Suppose a 5.00 L nickel reaction container filled with 0.0090 M H2 is connected to a 3.00 L container filled with 0.201 M F2. Calculate the molar concentration of H2 at equilibrium.
Suppose a 5.00 L nickel reaction container filled with 0.0090 M H2 is connected to a...
Consider the following reaction: 2HF(g) H2(g) + F2(g) Initially a container is filled with pure HF(g) at a pressure of 2 atm, after which equilibrium is reached. If y is the partial pressure of H2 at equilibrium, Express the value of Kp using y. a) b) If K = 0.01 at this temperature, calculate the equilibrium concentrations of the 3 species.
3. Consider the following reaction: 2HF(g) = H2(g) + F2(g) Initially a container is filled with pure HF(g) at a pressure of 2 atm, after which equilibrium is reached. If y is the partial pressure of H2 at equilibrium, a) Express the value of Kp using y.
1.00 mol Fe(s) and 3.00 mol H2 (g) were placed into a 5.00 L reaction vessel where the Kc for the reaction below is 0.825 at 400K. What is the concentration of hydrogen gas at equilibrium? Fe2O3 (s) + 3H2 (g) <----> 2Fe (s) + 3H2O (g)
A 5.00 L beaker is filled with an initial 2.00 mol of H2, 2.00 mol of I2, and 5.00 mol of HI with an Kc=200 at 500 K. Draw the Ice table and with that information, determine the equilibrium constant concentrations. Does Kp=Kc? Explain.
Consider the reaction: N2O4 (g) container. Suppose initially [N2O. (g)l- 0 and [NO (g)lo - 3.0 M. Further suppose that at some temperature the reaction proceeds to equilibrium and [NO (g)l - 2.0 M, i.e. the equilibrium concentration of [NO.g)).-2.0 M. Sketch a reasonable plot of molar concentrations of each substance as a function of time showing the progress of reaction to reach equilibrium. (Make sure the axes are labeled! Make sure you show linear increments along each axis!!!). 8....
Hydrogen iodide decomposes according to the reaction 2 HI(g) = H2(g) +1268) A sealed 1.50-L container initially holds 0.00623 mol of H2, 0.00414 mol of 12, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H2(g) is 0.00467 M. What are the concentrations of HI(g) and 12(g)? 112le [HI]
Suppose that 0.1000 mole each of H2 and I2 are placed in 1.000-L flask, stoppered, and the mixture is heated to 425oC. At equilibrium, the concentration of I2 is found to be 0.0210 M. a) What are the equilibrium concentrations of H2 and HI, respectively? Calculate Kc for the following reaction at 425oC. H2(g) + I2(g) ⇄ 2 HI(g) b) If the initial concentrations of H2 and I2 are 1.000 M each, and the initial concentration of HI is 0.000,...
Suppose a 500.mL flask is filled with 0.60mol of H2 and 0.70mol of Cl2. The following reaction becomes possible: H2(g) + Cl2(g) 2HCl(g) The equilibrium constant K for this reaction is 5.52 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places.
For the reaction: 2HI(g) ↔ H2(g) + I2(g) Keq = 0.016 Initially a container contains 0.60 M HI, 0.038 M H2, and 0.15 M I2 at equilibrium. What is the new equilibrium concentration of H2, if the H2 concentration is increased by 0.276 M?
4. Consider the following reaction at equilibrium CO(g) + H2O(g) + CO2(g) + H2(g) 2.50 mole of CO(g) and 2.50 mole of H2O(g) gas at 588 K are mixed in a 10.00 L container. (Kc = 31.4 at 588 K) Calculate the concentration of CO(g), H2O(g), CO (g), and H.(g) at equilibrium. 5. Consider the following reaction: CO(g) + H2O(g) + CO2(g) + H2(g) (a) If a 10.00L container has 2.50 mole of CO(g), 2.50 mole of H2O(g), 5.00 mole...