Click in the answer box to activate the palette. Balance the following redox reaction and do not include the states of matter. In one of the few reactions known for astatine, the oxidation of astinide ion by chlorine gas in acid solution produces astinate ion (AtO3¯) and chloride ion. X +3C12 +3H2 O-At 03 +6C1 +6H +6e

An electrochemical change occurs when a strip of nickel is immersed in an acidified solution that contains dichromate ions. The colour change that occurs as the reaction above proceeds is: Select one: Green to colourless Orange to green Colourless to green Green to orange Which of the following metals could have been used instead of nickel in order to maintain the original colour of the solution described above? Select one: O Gold Magnesium O Copper Cadmium Which of the following entities will react spontaneously with Cd(s) but not with Ni(s)? Select one: Sn²+ (aq) Cr²+ (aq) Coz+(aq) H₂Se(aq)

The equilibrium constant for the following reaction is 0.143, what is the equilibrium constant for the reverse reaction?   BrCl  ↔   Br2       +     Cl2       Keq = 0.143

Answer the four questions below related to the spontaneous redox reaction that occurs whenCr(OH)3(s) reacts with NO3–(aq) to produce CrO42–(aq)and NO2–(aq) under basic conditions. Write the balanced net ionic equation, including states of matter, for the overall reaction.

Given Zn(s) and AL(s), what observations would you make when combining AL(s) with ZnSO4(aq), and combining Zn(s) with Al(SO4)3(aq)?

Predict which species will be oxidized and which will be reduced in a molten salt mixture that contains CdI2, NaOH, and AlCI3. Cd2+(aq)  +  2e  →  Cd(s)                                        Eored = – 0.40 V I2(s)  +  2e  →  2 I–(aq)                                            Eored = + 0.54 V Na+(aq)  +  1e  →  Na(s)                                         Eored = – 2.71 V Cl2(g)  +  2e  →  2 Cl–(aq)                                       Eored = + 1.36 V Al3+(aq)  +  3e  →  Al(s)                                          Eored = – 1.66 V O2(g)  +  2 H2O(l)  +  4e  →  4 OH–(aq)                  Eored = + 0.40 V     which is oxidized    which is reduced

The standard free energy change for a reaction can be calculated using the equation ΔG∘′=−nFΔE∘′ where n is the number of electrons transferred, F is Faraday's constant, 96.5 kJ·mol−1·V−1, and ΔE∘′ is the difference in reduction potential. For each of the given reactions, determine the number of electrons transferred (n) and calculate standard free energy (ΔG∘′) . Consider the half-reactions and overall reaction for reaction 1. half-reactions: fumarate^2− + 2H^+ ↽−−⇀ succinate^2− CoQH2 ↽−−⇀ CoQ + 2H^+   overall reaction: fumarate^2− + CoQH2↽−−⇀succinate^2− + CoQ ΔE∘′= −0.009 V   n=____ ΔG∘′= ____ (kJ⋅mol^−1) Consider the half-reactions and overall reaction for reaction 2. half-reactions: cytochrome (c1) (Fe^2+) ↽−−⇀ cytochrome (c1) (Fe^3+) cytochrome (c) (Fe^3+) ↽−−⇀ cytochrome (c) (Fe^2+)   overall reaction: cyt (c1) (Fe^2+)+cyt (c) (Fe^3+)↽−−⇀cyt (c1) (Fe^3+)+cyt (c) (Fe^2+) ΔE∘′=0.034 V n= ____ ΔG∘′=____(kJ⋅mol^−1)

Please don't provide handwritten solution....

Complete and balance the following redox reaction in basic solution     NO3- (aq) + AsH3 (s) --> NH3 (g) + As (s)