Consider the equilibrium: Sno, (s) + 2CO (8) Sn (s) + 2C02 (8) 5.0g of tin (II) oxide and 0.85 M carbon monoxide were initially charged in a closed reactor at room temperature and allowed to reach equilibrium. At equilibrium 0.65 M of CO was measured. Calculate Kc for the equilibrium. O 0.095 04.2 O0.033 O0.22
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- Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.Given the reaction: CO2(g) + H2(g) ⇌ H2O(g) + CO(g) If Kc = 1.6 at 1263 K, calculate the number of moles of carbon monoxide gas (CO) in the final equilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O, and 1.00 mol of CO to a 5.00 L reactor at the given temperature.In the gas phase reaction 2 A(g) + B(g) ⇋ 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species, kx, kp and ∆G0
- i think it is The reaction quotient can be calculated from the reactants' and products' concentrations or partial pressures. 2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq) At non-standard conditions, the concentrations are: [SmCl3] = 2.00 M [Li] = 2.00M [Sm] = 0 (solid) [LiCl] = 0.0100 M The reaction quotient (Q) can be calculated as follows: Q = {[LiCl]^6}/[Sm3+ ]^2[Cl3]^2 = (0.0100)^6 /(2.00)^2 x (2.00)^2 = 6.25 x 10^-14For the liquid-phase reaction A + 2B ⇄ C + 2D , it was found that when 2 mol A, 4 mol B and 2 mol C were mixed in 1 L of water and allowed to come to equilibrium at 25 0C, the resulting mixture contained 2 mol of D. Calculate equilibrium constant, K, for this reaction.In the gas phase reaction 2 A(g) + B(g) = 3 C (g) + 2 D (g) it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate (a) the mole fractions of each species, (b) KX, (c) KP and (d) △Go . Answer: [0.087 (A); 0.370 (B); 0.196 (C); 0.348 (D); 0.326; 0.325; 2.76 kJ]
- The KspKsp of a salt corresponds to a reaction with the following general format: salt(s)⇌mcation(aq)+nanion(aq)where mm and nn are the coefficients that balance the equation. Equilibrium constants follow the general format of products over reactants (excluding pure liquids and solids) with each species raised to the power of its coefficient in the balanced equation. KspKsp is no exception, so Ksp=[cation]m[anion]nKsp=[cation]m[anion]n Part A If 500.0 mLmL of 0.10 mol L−1 Ca2+mol L−1 Ca2+ is mixed with 500.0 mLmL of 0.10 mol L−1 SO42−mol L−1 SO42−, what mass of calcium sulfate will precipitate? KspKsp for CaSO4CaSO4 is 2.40× 10−52.40×10−5. Express your answer to three significant figures and include the appropriate unitsFor the liquid-phase reaction A + 2B ⇄ 2C + D , it was found that when 2 mol A, 4 mol B and 2 mol C were mixed in 1 L of water and allowed to come to equilibrium at 25 0C, the resulting mixture contained 1 mol of D. Calculate equilibrium constant, K, for this reactionFor the liquid-phase reaction 2A + 2B ⇄C + D , it was found that when 3mol A, 4 mol B and 1mol C were mixed in 1 L of water and allowed to come to equilibrium at 25 0C, the resulting mixture contained 1 mol of D. Calculate equilibrium constant, K, for this reaction.
- Consider the mixing of 25.00 mL of 0.0500 M Pb(NO3)2 with 25.00 mL of 0.0500 M NaCl and the equilibrium reaction, PbCl2(s) ⇌ Pb2+(aq) + 2Cl-(aq) Ksp = 1.20 x 10-5 What is the molar concentration of Pb2+ in the resulting mixture? (0.500, 0.025, 0.0125 or 0.100) What is the molar concentration of Cl- in the resulting mixture? (0.500, 0.025, 0.0125 or 0.100) What is the ion product (Q)? Will a precipitate form? (yes or no)A 51.0-LL reactor at 1600 KK is charged with 50.0 gg of NiO(s)NiO(s) and 1.40 atmatm of CO(g)CO(g). After equilibrium is reached, what is the partial pressure of CO2(g)CO2(g) in the reactor?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 catalyst