Equation 1: X(s)+ NiCl, (aq)Ni(s) + XCl,(aq) Equation 2: X(s) + MgCl, (aq) → no reaction A sample of an unknown solid metal, X(s), is added to a solution of NiCl2 (ag), which results in the formation of Ni(s) and XCI2 (ag). When a sample of X(s) is added to a solution of MgCl, (aq), no changes are observed. The results of the experiment are summarized in equations 1 and 2. Which of the following represents a possible identity of metal X and provides the correct justification? A Cu, because Cu is oxidized more easily than both Mg and Ni. Cu, because Cu is oxidized more easily than Ni but less easily than Mg. C Zn, because Zn is oxidized more easily than both Mg and Ni. Zn because Zn is oxidized more easily than Ni but less easily than Mg.

Equation 1: X(s)+ NiCl, (aq)Ni(s) + XCl,(aq) Equation 2: X(s) + MgCl, (aq) → no reaction A sample of an unknown solid metal, X(s), is added to a solution of NiCl2 (ag), which results in the formation of Ni(s) and XCI2 (ag). When a sample of X(s) is added to a solution of MgCl, (aq), no changes are observed. The results of the experiment are summarized in equations 1 and 2. Which of the following represents a possible identity of metal X and provides the correct justification? A Cu, because Cu is oxidized more easily than both Mg and Ni. Cu, because Cu is oxidized more easily than Ni but less easily than Mg. C Zn, because Zn is oxidized more easily than both Mg and Ni. Zn because Zn is oxidized more easily than Ni but less easily than Mg.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A solution is prepared by dissolving 2.95 g Co2(SO4)3 in enough water to make 1.00 L of red solution; the red color is due to the presence of the cobalt ions. To this solution was added 1.52 g of magnesium powder. A redox reaction occurred, in which the magnesium atoms lose all of their valence electrons and the red color of the solution fades. (a) Write the total reaction that occurs and the net ionic equation for the redox process. (Assume that one of the products of the redox reaction is a metal.) (b) Calculate the initial concentration of cobalt ions, the final concentration of cobalt ions, and the final concentration of magnesium ions.
A 1.50 g sample of KCl is dissolved in 36.0 mL of water. The resulting solution is then added to 32.0 mL of a 0.470 M CaCl2 (aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution. Concentration of K* ions = M Concentration of Ca2+ ions = M Concentration of Cl ions = M
Solution X containing 0.020 mol of iron(II) sulfate requires 22.5 mL of potassium manganate(VII) for a complete reaction. The equation for the reaction is: 5Fe^2+ + MnO4^- + 8H^+ → Mn^2+ + 4H2O + 5Fe^3+. What is the molarity of the KMnO4 solution?
A student mixes 100.0 mL of 0.500 M AgNO3 with 100.0 mL of 0.500 M CaCl2. Write the balanced molecular equation for the reaction. Write the net ionic equation for the reaction. How many grams of precipitate will form? What is the concentration of Ag+, NO3‒, Ca2+, and Cl‒ in the final solution (assume volumes are additive).
Does a reaction occur when aqueous solutions of sodium carbonate and manganese(II) iodide are combined? O yes no If a reaction does occur, write the net ionic equation. (Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds. Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank.) + →
Barium can be analyzed by precipitating it as BaSO4BaSO4 and weighing the precipitate. When a 0.265 gg sample of a barium compound was treated with excess H2SO4H2SO4 8.50×10−2 gg of BaSO4BaSO4 formed. What is the percentage of barium in the compound?
The following chemical reaction takes place in aqueous solution: 2 FeCl3(aq) +3 K₂S(aq) →Fe₂S3(s)+6 KCl(aq) Write the net ionic equation for this reaction. 0 0-0 X S
You mix 29.0 mL of 0.312 M FeCl3 with 38.5 mL of 0.446 M NaOH. What mass of Fe(OH)3 (in grams) will precipitate from this reaction mixture? Mass= g One of the reactants (FeCl3 or NaOH) is present in a stoichiometric excess. What is the molar concentration of the excess reactant remaining in solution after Fe(OH)3 has been precipitated? Assume the volumes are additive. Concentration = M
Give detailed Solution with explanation needed
The reaction of sulfuric acid with sodium hydroxide is described by the equation: H₂SO4 + 2NaOH → Na₂SO4 + 2H₂O Suppose 50 mL of NaOH with an unknown concentration is placed in a flask, then a few drops of bromthymol blue were added. A solution of 0.20 M H₂SO4 is dripped into the NaOH solution. After exactly 25.0 mL of H₂SO4 is added, the color changes from blue to yellow. The Titrant in this experiment is
Solutions of RbBr and AgClO4 are mixed at room temperature, resulting in a solution that is 7.5 × 10–7 M RbBr and 1.5 × 10–5 M AgClO4. What is expected to happen to the new solution upon mixing? Ksp (AgBr) = 1.8 × 10–10 Silver bromide will precipitate out of solution, leaving an unsaturated solution of AgBr. Nothing will happen since the silver and bromide ions are not in high enough concentration to form a precipitate. Silver bromide will precipitate out of solution, leaving a saturated AgBr solution. There is not enough information to say anything about this solution. Nothing will happen since RbBr and AgClO4 are both soluble compounds.
Which of the following reaction is a precipitation reaction? A) HNO2(aq)+NaOH(aq)---NaNO2(aq)+H2O(I) B) 2C2H3OH(I)+7O2(g)---4CO2(g)+6H2O(I) C) 2H2O2(I)---2H2O(I)+O2(g) D) FeSO4(aq)+K2S(aq)---FeS(s)+K2SO4(aq)