Given 2 BrCl(g) reversible Cl_2(g) + Br_2(g) K_p = 0.169 2 IBr(g) reversible Br_2(S) + I_2(g)...
For the following system, 0.400 moles of I_2, . 0.400 moles of Br_2 and 2.10 moles of IBr are placed in a 2.00- L flask. The value of K_c for the reaction is 110.25. What are the concentrations (M) of Br_2 and IBr (in this order) when equilibrium is reached? I_2(g) + Nr_2(g) 2 IBr(g) a) 0.116, 1.22 b) 0.109, 1.14 c) 0.100, 1.05 d) 0.013, 1.42 e)none of these
What is Delta G in kJ for the reaction: Cl_2(g)+ 2 Br^- rightarrow Br_2(l) + 2 Cl^- if [Br^-] = 0.100, [Cl^-] = 0.50, and p(Cl_2) = 1.00 atm? The temperature 25 degree C.
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?
Calculate K_p at 25.00 degree C for reaction #1, ClI(g) leftrightarrow 1/2 ci_2(g) + 1/2 I_2(g), given that delta G degree = -27.9 kJ for reaction #2, CI_2(g) + I_2(g) leftrightarrow 2ClI(g).
For the reaction H_2(g) + Br_2 (g) rightarrow 2HBr(g) K_p = 3.6 times 10^4 at 1496 K. What is the value of K'_p for the following reaction at 1496 K? HBr(g) rightarrow 1/2 H_2(g) + 1/2 Br_2(g) K'_p =
Consider the following reaction: H_2 (g) + Br_2 (g) rlhar 2HBr(g) At some temperature, K_p = 35.5. Within a container, P_H_2 = 5.00 atm, P_Br_2 = 0.700 atm, and P_HBr = 1.60 atm Determine Q_p for this reaction under these conditions. (Round Q_p to 3 sig figs). Q_p = In which direction will the reaction shift to reach equilibrium? (Round Q_p to 3 sig figs).
Calculate the value of K_p for the reaction 2N_2(g) + O_2(g) reversible 2N_2 O(g) at 298.15 K and 1173 K. Thermodynamic data for N_2 O(g) are: delta H degree_t = 82.05 kJ/mol; S degree = 219.9 J/mol middot K; delta G degree f = 104.2 kJ/mol. 298.15 K Did you consider the stoichiometry of the balanced equation for the reaction? Did you check your signs and units? Would you expect K_p at 1173 K to be greater than or less...
Calculate the value of K_p for the equation C(s) + CO_2(g) 2CO(g) K_p = ? given that at a certain temperature C(s) + 2H_2O(g) CO_2(g) + 2H_2(g) K_p^1 = 3.75 H_2(g) + CO_2(g) H_2O(g) + CO(g) K_p^2 = 0.701 K_p =
The rate equation for the reaction 2NO(g) + Br_2(g) rightgarrow 2NOBr(g) was determined experimentally to be: Rate = k[NO]^2 [Br_2] Five possible mechanisms have been proposed (i)-(v). Determine the rate equation for each mechanism below and then decide with reasons, (based on the information given) which mechanism is the most likely. (i) 2NO (g) + Br_2 (g) rightarrow 2NOBr (g) (ii)NO (g) + Br_2 rightwardsharpoonoverleftwardsharpoon NOBr_2 (g) NOBr_2 (g) + NO (g) rightarrow 2NOBr (g) (iii) Br_2 rightwardsharpoonoverleftwardsharpoon Br +...
At elevated temperatures, BrF_5 establishes the following equilibrium. 2BrF_5(g) Br_2(g) + 5F_2(g) The equilibrium concentrations of the gases at 1500 K are 0.0064 mol/L for BrF_5, 0.0018 mol/L for Br_2, and 0.0090 mol/L for F_o. Calculate the value of K_r. The reaction of iron and water vapor results in an equilibrium 3Fe(s) + 4H_2O(g) Fe_3O_4(s) + 4H_2(g) and an equilibrium constant, K_c, of 4.6 at 850 degree C. What is the concentration of hydrogen present at equilibrium if the reaction...