2. (20 points) Please consider the reaction below. -1 +2 -1 -2 BrO3- + Br- →...
balance the reaction using the appropriate electrons. H+ or H2O. BrO3-+Br>Br2
The reaction shown below has the rate law: Rate = k[BrO3-][Br-][H+]^2. BrO3-(aq) + 5 Br-(aq) + 6 H+(aq) → 3 Br2(aq) + 3 H2O(l) What is the order of reaction with respect to Br - ?
The following skeletal oxidation-reduction reaction occurs under acidic conditions. Br- + Hg2+ Hg + BrO3- Write the balanced REDUCTION half reaction. (Enter electrons as e-.) Reactants Products
Consider the following reaction in aqueous solution: 5 Br−(aq) + BrO3−(aq) + 6 H+(aq) ---> 3 Br2(aq) + 3 H2O(l) i) The equation that relates the rate expressions for this reaction in terms of the disappearance of Br−, BrO3− and the formation of Br2 and H2O is (Choose the correct letter.): NOTE: { } is being used to represent the molar concentration. A. R = -1/5{ Δ Br - }/ Δ t = -1/1{ Δ BrO 3- }/ Δ t...
Consider the reaction: 5 Br¯ (aq) + BrO3 ¯ (aq) + 6 H+ (aq) → 3 Br2 (l) + 3 H2O (l) The rate of the loss of BrO3 ¯ at a particular temperature is -8.45 x 10-3 M/s. a. Determine rate of loss of Br¯ . b. Determine the rate of loss of H+. ANSWER BOTH A AND B
Question 2 of 15 Submit What is the rate at which Br-(aq) disappears in the reaction below if the rate of disappearance of BrO3- (aq) is 0.020 M/s? BrOz. + 5 Br- + 6 H+ + 3 Br2 + 3H2O
Consider the reaction 5 Br− (aq) + BrO3− (aq) + 6 H+ (aq) → 3 Br2 (aq) + 3 H2O (l) The average rate of consumption of Br− is 1.94 M/s over the first two minutes. What is the average rate of consumption of H+ during the same time interval? Enter your answer numerically in units of M/s.
2. Reaction of hydrogen peroxide to form water and oxygen gas Observations: Reaction Type: Balanced Reaction: (including states) Oxidation States of atoms in reactants Oxidation states of atoms in products 0 H=_ 0 = Substance Oxidized? Substance Reduced? Oxidizing Agent? = Reducing Agent? Number of electrons transferred 3. Reaction of copper metal with aqueous silver nitrate Observations: Reaction Type: Balanced Reaction: (including states) Oxidation States of atoms in reactants Oxidation states of atoms in products Cu = Ag = Substance...
1. 3NiO2 + 2NO+ 4H+ ------------------------3Ni2+ + 2NO3-+ 2H2O In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: name of the element reduced: formula of the oxidizing agent: formula of the reducing agent: 2. 2NO2 + Cu2++ 2H2O--------------------------Cu + 2NO3-+ 4H+ In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and...
Assignment 6.3-Balancing Redox Reactions 1 Balance the following reactions using the oxidation number method (fill in table as wel) a. NaClO+ H2S ? NaCl+ H2SO4 Element Initial Oxidation # Final Oxidation # Reduced or Oxidized? Element initial Oxidation # Final Oxidation # Reduced or Oxidized? K2Cr:07 + SnCl2 + HCl? CrCb + SnCl4 + KCl + H2O Element Initial Oxidation # Final Oodation # Reduced or Oxidized? 2. Balance the following half-reactions. Be sure to balance for atoms first, then...