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The reaction was stopped before all the nickel reacted, and 36.5 g of solid metal (nickel and silver) is present. Consequently the half-equation, \[\ce{2Ag^+ + 2e^{-} -> 2Ag} \nonumber \]. To balance a chemical equation, every element must have the same number of atoms on each side of the equation. What mass of nickel(II) nitrate would be produced given the quantities above? &\textrm{overall: }\ce{5Fe^2+}(aq)+\ce{MnO4-}(aq)+\ce{8H+}(aq)\ce{5Fe^3+}(aq)+\ce{Mn^2+}(aq)+\ce{4H2O}(l) Since there are an equal number of atoms of each element on both sides, the equation is balanced. In contrast, because \(\ce{Ag2Cr2O7}\) is not very soluble, it separates from the solution as a solid. One of the simplest cells is the Daniell cell. What is the molecular equation for nickel chloride and silver nitrate Draw a cell diagram for this reaction. By investigating a series of displacement reactions leaners aged 11-14 can learn about the reactivity series of metals. At this point, no current flowsthat is, no significant movement of electrons through the wire occurs because the circuit is open. 2NO3-, 2AgNO3 + NiCl2 -------> 2AgCl + Ni(NO3)2, The following uses nickel(II) chloride The net ionic equation is as follows: \(Pb^{2+} (aq) + 2I^-(aq) \rightarrow PbI_2(s) \), \(Fe^{2+}(aq) + 2OH^-(aq) \rightarrow Fe(OH)_2(s)\), \(2PO_4^{3-}(aq) + 3Hg^{2+}(aq) \rightarrow Hg_3(PO_4)_2(s)\), \(Ca^{2+}(aq) + CO_3^{2-}(aq) \rightarrow CaCO_3(s)\), Predicting the Solubility of Ionic Compounds: Predicting the Solubility of Ionic Compounds, YouTube(opens in new window) [youtu.be] (opens in new window). 15. Explanation: Ag+ + e Ag(s) And aluminum is oxidized.. Al(s) Al3+ + 3e And we add the half equations such that the electrons are eliminated. \end{align} \nonumber \], The cell used an inert platinum wire for the cathode, so the cell notation is, \[\ce{Mg}(s)\ce{Mg^2+}(aq)\ce{H+}(aq)\ce{H2}(g)\ce{Pt}(s) \nonumber \]. Nickel replaces silver from silver nitrate in solution according to the following equation: 2AgNO3 + Ni (arrow) 2Ag +Ni(NO3)2 a. &\underline{\textrm{reduction: }2(\ce{Ag+}(aq)+\ce{e-}\ce{Ag}(s))\hspace{40px}\ce{or}\hspace{40px}\ce{2Ag+}(aq)+\ce{2e-}\ce{2Ag}(s)}\\ We described a precipitation reaction in which a colorless solution of silver nitrate was mixed with a yellow-orange solution of potassium dichromate to give a reddish precipitate of silver dichromate: \[\ce{AgNO_3(aq) + K_2Cr_2O_7(aq) \rightarrow Ag_2Cr_2O_7(s) + KNO_3(aq)} \label{4.2.1} \]. I need help with describing the process of obtaining the following question in detail with a balanced equation and all the calculations. Nickel (II) chloride reacts with aluminum to produce nickel and aluminum chloride: 3NiCl2 + 2Al ==> 3Ni + 2AlCl3 Net ionic equation of silver nitrate and nickel chloride? Note that \(\ce{K^+ (aq)}\) and \(\ce{NO3^{} (aq)}\) ions are present on both sides of Equation \(\ref{4.2.2a}\) and their coefficients are the same on both sides. d. Is the reaction spontaneous as written? Clearly the copper metal has lost electrons and been oxidized to Cu2+, but where have the donated electrons gone? We will discuss solubilities in more detail later, where you will learn that very small amounts of the constituent ions remain in solution even after precipitation of an insoluble salt. The solution acquires the blue color characteristic of the hydrated Cu2+ ion. 1). Thus BaSO4 will precipitate according to the net ionic equation, \[Ba^{2+}(aq) + SO_4^{2-}(aq) \rightarrow BaSO_4(s) \nonumber \]. Aqueous ammonia precipitates green gelatinous Ni(OH)2: The nickel(II) hydroxide precipitate dissolves in excess ammonia to form a blue complex ion: Sodium hydroxide also precipitates nickel(II) hydroxide: Nickel(II) hydroxide does not dissolve in excess \(\ce{NaOH}\).