Express your chemical equation: 13.HBr(aq)+Al(OH)3(s)→ 13.1 HI(aq)+CaCO3(s)→ 14. H2SO4(aq)+NaOH(s)→ (neutralization of both acidic protons) 14.1 HBr(aq)+LiOH(s)→ 18. CO(g)+H2O(g)⇌H2(g)+CO2(g) K=[CO2][H2][CO][H2O] K=[CO][H2O][CO2][H2] K=[CO2][H2][CO][H2O] K=[CO2][H2][CO] 18.1 CH3COOH(aq)+H2O(l)⇌H3O+(aq)+CH3COO−(aq) K=[CH3COOH][CH3COO−][H3O+] K=[CH3COO−][H3O+][CH3COOH] K=[CH3COO−][H3O+][CH3COOH] K=[CH3COO−][H3O+][CH3COOH][H2O] 19. N2(g)+3Br2(g)⇌2NBr3(g) K=[NBr3][N2][Br2] K=[NBr3]2[N2][Br2]3 K=[N2][Br2]3[NBr3]2 K=[NBr3]2[N2][Br2]3 19.1 C(s)+O2(g)⇌CO2(g) K=[O2][CO2] K=[CO2][O2] K=[CO2][O2][C] K=[CO2][O2]
6) For the reaction 4 HBr(aq) + O2(g) = 2 Br2(aq) + 2 H2O(l), K. -6.7 x 1010. Use this information to calculate the equilibrium constant for each of the following reactions. a) 2 HBr(aq) + 12 O2(g) + Brz(aq) + H2O(1) b) 4 Br2(aq) + 4H2O(l) = 8 HBr(aq) + 2 O2(g)
MgCl2(aq)+H2(g)→ C4H10(g)+O2(g)Δ ⟶ Al(s)+O2(g)→ HCl(aq)+Pb(NO3)2(aq)→ complete and balance the following equations
84. Which reactions are redox reactions? (a) Al(s) + 3 Ag+(aq) -> Al+(aq) + 3 Ag(s) (b) 4 K(s) + O2(g) → 2K2O(s) (c) SO3(g) + H2O(l) → H2SO4(aq) (d) Mg(s) + Brz(1) ► MgBrz(s)
I, K, M, N
R-O-O-R (trace +HB HBr Q. 1) Hg(OAc)+H20 2) NaBH4 OH CH3 J. K. CH 2 1) BH3/THF 2) H202/ OH OH 1) BH3/THF L. 2) H202/ OH M. Br2 CH3-CC-CH N. (1) O3 (2) Zn/H20 liq NH +2 P.
Determine AS for the reaction to form 45.92 g of, Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g), given (answer in J) Substance Sº (J/mol · K) Zn(s) 60.9 HCl(aq) 56.5 H2(g) 130.58 Zn2+ (aq) -106.5 cl(aq) 55.10 Answer: Check
4. Balance the following equations: Al(NO)(aq) + NH.OH(aq) Al(OH),(s) + (NH) (NO) (aq) classify Fe(OH)3(s) + __H,SO.(aq) → ___ Fer(SO.)s(aq) + _ H2O(1) classify CH,CI(I) + O2(g) → - CO2(g) + H2O(g) +- HCI(9) classify Ca(s) + __P_Os() → _ Cao(s) + - P.(I) classify LI.CO() - - HCl(aq) + LICH(aq) H2O(l) + - CO2(g) classify NO2(g) → N2(g) + H2O(1) classify + N2H400) + - 5. P.(s) + O2(g) → - P.Os(s) balance, then classify Calculate the following, with...
Determine
S°rxn for Zn (s) + 2HCl (aq)
ZnCl2 (aq) + H2 (g).
Substance
S° (J/mol ⋅ K)
Zn(s)
60.9
HCl(aq)
56.5
H2(g)
130.58
Zn2+(aq)
−106.5
Cl−(aq)
55.10
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For the reaction NH4Cl(aq)NH3(g) + HCl(aq) H° = 86.4 kJ and S° = 79.1 J/K The equilibrium constant for this reaction at 261.0 K is
Which of the reactions are exothermic? 2Mg(s)+O2(g)⟶2MgO(s)+heat2Mg(s)+O2(g)⟶2MgO(s)+heat NH3(g)+HCl(g)⟶NH4Cl(s)+heatNH3(g)+HCl(g)⟶NH4Cl(s)+heat AgCl(s)+heat⟶Ag+(aq)+Cl−(aq)AgCl(s)+heat⟶Ag+(aq)+Cl−(aq) 2Fe2O3(s)+3C(s)+heat⟶4Fe(s)+3CO2(g)2Fe2O3(s)+3C(s)+heat⟶4Fe(s)+3CO2(g) C(graphite)+O2(g)⟶CO2(g)+heatC(graphite)+O2(g)⟶CO2(g)+heat CH4(g)+2O2(g)⟶CO2(g)+2H2O(l)+heat