Fe³+ (aq) | Fe(s) || Cl(aq) | Cl₂(g) | Pt 3+ Cl₂(g) | Cl(aq) | Pt || Fe(s)| Fe³+ (aq) 3+ Fe(s) | Fe³+ (aq) || Cl₂(g) | Cl(aq) | Pt 3+ Fe(s) | Cl2(g) || Fe³+ (aq) | Cl(aq) | Pt Cl(aq) | Cl₂(g) | Pt || Fe³+ (aq) | Fe(s) 3+
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determine the cell notation for the
3Cl2(g) + 2Fe(s) --> 6Cl-(aq) + 2Fe3+(aq)
(see image)
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- C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.d) Explain the effect on equilibrium of:i) Increasing temperatureii) Increasing pressureiii) Decreasing the concentration of oxygeniv) Increasing the concentration of carbon dioxidev) Adding a catalystCopper(I) ions in aqueous solution react with NH3 (aq) according to Cu+ (aq) + 2 NH3 (aq) · → Cu(NH3)2(aq) K₁ = 6.3 × 1010 Calculate the solubility (in g·L-¹) of CuBr(s) (Ksp = : 6.3 × 109) in 0.74 M NH3(aq). solubility of CuBr(s): g/LAgBr(s) = Ag*(aq) + Br(aq) Ksp = 5.30 x 10-13 Ag (aq) + 2NH3(aq) [Ag(NH3)₂1 (aq) K+ = 1.70x107 123 When NH3(aq) is added to AgBr(s), a combination of these two reactions occurs: AgBr(s) + 2NH3(aq) == [Ag(NH3)2]* (aq) + Br (aq) What mass of AgBr(s) (187.8 g/mol) can react with 1.00 L of 3.22 M NH3? Provide answer in grams to 3 significant figures.
- Select the reaction for which K, = Kc. 2 Na,0,(s) + 2 CO,(g) =2 Na,CO3(s) + 0,(g) 2 KCIO3 (s) = 2 KCI(s) + 30,(g) 2 H,S(g) + SO,(g)= 3 S(s) + 2 H,O(g) Br, (g) + Cl,(g) 2 BRCI(g)AgBr(s) 2 Ag*(aq) + Br (aq) Ag*(aq) + 2NH3(aq) Ag(NH3)2*(aq) Kf = 1.5 x 107 RS Ksp = 7.7 x 10-13 When NH3 is added to AgBr(s), a combination of these reactions result: AgBr(s) + 2NH3(aq) 2 Ag(NH3)2*(aq) + Br (aq) What mass of AgBr will dissolve in a 5.0 L container of 3.0 M NH3 solution?Silver chloride is classified as an insoluble compound because it dissolves only to a small extent in water. Consider the balanced equation and equilibrium constant that shows the partial dissolving of silver chloride in water: AgCl(s) = Ag*(aq) + CI"(ag) Keg = 1.70 x 10-10 a) The reaction AgCl(s) = Ag*(aq) + Cl (ag) is classified as a (homogeneous or heterogeneous) equilibrium because it involves more than one physical state, solid and aqueous. b) Based on the equilibrium constant value and the equilibrium constant expression, the concentration of each ion in a saturated solution of silver chloride is : Concentration of Ag = x 10 Concentration of CI" = x 10 M
- Calculate the value of the equilibrium constant, Kc, for the reaction Q(g) + X(g) 2 M(g) + N(g) given that Kc = M(g) = Z(g) 6R(g) — 2N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kc1 = 3.01 Kc2 = 0.433 Kc3 = 12.5Part 1: (a) Calculate K at 298 K for the following reaction: 2C(graphite) + O₂(g) = 2CO(g) K = 1.25 C(graphite) CO(g) 0₂ (8) Part 2 out of 2 AGⓇ x 10 || 48 (b) Use the equilibrium constant to calculate AG (in kJ) at 298 K for the following reaction: 2HCl(g) + Br₂(1) ⇒ 2HBr(g) + Cl₂(g) K= 2.22 × 10-15 at 298 K AG KJ kJ C mol x 10 0 -137.2 0 kJWrite the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HCN(aq) + H,O(1) H30*(aq) + CN'(aq) K =
- Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HNO2 (aq) + OH" (aq)NO, (aq) + H2O (1) K =Consider the reaction 3A(g)+2B(g)=2C(g)+1D(aq). In 3.1L, 2.79mol A and 2.72mol B are mixed. At equilibrium, 0.573mol D are detected. What is the concentration equilibrium constant (K) of the reaction? Enter your answer to four decimal places if it is less than 1, otherwise answer with a minimum of four digits (ie: 2543, 153.4, 12.52, or 6.523). If your last digit is a trailing zero remember that it's okay that canvas removes it. If it is smaller than 0.0001, enter "0" and make sure you indicate your actual answer clearly on your work.2 Zn*2 (aq) +Fe*2 (ag) + 6 CN (ag) = Zn2Fe(CN)6 (5) [znz Fe (CN),] A certain equilibrium reaction has K = 2.8 x 10-13 at 25 °C. What is the change in Gibbs Free Energy (kJ/mole) under these conditions?