(b) Given the following initial concentrations, what are the equilibrium concentrations of Fe³+, HSCN, and FeSCN²* and the value of K for the equilibrium? Trial 1 2 3 4 5 Initial Concentrations Fe³+ HSCN (M) (M) 0.001 0.0002 0.001 0.0004 0.001 0.0006 0.001 0.0008 0.001 0.0010 Fe³ (M) Equilibrium Concentrations HSCN (M) FeSCN²+ (M) H* (M) 0.5 0.5 0.5 0.5 0.5 Kea

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What is the value of the equilibrium constant Ko for the following reaction at the temperature of the mixture? 2NO,(g) N,0,(g) 3rd attempt See Periodic Table O See Hint Analyses of an equilibrium mixture of N204(g) and NO2(g) gave the following results: [NO2(g)] = 4.210×10-3 M [N204(g)] = 2.706×10³ M 221.3

The value of K.for the the following reaction is 0.550 at 473 K. N2O4(g) = 2NO, (g) 3rd attempt Part 1 See Periodic Table If a reaction vessel at that temperature initially contains 0.0350 M NO2 and 0.0350 M N204, what is the concentration of NO2 at equilibrium? .105 M Part 2 O See Hint What is the concentration of N204 at equilibrium? M

It's a 3 part question; I'm struggling to figure out how to solve each part. Please help! Thanks!    Which equilibrium constant expression(s) are for the following reaction. I2(g)↔I2(solution) Choose from the list below and enter the letters alphabetical order. (e.g. AH) A) (pI2)eq F) [I2(solution)]eq2 B) [I2(solution)]eq G) (pI2)eq-2 C) (pI2)eq-1 H) [I2(solution)]eq-2 D) [I2(solution)]eq-1   Remember that keq is [products]/[reactants], each raised to their stoichiometric coefficients. Also, you should not mix solid, liquid and gas phases carelessly.   2. What is the equilibrium constant expression for the following reaction: PtCl42−(aq)↔Pt2+(aq) + 4Cl−(aq) Choose from the list below and enter the letters alphabetical order. (e.g. For an equilibrium constant of [Cl-]4eq[Pt2+]eq enter AH.) A) [Pt2+]eq E) [Cl-]-1eq I) [PtCl42-]4eq B) [Cl-]eq F) [PtCl42-]-1eq J) [Pt2+]-4eq C) [PtCl42-]eq G) [Pt2+]4eq K) [Cl-]-4eq D) [Pt2+]-1eq H) [Cl-]4eq L) [PtCl42-]-4eq…

8 PM Sat Feb 11 Question 30 of 30 At equilibrium, a 1.0 L reaction vessel contains 2.3 mol of Mg(OH)2 and 0.170 mol of OH-. What is the equilibrium concentration of Mg2+ based on the reaction: Mg(OH)₂ (s) = Mg2+ (aq) + 2 OH- (aq) Kc = 1.80 x 10-¹1 Tap here or pull up for additional resources

A mixture initially contains A , B , and C in the following concentrations: [A] = 0.500 M , [B] = 0.950 M , and [C] = 0.450 M . The following reaction occurs and equilibrium is established: A+2B⇌C At equilibrium, [A] = 0.330 M and [C] = 0.620 M . Calculate the value of the equilibrium constant, Kc . Express your answer numerically. View Available Hint(s)

rs Whiskey attacks Sos me. I told my nothing bc i 2. Write the equilibrium constant expression in terms of K, for the reaction: CS₂ (g) + 4H₂ (g) = CH4 (g) + 2 H₂S (g) TAT 062