b.At equilibrium the concentrations of the ionized substances are:[C6H5NH2] = 0.0537 mol/L[C6H5NH3+] = 4.79 x 10 mol/L [OH]= 4.79 x 100 mol/LwwwwwwwwwwwwIf this reaction is taking place in a 2.0L container, and 1.5 moles of phenylamine were added to thereaction, what will the new concentrations of the three ionic species be when equilibrium is re-established?C6H5NH2 (aq) +H2O (P) C6H5NH3 (aq)+OH (aq)E'-CE 2. Determine the Ka for the solution from 1b3. Determine the pH for the solution from 1b

Given: at eq.: [C6H5NH2]=0.0537M;0.0537M;[C6H5NH3+]=[OH−]=4.79x10−6MAdded with:…

Answered: b. At equilibrium the concentrations of…

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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The following reaction is important in the manufacture of sulfuric acid. SO2(g) + 1/2 O2(g) SO3(g) At 900 K, 0.0178 mol of SO2 and 0.0214 mol of O2 are sealed in a 1.00-L reaction vessel. When equilibrium is reached, the concentration of SO3 is determined to be 0.0154 M. Calculate Kc for this reaction.
If 0.54 molmol of Br2Br2 and 1.23 molmol of Cl2Cl2 are introduced into a 3.0-LL container at 400 KK, what will be the equilibrium concentration of Br2Br2? If 0.54 molmol of Br2Br2 and 1.23 molmol of Cl2Cl2 are introduced into a 3.0-LL container at 400 KK, what will be the equilibrium concentration of Cl2Cl2? If 0.54 molmol of Br2Br2 and 1.23 molmol of Cl2Cl2 are introduced into a 3.0-LL container at 400 KK, what will be the equilibrium concentration of BrClBrCl?
The reaction below is at equilibrium. Before the reaction began, the concentrations of the reactants were 0.060 M of SO2 and 0.050 M O2. After the equilibrium is reached, the concentration of SO3 is 0.040 M. What is the value of K? 2 SO2(g) + O2(g) <===> 2 SO3(g) 130 2.7 0.0075 8.9 0.38
In air at 25 °C and 1.00 atm, the N₂ concentration is 0.01 M and the O₂ concentration is 0.033 M. The reaction N₂(g) + O₂(g) → 2NO(g) has Kc = 4.8 x 10-³1 at 25 °C. Taking the N₂ and O₂ concentrations given above as initial values, calculate the equilibrium NO concentration that should exist in our atmosphere from this reaction at 38 °C, Kc = 1.0E-29. Make simplifying assumptions in your calculations. (Express your answer in scientific notation.) [NO] = i M
The colorless gas dinitrogen tetroxide decomposes to the brown coloured air pollutant nitrogen dioxide and exists in equilibrium. A 0.125 mol sample of dinitrogen tetroxide is introduced into a 1.00 L container and allowed to decompose at a given temperature. When equilibrium is reached, the concentration of the dinitrogen tetroxide is 0.0750 mol/L. What is the value of K eq for this reaction?
Consider the following equilibrium reaction:CO + H2O ⇌ CO2 + H2; Kc = 1.56If 1.00mol of CO is mixed with 3.00mol of H2O in a 1.00L container, what is the concentration of H2 atequilibrium?
Consider the following chemical reaction. H2(g) + I2(g) ---> 2 HI(g) At equilibrium, the concentration of H2, I2 and HI were found to be .20M, .044M, and .74M respectively. What is the value of Kc for this reaction? Group of answer choices 23 112 62 .0089
One more: H2 + I2 <----> 2HI. If K=50, what is the equilibrium concentration of HI if the initial concentration of HI is 0.10?
For the reaction below, the concentration of HI is 0.210 M and the concentrations of H2, and 12 are both 0.564 M. What must happen for the reaction to reach equilibrium? 2 HI (g) = H₂ (g) + I2 (g) Kc = 7.21 ( Note Kc is sometimes called K.)
Consider the reaction 2 A + B <=> 3C + D. 3.00 moles A and 2.00 moles B was placed in a 2.00 L flask and allowed to reach equilibrium. At equilibrium the concentration of D was 0.500 M. Calculate Kc for this reaction.
Find the equilibrium concentration expression for the following reaction 4HNO3(aq)+3Ag(s)-->3AgNO3(aq)+NO(g)+2H2O
9. For the reaction Hg²+ (aq) + 4 I- (aq) → [HgI4]²+ (aq) the value of Kc = 1.0 × 1030. If the initial concentration of I- is 0.78 M and Hg2+ is 0.010 M, what will be the equilibrium concentrations of Hg²+?

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