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Eqation: 2I^-(aq) + 2NO2^-(aq) + 4H^+(aq) ---> I2(aq) + 2NO(aq) + 2H2O(l) 1. MI*V1 - M2*V2...
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...
answer number three please using the equation provided. I dont
understand. thanks!
21'(aq) + 2NO2 (aq) + 4H(aq) - 12(aq) + 2NO(aq) + 2H2O(1) [Eq. 3] (Note from this equation, that in the experiment, the number of moles of iodide ion present is twice the number of moles of iodine that will be determined by the absorbance measurements. That is, the mole ratio of 12:I" is 1:2. You will not need to account for this mole ratio explicitly, if you...
Cu(s) + 4HNO3 --> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) Cu2+(aq) + 4NH3(aq) --> [Cu(NH3)4]2+(aq) a. For each reaction, identify the oxidation number for each of the elements on both sides of the equation. b. Which of the reactions above is a redox reaction? Explain. c. Identify the element that is being reduced and the one that is being oxidized in the redox reaction. d. Identify the strong oxidizing agent and strong reducing agent in the redox reaction.
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Problem 2 (22 points): Consider the overall balanced redox reaction: 2V0;(aq) + 4H+ (aq) + Zn(s) + 2V02+(aq) + 2H2O(l) + Zn2+ (aq) a. (3 points) Which element is being oxidized? Specify the initial and final oxidation states. b. (3 points) Which element is being reduced? Specify the initial and final oxidation states. c. (3 points) Represent the voltaic cell setup for this reaction using line notation. d. (3 points) Assume this voltaic cell uses a salt...