Balance the following in acidic conditions: I_2(l) + SO_2(g) rightarrow I^-(aq) + SO_4^2-(aq)
Balance the reaction in acidic conditions Pbo_2(8) + I^-(aq) rightarrow Pb^2+(aq) + I_2(s) I_2(s) rightarrow I^-(aq)
Balance the following redox reactions under both acidic and basic conditions I_2O_5(s) + CO(g) rightarrow I_2(s) + CO_2 (g) IO^- _3 + H_3AsO_3(aq) rightarrow H_3AsO_4(aq) + I_2(s) PbSO_4(s) + Br_2(I) rightarrow Pb(s) +SO^-2 _4(aq) +BrO^- _3(aq)
Complete and balance the following equations I_2 (s) + OC^- (ag) rightarrow IO_3^- (aq) + Cl^- (aq) (acidic solution) Express your answer as a chemical equation. Identify all of the phases in your answer.
Fc^2+ (aq) + Mo_3^- (aq) rightarrow Fe^3+ (aq) + No(g) acidic solution.
Balance the 1/2 reaction using the 1/2 rxn method: MnO_4^- (aq) rightarrow MrvO_2(aq) (basic) Skip 4d Balance the Redox Equat. using, the 1/2 rxn method (acidic conditions): H_2C_2O_4(aq) + MnO_4^-(aq) rightarrow Mn^2+(aq) + CO_2(g)
1. Balance the following redox reaction in acidic conditions; KMnO4 (aq) + NO (g) → MnO2 (s) + NO2(g) (Please show every step when balancing this redox reaction in acidic condition, thanks.) 2. Which chemical has more entropy and explain why. Linear polyethylene (s) or hyperbranched polyethylene (s)
H_2(g) + I_2(g) rightarrow 2HI(g) Initial concentration [H_2] = 2: [I_2] = 2: [HI] = 3 Kc = 55.17 Is the system at equilibrium? If not, which direction should equilibrium shift? What is equilibrium concentration of each species? 55.17 == [3 + 2X]^2/[2 - X]^2 X = ? Relative strength of acid and base: The stronger the acid, the weaker its conjugate base The stronger the base, the weaker its conjugate acid
2. Balance the following reaction under acidic conditions. Cl2(aq) + Br2(1) BrO3-(aq) + Cl-(aq)
Identify the changes in oxidation states in the following equations Mg(s) + FeSO_4(aq) rightarrow Fe(s) + Mg SO_4(aq) 2 HNO_3(aq) + 3H_2S(aq) rightarrow 2NO(s) + 3S(s) + 4 H_2O(l)
Balance each of the following redox reactions occurring in acidic solution. 1. I−(aq)+NO−2(aq)→I2(s)+NO(g) 2. IO3−(aq)+H2SO3(aq)→I2(aq)+SO42−(aq) 3. NO−3(aq)+Sn2+(aq)→Sn4+(aq)+NO(g)