Q1. Consider the following reaction: 2 KMnO4(aq) + 3 H₂SO4(aq) + 5 H₂O2(aq) Complete the table below (answers must be values with proper signs and units). A[H₂SO4)/At -0.156 ml L 2-15-1 Δ[02]/ΔΙ 0.260 mol L¹5-1 K₂SO4(aq) + 2 MnSO4(aq) + 8 H₂O(1) + 5 O2(aq) A[KMnO4)/At -0.104 mol L'S Reaction Rate 0.052 HOLL'S!

Q1. Consider the following reaction: 2 KMnO4(aq) + 3 H₂SO4(aq) + 5 H₂O2(aq) Complete the table below (answers must be values with proper signs and units). A[H₂SO4)/At -0.156 ml L 2-15-1 Δ[02]/ΔΙ 0.260 mol L¹5-1 K₂SO4(aq) + 2 MnSO4(aq) + 8 H₂O(1) + 5 O2(aq) A[KMnO4)/At -0.104 mol L'S Reaction Rate 0.052 HOLL'S!

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...

See similar textbooks

Similar questions

1.15 g of an unknown triprotic acid (H3A) is titrated with 2.50 M KOH. It takes 35.5 mL of KOH to reach the equivalence point of the titration. Calculate the molar mass of the unknown acid. H3A (aq) + 3 KOH (aq) → 3 H2O (l) + K3A (aq)
I need help on this question
For the reaction below, Kc = 1.10 × 10⁻⁸. Note Kc is sometimes called K. What is the equilibrium concentration of OH⁻ if the reaction begins with 0.420 M HONH₂? HONH₂ (aq) + H₂O (l) ⇌ HONH₃⁺ (aq) + OH⁻ (aq)
When 2.24 mol KOH is added to 1.00 L of 0.50 M Al(NO3)3. After the aluminum nitrate has reacted with the potassium hydroxide aluminum ion concentration can be expressed with the scientific notation : [Al^3+]= a x 10^-32 M. What is the value of coefficient a? Report one decimal place. Kf= 3.0 x 10^33 for Al(OH)^4-
Calculate the change in pH when 4.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Consult the table of ionization constants as needed. ΔpH= Calculate the change in pH when 4.00 mL of 0.100 M NaOH is added to the original buffer solution. ΔpH=
The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is: Group of answer choices 2H+ (aq) + 2OH- (aq) → 2H2O (l) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq)
ssume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 7.00 ✕ 102 mL of solution and then titrate the solution with 0.153 M NaOH. C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2- M Na+ M H3O+ M OH- M C6H5CO2-
What is the net ionic reaction of HNO3 (a strong acid) with KOH (a strong base)? H2O (0)→ H+ (aq) + OH (aq) H+ (aq) + OH- (aq) → H₂O (1) HNO3(aq) + KOH (aq) → KNO3 (aq) + H₂O (1) K+ (aq) NO3(aq) →>> KNO3(aq)
balance the following chemical equation (if necessary)
Given the value of Kw = 1.0 × 10^-14 at 25 °C.a. Write the relevant chemical reaction.b. Calculate the molarity of OH^- in a solution where the concentration of H+ is 0.4 M at 25 °C.c. Calculate pOH for this solutiond. At 40 °C the ionization constant for water (Kw) is 2.9 × 10^-14. Calculate [H3O^+], [OH^−], pH, and pOH for pure water at 40 °C.
7
A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) ⇒ H+ (aq) + A¯(aq) The equilibrium concentrations of the reactants and products are [HA] A¯] = 3.00 × 10-4 M. Calculate the value of pK₁ for the acid HA. a pK₂: a = = 0.240 M, [H+] = 3.00 × 10−4 M, and