Balance the following redox reaction which takes place in basic solution. Write your balanced equation on the line and then answer the following questions ClO3-(aq) + Cu(s) + I-(aq) → Cl2(g) + CuI(s) a. What is the oxidation state of Cl in ClO3-(aq)? b. What is the oxidation state

When the following skeletal equation is balanced under basic conditions, what are the coefficients of the species shown? NiO2 + Sno,2- → Ni(OH)2 + Sno32- (Enter 0 Water appears in the balanced equation as a for neither.) (reactant, product, neither) with a coefficient of Which species is the reducing agent?

Write the balanced NET ionic equation for the reaction when ZnI₂ and Pb(ClO₄)₂ are mixed in aqueous solution. If no reaction occurs, simply write only NR.

ENTS IN GENERAL CHEMISTRY GENERAL CHEMISTRY STUDY SHEET NO. 4 1. Balance the following chemical equations: a) C„H; + O, → CO2 + H,O s b) Al,S, + PbCl,4 PbS, + A1CI, nos 0 c) BaCl, + Na,PO, → Ba, (PO), + NaCl 2. Assume the follon 100

Which species is the “oxidizing agent” in the reaction shown below? 2 Mn2+ + 5 Cl2+ 8 H2O →2 MnO4– + 16 H+ + 10 Cl –

3. . Predict the products and states of the products for the following reactions. Balance the equations. If no reaction is expected, write NR. a) H2SO4(aq) + M9CO3(s) b) Mg(s) + F2(g) c) Li(s) + H2O(1) → d) Na2S(aq) + AICI3(aq) e) Ca(s) + MnCl2(aq) f) Br2(g) + KF (aq)

Balance the Net Ionic equation for this reaction.

Consider the reaction:    2 NH3(g)  →  N2(g) + 3 H2(g)   .The oxidation numbers for the N in NH3, the H in NH3, The N in N2, and the H in H2 are, respectively? a)    0, 0, -3, +1c)   -3, +1, 0, 0    b)   -1, +1, 0, 0  d)  +3, –1, 0, 0 Which of the following would not be a product of the reactants: Sulfuric acid and Sodium carbonate? a)   Na2SO4 c)   H2O b)   CO2 d)   H2

a. Complete and balance the following double displacement reaction. Include the states of the products. LiOH (aq) + MgCl2 (aq)   ? + ? b. Write the net ionic equation for the above reaction?

Question 7. What is the oxidation state of Cr in each compound?a. CrOb. CrO 3c. Cr2O 3   Question 8. Consider the following reactions:a. Zn(s) + 2 AgNO3(aq) → Zn(NO3) 2(aq) + 2 Ag(s)b. 2 Li(s) + Fe(C 2H3O 2) 2(aq) → 2 LiC2H3O 2(aq) + Fe(s)c. Ni(s) + 2 AgClO 4(aq) → Ni(ClO4) 2(aq) + 2 Ag(s)For each reaction, assign oxidation states to each element on the reactant and product side of thereaction. In addition, answer the following questions: Which element is being reduced? Which is beingoxidized? What is the reducing agent? What is the oxidizing agent?