For the reaction below, Kc = 9.2 × 10-5. Note Kc is sometimes called K. %3D What is the equilibrium concentration of D if the reaction begins with 0.58 M A? A (aq) + 2 B (s)=C (s) + 2 D (aq)
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- The equilibrium constant, Kc is 0.0183 for the reaction at a certain temperature: 2 HI(g) ⇄ H2(g) + I2(g) If 3.00 moles of HI are placed in a 5.00 L vessel and allowed to reach equilibrium, what is the equilibrium concentration (in mol/L) of H2 gas? Hint: use the perfect square method and construct an ICE table. Record your answer as a standard number to 3 significant figures. For example, if the answer is 2.75 x 10-3 mol/L then you should enter 0.00275 as the answer.A certain reaction has an equilibrium constant of 10.1 at 25oC. A ⇄ B Determine its ΔG, in kJ/mol, if [A]=0.05 M and [B]=1x10-4 M?At 25 °C, the reactionCaCrO4(s) ⇌ Ca2+(aq) + CrO42-(aq)has an equilibrium constant Kc = 7.1 x 10-4. What arethe equilibrium concentrations of Ca2 + and CrO42- in aa saturated solution of CaCrO4?
- The simplifying assumption (a.k.a. the 100 rule) Nitrogen oxides from exhaust gases are a serious pollution problem. One such reaction is given here: N2(g) + O2(g) ⇌ 2 NO(g) At the temperature of the exhaust gases from a particular engine the value if K is 4.2 x 10-8. A chemist puts 0.085 mol of nitrogen and 0.038 mol of oxygen in a rigid 1.50 dm3 cylinder. What is the concentration of nitrogen monoxide gas in the mixture at equilibrium?Chemistry If you mix 5.00 mL of 0.375 M Co(NO3)2 with 7.50 mL of 0.400 M Na2C2O4 (sodium oxalate), you form Na4(Co(C2O4)3)(aq) (Kf = 5.00x109). Determine the equilibrium concentrations of all relevant species. Give your answers to 3 sig. figs. and in scientific notation (e. g. 1.23E-4) but do not include the units in the answer. Co(NO3)2 = Na2C2O4 = Na4(Co(C2O4)3) =The value of Kc for the reaction below is 0.210 at 373 K.N2O4 (g) ⇌ 2 NO2 (g)a. Mathematically determine in which direction the reaction will proceed if the reaction vesselinitially contains 0.300 M N2O4 at the given temperature?
- For the following reactionC(??) + 2H2(??) ⇌ CH4(??)K =0.26 at 1000 °C (3 significant figures). What is the equilibrium constant at 750 °C (3significant figures)?For the following reaction : H2 (g) + I2 (g) 2HI (g) it was found that a 13.0L vessel at equilibrium contained 0.852 mol H2, 0.361 mol I2, and 2.99 mol of HI. A) Write an expression for Kc. B). Determine the value of Kc for this reaction.There are two questions here if that is okay...Question 1 Consider the reaction: 2 A (aq) ⇌ B(aq) Given the following KC values and starting with the initial concentration of A = 4.00 M, complete ICE diagram(s)and find the equilibrium concentrations for A and B.A) KC = 4.00B) KC = 200C) KC = 8.00 x10-3 Question 2 Consider the reaction: Cl2 (g) + F2 (g) ⟷ 2 ClF (g) KP=? The partial pressure of 203 kPa for Cl2 and a partial pressure of 405 kPa for F2. Upon reaching equilibrium, thepartial pressure of ClF is 180 kPa. Calculate the equilibrium concentrations and then find the value for KP.
- On analysis, an equilibrium mixture for the reaction 2H2S(g) <--> 2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction. (2 sig figs)At 25oC, the ΔH o andΔH o for the following reaction is -24.7 kJ/mol and -49.9 J/mol-K, respectively. H2S (aq) + CN- (aq) ⇋ HS- (aq) + HCN (aq) If you mix 100 mL of 0.0450 M NaCN with 100 mL of 0.0450 M H2S, the reaction will proceed as indicated in the equation and will reach an equilibrium in the end. What will be the molar concentration of HCN at equilibrium?How I find the equilibrium constant? I was able to get K to be 0.001789 by having Ba and AsO = to S. I got 1.1e-13= [3S]^3 [2S]^2 so S=0.001789 then I plugged that in to find my Ba but got it wrong.