Calculate equilibrium concentration from an constant 12 at 25degree C k_s = 6.90 for the following...
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...
The following reaction was allowed to come to equilibrium at 35 degree C. The initial molar concentration for SO_3 is 0.675 M ([SO_3| = 0.675 M) and the initial molar concentration for CO_2 is 0.444 M (|CO_2] = 0.444 M). After the reaction reached equilibrium the concentration of CO_2 now equals 0.214 M ((CO_2] = 0.214 M). What is the K_c value for the reaction? 0.00987 0.0342 7.31 11.8 16.7 At 35 degree C the equilibrium constant value (K_c) for...
5-3 Write the equilibrium constant expression of this reaction and calculate the concentration of all the gases at equilibrium for the reaction: CO(g) + H20 (g) = CO2(g) + H2 (g) Given that the initial concentrations of all the gases are 0.05 M and that Kc = 5.1 at 700 K.
. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part II (y values and the best-fit line equation from Part I to calculate the [FeSCN2"), at equilibrium. Show two sets of calculations and complete Table 6 below. Sample Calculation with hypothetical values of Absorbance from Table 4 & fitted egn. from Table 3 y = mx + b (y is absorbance) 0.0620 - 2000x -0.0250 x-0.0620+ 0.0250 2000 = 4.35 x 10 с D...
12. Calculate the equilibrium constant for the following reaction if the equilibrium concentrations of NH3, N2, and H, are 0.0100 M, 0.100 M, and 0.162 M, respectively. 2NH, (g) N2(g) + 3H2(8)
The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=7.3 What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?
Calculate the equilibrium concentrations of N2O4and NO2 at 25 ∘C if the initial concentrations are [N2O4]= 0.0150 M and [NO2]= 0.0360 M. The equilibrium constant Kc for the reaction N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C. Part A Calculate the equilibrium concentration of N2O4. Express your answer with the appropriate units. Part B Calculate the equilibrium concentration of NO2. Express your answer with the appropriate units.
Beers law solve for E3 and E4 showing work Part II. Equilibrium Constant Calculations Calculate the initial moles of Fe3+ and SCN- for solutions E2 through E6 and record these values in the table on your Data Sheet. You obtain the moles of the reactants by multiplying their molarity by the volume (in L) of their solution used. Determine the equilibrium concentration of FeSCN2+ for each of the solutions E2-E6 from your Beer’s Law plot. Using these equilibrium concentrations, the...
4. Calculate the equilibrium constant in terms of concentration (K) for the following reaction when at equilibrium, there are 0.0406 mol of CH,OH, 0.170 mol of CO, and 0.302 mol of H2 in a 2.00 L container. (Hint: you will have to calculate equilibrium concentrations using moles and volume.) COⓇ) + 2 H20) = CH3OH)
Part A The equilibrium constant, K. of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium, For a gaseous reaction with the general form aA +B=cC+ DD the K, and Ky expressions are given by CDI K= A "B" (PE) K- Phosgene (carbonyl chloride). COClz, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine...