How many liters of a 0.209M KI solution is needed to completely react with 2.43 g of Cu(NO.), according to the balanced chemical reaction: 2 Cu(NO,),(aq) + 4 KI(aq) - 2 Cul(aq) + 1,(s) + 4 KNO,(aq) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 0.0310 2.43 0.00542 6.022 x 1023 0.209 0.124 187.57 0.0620 166 1 4 g KI M KI mL KI mol Cu(NO,), mL Cu(NO,), mol KI L KI g Cu(NO,), L Cu(NO,), +

1) For each pair of reactants, will there be a reaction? Co(s) + HCl(aq) Cu(s) + HCl(aq) Al(s) + HCl(aq) K(s) + Fe(C₂H30₂) 2 (aq) Reaction No reaction Reaction No reaction V Activity Series

Question 8 of 9 Submit Write the balanced molecular chemical equation for the reaction in aqueous solution for lead(II) nitrate and sodium chloride. If no reaction occurs, simply write only NR. 3C,2- Reset 1 2 3 4 5 6. 7 8 9 + (s) (1) (g) (aq) N NR Na Pb S NO CI • x H2O Tap here or pull up for additional resources

Classify each of the possible reactions according to whether a precipitate will form or will not form. Precipitate forms Na₂CO3(aq) + CuCl₂(aq) → ? CrCl,(aq) + Li,CO,(aq) — ? Answer Bank Na3PO4 (aq) + CoCl₂(aq) → ? No reaction KI(aq) + NaCl(aq) →→→ ? KNO3(aq) + NaCl(aq) →

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The concentration of a Cu* solution is determined by titrating it with a 0.1395 M solution of permanganate. The balanced net ionic equation for the reaction is shown below. MnO, (aq) + 5 Cu*(aq)+8 H3O*(aq) Mn2*(aq) + 5 Cu2*(aq)+12 H,0(1) In one experiment, 21.54 mL of the 0.1395 M MnO, solution is required to react completely with 40.00 mL of the Cu* solution. Calculate the concentration of the Cut solution.

What volume (in mL) of 0.150 M HCI would be required to completely react with 4.30 g of Al in the following chemical reaction? 2 Al(s) + 6 HCI(aq) → 2 AICI, (aq) + 3 H,(g) 1 4 7 +/- MacBook Pro 888 %23 $ % 3 4 7 1 Q W E R Fab K A F lock C V M control option command * C

The coefficients in front of Cr(OH)4⁻ and ClO⁻ in the balanced reaction for basic conditions are:                 Cr(OH)4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq)  Group of answer choices Cr(OH)4⁻ = 2, ClO⁻ = 5 Cr(OH)4⁻ = 3 ClO⁻ = 2 Cr(OH)4⁻ = 2, ClO⁻ = 3 Cr(OH)4⁻ = 8, ClO⁻ = 5   2. All of the following statements regarding electrochemical cells are correct EXCEPT Group of answer choices Electrolytic cells require the addition of electricity. Reduction occurs when electrons are lost. In a galvanic cell, oxidation occurs at the anode. The longer that currect is passed through an electroplating cell, the more metal will plate on the object.