balance redox equation number 7 and 11 Cu(s) + - HNO3(aq) => Cu(NO3)2(aq) + _NO2(0) (conc,...
Name Questions Section 1 1. HNO3(aq) + Cu(s) → Cu(NO3)2 (aq) + _NO2(g) + __ H20 (1) net ionic equation: Observation: Reaction Type: What is in the solution after the reaction is complete? What color is the gas that evolved from this reaction? 2. _ Cu(NO3)2 (aq) +_ NaOH(aq) → Cu(OH)2 (5) + _ NaNO3(aq) net ionic equation: Observation: Dark blue and thick Reaction Type: What color and texture is the suspended product in this reaction? What is formed in...
Complete and balance the equations below by ½ reaction method. 6. _ _C _HNO - Cu(NO3)+ NO (dilute acid) Write balanced equation: 7. _Cus+ _ _HNO3) => _ _Cu(NO3)2) + NO2 (cono, acid) Write balanced equation: 8. MnO + CO2) => Costa) + MnO2is) (basic soln.) Write balanced equation:
Balance the equation for the reaction observed: _ Cu(s) + HNO3(aq) → Cu(NO3)2(aq) +_ NO2(g) + H2O(1) 3. Add 40 mL of 3.0 M NaOH (sodium hydroxide) to the solution in your beaker. Write the balanced equation for the reaction observed: 4. Add 2-3 boiling chips to your beaker and carefully heat the solution, while stirring with a stirring rod, just to the boiling point. (Do NOT boil. Have a low flame and keep the beaker well above the flame.)...
balance redox equation in basic solutions 11. NO2- (aq) + MnO4- (aq) + NO3- (aq) + MnO2 (s) Answer:
Cu + HNO3 ---> Cu(NO3)2 + H2O + NO Balance the Equation
identification half-reaction Cu(s)— Cu²+(aq) + 2€ Fe3+ (aq) + >Fe²+ (aq) oxidation reduction (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients.
Consider the unbalanced chemical reaction shown below: Cu(s)+HNO3(aq)→Cu(NO3)2(aq)+NO(g)+H2O(l) The oxidation state of Cu in Cu(s)Cu(s) = The oxidation state of Cu in Cu(NO_3)_2(aq)Cu(NO3)2(aq) = The oxidation state of N in HNO_3(aq)HNO3(aq) = The oxidation state of N in NO(g)NO(g) = The total number of electrons transferred in this reaction is = The sum of the coefficients in the balanced chemical reaction =
1. Balance the three copper reactions: +H20 (1) +NO2 (g) Cu(NO3)2 (aq) i) Cu (s) HNO3 (aq) NANO3 (aq) NaOH (aq) Cu(OH)2 (s) + ii) Cu(NOs)2 (aq) + H2O (1I) CuO (s) iii) Cu(OH)2 (s) 2. In reaction (i), suppose you add 4.0 mL of 6M nitric acid to a sphere of copper metal that weighs 0.65 grams. Which reactant is the limiting reagent? (Show your work)
Balance the following redox reaction in acidic solution: Cu(s)+NO3−(aq)→Cu2+(aq)+NO2(g) Express your answer as a chemical equation including phases.
HNO3 (aq) + Cu (s) + H2(g) + CuNO3 (aq) •Identify what type of reaction it is: precipitation, redox or acid-base. •Balance the above equation. •Write the balanced net ionic equation. d. Indicate the element that has been oxidized and the one that has been reduced. You should also identify the oxidation number (ox #) of each before and after the process. Identify the reducing agent and the oxidizing agent. Element Oxidized: Ox # Reactant: Ox # Product: Element Reduced:...