2. What is the K, of the following reaction? 280) + Og) = 2SO with concentration SO = 0.2MO) = 0.5MSO) = 0.7 M Also, What is the K, of this reaction? At room temperature? 3. For the same reaction, the differing concentrations: SO%) = 0.1 M0% = 0.3 M SOie) = 0.5 M Would this go towards to product or reactant? Activate Windows

2. What is the K, of the following reaction? 280) + Og) = 2SO with concentration SO = 0.2MO) = 0.5MSO) = 0.7 M Also, What is the K, of this reaction? At room temperature? 3. For the same reaction, the differing concentrations: SO%) = 0.1 M0% = 0.3 M SOie) = 0.5 M Would this go towards to product or reactant? Activate Windows

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter13: An Introduction To Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 13.12QAP: The equilibrium constant for the reaction 2CrO42+2H+Cr2O72+H2O is 4.2 1014. The molar...

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Reaction: CrO42-(aq)+2H+(aq) <--> Cr2O72-(aq)+H2O(l) YELLOW ORANGE If sulfuric acid (H2SO4) is added to this solution, will a color change be observed? If so, how does the addition of sulfuric acid result in a color change? Explain your reasoning by showing the effect of the addition of H2SO4 on the equilibrium for the reaction.
Complete this sentence based on what you’ve learned above: If CO2 levels increase, the reaction will run _______________ (toward/away from) CO2 to produce more ___________ (CO2 + H2 O / H+ + HCO3 −). If CO2 levels decrease, the reaction will run _______________ (toward/away from) CO2 to produce more _____________ (CO2 + H2 O / H+ + HCO3 −). CO2+ H2O ⇌ H2CO3 ⇌ H++ HCO3−
Ka of HNO2 in 25 degree is 4.5 x 10^-4. (a) Write the equilibrium chemical reaction corresponding to Ka for nitrous acid (HNO2) at 25°C. (b) Calculate ΔG° for the dissociation of nitrous acid in solution using the given Ka value. (c) What is the value of ΔG at equilibrium? (d) When [H+] = 5.0 × 10^-2 M, [NO2^-] = 6.0 × 10^-4 M, [HNO2] = 0.20 M, what is the value of ΔG?
1.For the aqueous reaction A + B à C + D, the equilibrium concentrations in moles per liter are [A] = 0.002, [B] = 0.005, [C] = 0.00004 [D] = 0.00025 i. What is the equilibrium constant Keq? ii. What is the dissociation constant pK? a. The partial pressure of gas A is 10 ppmv. It has a Henry’s constant for dissolution in water of KH = 0.02
I know the answer is D and that the K1 X K2 X K3 = K. And these cancel out to give D as the product, but won't that be the case for any series of reactions? I wouldn't think that automatically makes D the dominant species but maybe it does. Could you explain how the dominant special could be anything other than the final product in a reaction series based of K values?
A particular reaction, which does not involve H+, has K = 0.529 at 25.0 °C. Calculate the value of ΔG°' for this reaction in kJ mol-1. (R = 8.3145 J mol-1 K-1)
Calculate the value of the equilibrium constant for each of the following reactions in aqueous solution. a) HC2H3O2 + OH- <--> C2H3O2- + H2O b) C2H3O2- + H+ <--> HC2H3O2 c)HCl + NaOH <--> NaCl + H2O and I need an actual value for Kc not just the Kc formula which I already know. thanks.
The kinetics and equilibrium of the decomposition of hy-drogen iodide have been studied extensively:2HI(g)⇌ H₂(g)+I₂(g) (a) At 298 K, K꜀=1.26X10⁻³ for this reaction. Calculate Kₚ.(b) Calculate K꜀ for the formationof HI at 298 K.(c) Calculate ΔH°ᵣₓₙ for HI decomposition from H°f values. (d) At 729 K, K꜀ =2.0X10⁻² for HI decomposition. Calculate ΔHᵣₓₙ for this reaction from the van’t Hoff equation.
calculate ΔG rxn at 325 K for the hypothetical reaction below A2B8 (g) + 3O2 (g) ----> 2AO (g) ΔH°f (kJ/mol) -198 0 23 S° (J/mol•K) 281 205 180
For the reaction: 2SO2 + O2 <------> 2SO3, calculate the equilibrium constant if you start with 1.0M SO2 and 1.0M O2, and the equilibrium constant for the SO3 is 0.925M.
The equilibrium constant for the reaction 2CrO42+2H+Cr2O72+H2O is 4.2 1014. The molar absorptivities for the two principal species in a solution of K2 Cr2 O2 are Four solutions were preparedby dissolving 4.00 10-4, 3.00 10-4, 2.00 10-4,and 1.00 10-4 moles of K2 Cr2 O7 in water and diluting to 1.00 L with a pH 5.60 buffer. Derive theoretical absorbance values (1.00-cm cells) for each solution and plot the data for (a) 345 nm, (b) 370 nm, and (c) 400 nm.
In the text, the equation G=G+RTIn(Q) was derived for gaseous reactions where the quantities in Q were expressed in units of pressure. We also can use units of mol/L for the quantities in Q, specifical.ly for aqueous reactions. With this in mind, consider the reaction HF(aq)H+(aq)+F-(aq) for which Ka = 7.2 104 at 25C. Calculate G for the reaction under the following conditions at 25C. a. [HF] = [H+] = [F] = 1.0 M b. [HF] = 0.98 M, [H+] = [F] = 2.7 102M c. [HF] = [H+] = [F] = 1.0 105 M d. [HF] = [F] = 0.27 M, [H+] = 7.2 104M e. [HF] = 0.52 M, [F] = 0.67 M, [H+] = 1.0 103M Based on the calculated G values, in what direction will the reaction shift to reach equilibrium for each of the five sets of conditions?