Question 4A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO, and oxygen,0, shown here. At high temperatures, the rate of formation of SO, is higher, but the equilibrium amount (concentration or partialpressure) of SO, is lower than it would be at lower temperatures. The balanced reaction equation is 2S0, (g) +0,(g) → 2SO,(g)What does the equilibrium constant for this reaction do as the temperature increases?A Remains the sameIncreasesDecreasesResetsQuestion 5For a precipitation reaction to be useful in a gravimetric analysis, the product of the reaction must be insoluble.TrueB) FalseQuestion 6Analysis of the gases in a sealed reaction vessel containing NH3, N2, and H2 at equilibrium at 400° C established the concentrationof N2 to be 1.2 M and the concentration of H, to be 0.24 M.N,(g) + 3H,(g) =2NH,(g)K¸=0.50 at 400° C_ What is the equilibrium molar concentration of NH, ?A0.091B) 0.00910.00830.24

Equilibrium constant of an equilibrium reaction is given by aA + bB ↔cC +dDKeq = [C]c[D]d[A]a[B]b

A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO, and oxygen, 02, shown here. At high temperatures, the rate of formation of SO, is higher, but the equilibrium amount (concentration or partial pressure) of SO, is lower than it would be at lower temperatures. The balanced reaction equation is 2SO,(g) + O,(g) → 250,(g) . What does the equilibrium constant for this reaction do as the temperature increases? A Remains the same B Increases Decreases Resets

A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO, and oxygen, 02, shown here. At high temperatures, the rate of formation of SO, is higher, but the equilibrium amount (concentration or partial pressure) of SO, is lower than it would be at lower temperatures. The balanced reaction equation is 2SO,(g) + O,(g) → 250,(g) . What does the equilibrium constant for this reaction do as the temperature increases? A Remains the same B Increases Decreases Resets

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 10CR: . Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why...

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2:25 1 Question 17 of 25 Submit Consider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled 0.0560 mol O, and 0.200 mol N20 and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Determine the concentrations of all species and then calculate the value of Kc for this reaction. 2 N20(g) + 3 O2(g) =4 NO2(g) 1 2 Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. 2 N20(g) + 3 O2(g) = 4 NO2(g) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190 0.0410 0.0710 0.0360 0.180
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