Predict the equilibrium concentration of O₂ in the reaction described below by constructing an equilibrium expression for Qc, constructing an ICE table, writing an equilibrium expression for Kc, and solving for the equilibrium concentration. Complete Parts 1-4 before submitting your answer. N₂(g) + O₂(g) = 2 NO(g) Question 4 of 7 2 Qc = 3 NEXT > In a 1.0 L container at high temperature, 0.20 mol N₂ and 0.15 mol O₂ are allowed to react. Set up the expression for Qc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qc to determine the direction of the reaction. 4 =

Predict the equilibrium concentration of O₂ in the reaction described below by constructing an equilibrium expression for Qc, constructing an ICE table, writing an equilibrium expression for Kc, and solving for the equilibrium concentration. Complete Parts 1-4 before submitting your answer. N₂(g) + O₂(g) = 2 NO(g) Question 4 of 7 2 Qc = 3 NEXT > In a 1.0 L container at high temperature, 0.20 mol N₂ and 0.15 mol O₂ are allowed to react. Set up the expression for Qc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qc to determine the direction of the reaction. 4 =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Bookmarks Profiles Tab Window Help 236/quizzes/64048/take Consider again the equilibrium: H2 (g) + 12 (s) A 2HI (g) This reaction is endothermic (absorbs heat). Using Le Chatelier's Principle, you would predict which of the following: O Removing HI as it forms shifts the equilibrium to the left. Adding l2 will increase the equilibrium concentration of HI. None of these predictions are correct. Raising the temperature will decrease the equilibrium constant. If the volume is increased, more HI will be produced.
Suppose a 500. mL flask is filled with 1.5 mol of SO, and 0.20 mol of SO2. This reaction becomes possible: 2 (3) 2S0, (g) + 0,(g) =2SO3(g, Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of 0,. You can leave out the M symbol for molarity. 2 so, 02 so, initial ? change equilibrium olo
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 125 L tank with 20. mol of carbon monoxide gas and 24. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 7.0 mol of carbon monoxide gas, 11. mol of water vapor and 13. mol of carbon dioxide. The engineer then adds another 7.0 mol of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the moles of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. mol
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 25 L tank with 11. mol of carbon monoxide gas and 12. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.9 mol of carbon monoxide gas, 7.9 mol of water vapor and 4.1 mol of hydrogen gas. The engineer then adds another 3.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol
4. The formation of glucose from water and carbon dioxide is an extremely important reaction for life to exist. Plants perform this reaction through the process of photosynthesis, creating the base of the food chain. The UNBALANCED equation is: H₂O (9) CO2 (g) C6H12O6 (s) + O2 (g) At a particular temperature the equilibrium concentrations were found to be: [H₂0] = 7.90x10-2M, [CO₂] = 0.930M, [0₂] =2.40x10-³M. a. Balance the equation. b. Write an expression for Kc- c. Calculate the value of Kc for the reaction at equilibrium.
Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4(g) + H2O(g) 3H2(g) + CO(g). a. Write the equilibrium constant Kc for this reaction. b. How much hydrogen gas is at equilibrium if Kc = 6.3 and the remaining gases have the following concentrations: CH4 = 0.126 M; H2O = 0.242 M; CO = 0.126 M; at a temperature of 760 °C?
2. A reaction is represented by this equation: A(aq) + 2B(aq) = 2C(aq) Ke = 1 × 10³ (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations S1 M, make up two sets of concentrations that describe a mixture of A, B, and C at equilibrium.
For the reaction below, Kc = 1.10 x 10-8. Note Kc is sometimes called K. What is the equilibrium concentration of OH¯ if the reaction begins with 0.140 M HONH,? HONH2 (aq) + H,0 (I) = HONH3* (aq) + ОН (аq)
The reaction 2CO(g) + O2(g) = 2 CO2(g) is known to be exothermic. According to Le Chatelier's principle, how will this reaction's equilibrium be affected if the reaction temperature is increased? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will increase and the reaction will shift to the right. (D) The equilibrium constant will be unchanged, but the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.
Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction? (a) A catalyst is added to the reaction mixture. which will happen? the equilibrium will not shift the equilibrium will shift towards product but keq will not change the equilibrium will shift towards reactant but keq will not change the equilibrium will shift towards product and keq will increase the equilibrium will shift towards reactant and keq will decrease (b) The total pressure of the system is increased by adding a noble gas. (c) Cl2(g) is removed from the system.
The reaction of bromine gas with chlorine gas, shown below, has a Kc of 7.20 at 200 oC. If a closed vessel was charged with the two reactants, each at an initial concentration of 0.50 M, what would be the equilibrium concentration of Cl2(g)?
Be sure to answer all parts. Given the value of the equilibrium constant (K) for equation (a), calculate the equilibrium constant for equation (b). 2 (a) O2(g) S,03(g) K = 8.58 × 10-9 %3D х 10 (Enter your answer in scientific notation.) (b) 302(g) 5 203(g)