Using data from Appendix E, calculate the equilibrium constant for the disproportionation of the copper(I) ion at room temperature: 2 Cu+1aq2 ¡ Cu2+1aq2 + Cu1s2

Copper(I) ion disproportionates to copper metal and copper(ll) ion. (See Study Question 99.) 2 Cu+(aq) Cu(s) + Cu2 + (aq) (a) What two half-reactions make up the disproportionation reaction? (b) Use values of the standard reduction potentials for the two half-reactions in part (a) to determine whether this disproportionation reaction is product-favored at equilibrium. (c) What is the equilibrium constant for this reaction? If you have a solution that initially contains 0.10 mol of Cu+ in 1.0 L of water, what are the concentrations of Cu+ and Cu2+ at equilibrium?

Sodium perchlorate, NaClO4, is produced by electrolysis of sodium chlorate, NaClO3. If a current of 2.50 103 A passes through an electrolytic cell, how many kilograms of sodium perchlorate are produced per hour?

A constant current of 1.40 amp is passed through an electrolytic cell containing a 0.100 M solution of AgNO3 and a silver anode and a platinum cathode until 2.48 g of silver is deposited. a How long does the current flow to obtain this deposit? b What mass of chromium would be deposited in a similar cell containing 0.100 M Cr3+ if the same amount of current were used?

Copper(I) disproportionates to copper metal and copper(II) ion.  2 Cu+(aq) --> Cu(s) + Cu2+(aq) (a) What two half-reactions make up the disproportionation reaction? (b) Is this disproportionation product favored? (c) What is the equilibrium constant for this reaction?

Given: You weigh out exactly 0.200 g of Fe(NH4)2(SO4)2·6H2O and dissolve it in the 100.00 mL volumetric flask. You then pipette 2.00 mL of this solution into the 50.00 mL volumetric flask to prepare the stock standard tris-bipyridyl-iron(II) solution. a. Calculate the molar concentration of iron(II) in this solution in the 50.00 mL volumetric flask. (The MW of Fe(NH4)2(SO4)2·6H2O is 392.14 g/mol) (answer a given the information above)

The standard reduction potential for the reaction [Co(H2 O)6]3+(aq) + e− ⟶ [Co(H2 O)6]2+(aq) is about 1.8 V. The reduction potential for the reaction [Co(NH3)6]3+(aq) + e− ⟶ [Co(NH3)6]2+(aq) is +0.1 V. Calculate the cell potentials to show whether the complex ions, [Co(H2O)6]2+ and/or [Co(NH3)6]2+, can be oxidized to the corresponding cobalt(III) complex by oxygen.

Titanium (IV) exists in aqueous solution but not as the Ti4+(aq) ion. Suggest the identity of the species.

One of the steps for refining silver involves converting silver into dicyanoargenate(I) ions:      4Ag(s) + 8CN−(aq) + O2(g) + 2H2O(l) ⟶ 4[Ag(CN)2]−(aq) + 4OH−(aq)Explain why oxygen must be present to carry out the reaction. Why does the reaction not occur as:            4Ag(s) + 8CN−(aq) ⟶ 4[Ag(CN)2−(aq)?

Write the balanced NET ionic equation for the reaction when NH₄Cl and Cu(C₂H₃O₂)₂ are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.