3 Show that the equilibrium constant for HCl +DBr DCI +HBr approaches unity at sufficiently high...
For the reaction 2 HBr(g) + Cl_2(g) rightarrow 2 HCl(g) + Br_2(g) a. Write the equilibrium constant expression for the reaction. b. Using the following G degree values, calculate Delta G degree for the reaction. HBr(g) = -53.22 kJ/mol HCl(g) = -95.27 kJ/mol Cl_2(g) = 0 kJ/mol Br_2(g) = 3.14 kJ/mol c. Calculate the equilibrium constant K_eq be at 298 K. d. Does this equilibrium lie more with reactants or products?
The molar constant volume heat capacity of acetylene (H-C≡C-H) approaches xR at high temperatures. What is x? Assume ideality.
Please Help. Physical Chemistry question 3. If you do a careful job recording HCl and DCI spectra at the highest available resolu- tion, you will be able to see that each rotational line is split into a doublet (two closely spaced lines). Can you explain the origin for this splitting? Calculate the effective masses for the D"C1 and Dºci (H²Cl and H Cl) isotopes, and evaluate the expected shift of the vibrational fre- quency and change in the rotational constant....
3) The reaction H2 + Cl2+ Br2 behavior: HCl + HBr + CIBr is shown to have the following rate Rate (M/s) H2] (M) [Cl2] (M) Br2] (M) 0.38 0.1 0.4 0.12 0.12 0.76 0.2 0.2 0.4 0.76 1.52 0.8 0.12 0.2 0.8 0.24 b) (15 points) What is the rate constant for the reaction? Use appropriate units. a) (15 points) What is the rate law for the reaction? WD/RE c) (30 points) Propose a mechanism for the reaction.
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperatures: Kp: 170K 3.8*10^-3 180K 0.34 190K 18.4 200K 681 Part A Use the data to find ΔH∘rxn and ΔS∘rxn for the reaction. i found ΔH∘rxn = 114 kJ but i dont know how to get ΔS∘rxn. please help and show work
The equilibrium constant, Kc, for the following reaction is 1.28×10-3 at 231 K. 2NOBr(g) goes to 2NO(g) + Br2(g) . When a sufficiently large sample of NOBr(g) is introduced into an evacuated vessel at 231 K, the equilibrium concentration of Br2(g) is found to be 0.200 M. Calculate the concentration of NOBr in the equilibrium mixture. __M
3. At high pH, some metals precipitate as metal hydroxides. For cadmium, the equilibrium constant for the reaction is 5.5 x 1013 Cd" +20H' Cd(OH),(s) a. If the pH of the water is maintained at 8.0, what is the dissolved cadmium concentration in mg/L? b. What pH is required to meet a goal of 100 mg/L dissolved cadmium?
Question 3 Not yet answered Points out of 2 Flag question The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. H2(g) + Br2(g) 2 HBr(g) Kc 3.8 x 104 2 HBr(g) H2(g) + Br2(g) Kc = ? Select one: O a. 1.9 x 104 ○ b. 5.3 × 10.5 O c. 2.6x 10-5 d. 6.4 x 10-4 e. 1.6 x 103 O o
(1). The equilibrium constant, K, for the following reaction is 1.32×10-3 at 565 K. NH4Cl(s) =NH3(g) + HCl(g) An equilibrium mixture in a 10.4 L container at 565 K contains 0.285 mol NH4Cl(s), 4.47×10-2 M NH3 and 2.95×10-2 M HCl. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 4.25 L? [NH3] = M [HCl] = M
3. Calculate deltaS and deltaG and the equilibrium constant 298 K for each of these reactions, and indicate whether they are spontaneous under standard conditionsa. H2 (g) + F2 (g) --> 2HF (g) b. C2H5OH (g) --> C2H4 (g) + H2O (g) (Calculate deltaH for this one as well ) c.2HCl (g) + Br2 (g) → 2HBr(g) + Cl2 (g) d. PCl3 (g) + 3 H2 (g) --> PH3 (g) + 3 HCl (g) (Calculate H for this one as...