of that limiting reactant you would need in order to use up all of the non-limiting reactant. Assume you have 25 grams of glucose and 40 grams of oxygen as reactants for the following photosynthesis reaction: A) Glucose is the limiting reactant; You would need .1388 moles of glucose to use up all of the Oxygen (non-limiting reactant). B Glucose is the limiting reactant; You would need .208 moles of glucose to use up all of the Oxygen (non-limiting reactant). C Oxygen is the limiting reactant; You would need 1.25 moles of Oxygen to use up all of the glucose (non-limiting reactant). D Oxygen is the limiting reactant; You would need .8328 moles of Oxygen to use up all of the glucose (non-limiting reactant).

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