Identify the changes in oxidation states in the following equations Mg(s) + FeSO_4(aq) rightarrow Fe(s) +...
Calculate the standard cell potential for the following reaction. Fe (s) +Ni^+2 (aq) rightarrow Fe^+ 2 (aq) + Ni (s) 3 Cu + 2 NO_3^- + 8 H^+ rightarrow 3 Cu^+ 2+ 2 NO +4 H_2O Cr_2O_7^-2 + 6 Fe^+2+14 H6+ rightarrow 2 Cr^+ 3 + 6 Fe^+ 3 +7 H_2O
FeSO_4 (aq) + Mg (s) rightarrow Fe (s) + MgSO_4 (aq) Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction.
Which of the following is so oxidation-reduction reaction? A) Cu (s) + 2AgNO_3(aq) rightarrow 2Ag (s) + Cu(NO_3)_2 (aq) B) HCl(aq) + NaOH(aq) rightarrow H_2O (l) + NaCl(aq) C) AgNO_3(aq) + HCl (aq) rightarrow AgCl (s) + N\HNO_3(aq) E) H_2CO_3(aQ) + Ca(NO_3)_2 (aq) rightarrow 2HNO_3(aq) + CaCO_3(s) How many moles of K^+ are present in 343 mL of a 1.27 M solution of K_3PO_4? A) 0.436 B) 1.31 C) 0.145 D) 3.70 E) 11.1 What is the concentration (M) of...
Help For which of the following chemical equations are the stoichiometric coefficients of at least two substances the same when the equations is Na_3PO_4(aq) + AgNO_3 (aq) rightarrow Ag_3PO_4(s) + NANO_3(aq) C_3H_4(g) +O_2(g) rightarrow H_2O(g) + CO_2(g) H_3PO_4(aq) +Mg(OH)_2(s) rightarrow H_2O(J) + Mg_3(PO_4)_2(s) Which of the following chemical equations is NOT balanced? H_3PO_4(aq) -Al(OH)_3(s) rightarrow 3 H_2O(l) + AlPO_2(s)
Question 28 4 pts 28. Identify the oxidation state of Mg in Mg(s). Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g) +1 +2 0 -1 -2 Question 29 4 pts INTI
#15 Assign oxidation states to al the elements In this unbalanced reaction: Ag^+(aq) + Cu(s) rightarrow Ag(s) + Cu^2+ (aq) Which substance gets oxidized? Ag^+(aq) Cu(s) Ag(s) Cu^2+(aq) Which substance gets reduced? Balance the redox reaction: Ag^+(aq) Cu(s) Ag(s) Cu^2+(aq)
Identify the species (atoms/ elements) undergoing oxidation and reduction in the following equations, assign oxidation numbers to each, and write balanced net ionic equations. a) Cu(s) Cu2+(aq) + 2e- b) Cl2(aq) + 2e- Cl-(aq) c) Cu(s) + Cl2(aq) Cu2+(aq) + 2Cl-(aq) d) 4CuO(s) + CH4(g) 4Cu(s) + CO2(g) + 2H2O(l) e) 2CuSO4(aq) + 4KI(aq) 2CuI (aq) + 2K2SO4(aq) + I2(aq) f) Cu2O(s) + Fe(SO4)3 (aq) + H2SO4(aq) 2CuSO4(aq) + 2FeSO4(aq) + H2O(l)
Classify the following as acid-base reactions or oxidation-reduction reactions. (a) 3 HClO4(aq) + Fe(OH)3(s) → Fe(ClO4)3(aq) + 3 H2O(l) (b) HC2H3O2(aq) + NaHCO3(aq) → NaC2H3O2(aq) + CO2(g) + H2O(l) (c) 4 H2O(l) + 2 KMnO4(aq) → 2 MnO2(s) + 2 KOH(aq) + 3 H2O2(aq) (d) Cl2(g) + KOH(aq) → KClO(aq) + HCl(aq) (e) 2 Fe(s) + 3 NaOCl(aq) → Fe2O3(s) + 3 NaCl(aq) (f) CaC2(s) + 2 H2O(l) → C2H2(g) + Ca(OH)2(s) Explain your reasoning
Construct a frost diagram for the species in the Latimer diagram in problem 2. Here is problem 2 but I do not need you to do problem 2 I need help with the diagram. Problem 2: Identify the changes in oxidation states in the following equations: Mg (s) + FeSO4 (aq) -> Fe (s) + MgSO4 (aq) 2 HNO3 (aq) + 3 H2S (aq) -> 2 NO (g) + 3 S (s) + 4 H2O (l)
Balance the following in acidic conditions: I_2(l) + SO_2(g) rightarrow I^-(aq) + SO_4^2-(aq)