Which of the following elements is being oxidized in the reaction below? Cu (s) + 2AgNO3...
Which element in the following reaction has been reduced? T Cu (s) + 2AgNO3 (aq)2Ag (s)+ Cu(NO3)2 (aq) Copper Nitrogen Silver Oxygen
PartA Identify the reactant that is oxidized in the following reaction. Cu(s) + 2Ag (aq) - Cu-* (aq) + 2Ag(s) View Available Hint(s) O Cu2+(aq) Ag(s) Ag (aq) O Cu(s) Submit < Return to Assignment Provide Feedback
Which of the following are redox reactions? 2AgNO3(aq) + Cu(s) + Cu(NO3)2(aq) + 2Ag(s) 2Cus(s) + O2(g) + Cu(s) + SO2(g) 2AgNO3(aq) + Na2SO4(aq) + 2NaNO3(aq) + Ag2SO4(s) CO(g) + H2O(g) + CO2(g) + H2(g) CO2(g) + 2H20(1) + H30+(aq) + HCO3(aq)
In the reaction 2AgNO3(aq) + Cu(s) --> 2Ag(s) + Cu(NO3)2(aq), what volume of 1.88M AgNO3(aq) would completely react 20.0g Cu(s)?
Question 29 Consider the reaction: Pb(s) + 2AgNO3(aq) -> Pb(NO3)2(aq) + 2Ag(s) In this reaction silver goes from +1 to 0. We can say that silver is __ because it_electrons. reduced, loses oxidized, loses reduced, gains oxidized, gains
#15
Assign oxidation states to al the elements In this unbalanced reaction: Ag^+(aq) + Cu(s) rightarrow Ag(s) + Cu^2+ (aq) Which substance gets oxidized? Ag^+(aq) Cu(s) Ag(s) Cu^2+(aq) Which substance gets reduced? Balance the redox reaction: Ag^+(aq) Cu(s) Ag(s) Cu^2+(aq)
What is the mass of of silver that can be that can be prepared from 1.00 g of copper metal? Cu(s) + 2AgNO3 (aq) -----> Cu(NO3)(aq)+2Ag(s)
For each reaction, write the chemical formulae of the oxidized reactants in the space provided. Write the chemical formulae of the reduced reactants in the space provided. reactants 0 oxidized: 2 AgNO3(aq) + Mg(s) — 2Ag(s) + Mg(NO3)2(aq) reactants 0 reduced: x ! ? reactants oxidized: 0 Zn(s) + 2AgNO3(aq) → Zn(NO3), (aq) + 2Ag(s) reactants a reduced: D reactants 0 oxidized: D Fel (aq) + Mg(s) → Mgl (aq) + Fe(s) reactants reduced: 0
Which of the following describes the correct net ionic equation for the reaction of copper (II) chloride solution with silver nitrate solution? CuCl2 (aq) + AgNO3 (aq) --> Cu(NO3)2 (aq) + AgCl (s) CuCl2 (aq) + 2AgNO3 (aq) --> Cu(NO3)2 (aq) + 2AgCl (s) Cu2+ (aq) + 2Cl- (aq) + 2Ag+ (aq) + 2NO3- (aq)--> Cu2+ (aq) + 2NO32- (aq) + 2AgCl (s) 2Cl- (aq) + 2Ag+ (aq) --> 2AgCl (s)
Assign oxidation states to all the elements in this unbalanced reaction: Ag+(aq) + Cu(s) --> Ag(s) + Cu2+ (aq) Which substance gets oxidized? Which substance gets reduced? Balance the Redox reaction.