A sealed 1.5-L container initially holds 0.00623 mol H2, 0.00414 mol Br2, and 0.0244 mol of HBr at 550 K. when equilibrium is established, [H2]= 0.00467M
H2(g)+Br2(g) <-> 2HBr(g)
A. what are [HBr}eq and [Br2}eq?
B. what are Kc and Kp at 550 K?
C.A 0.00209 mol sample of Br2 is added to the equilibrium mixture of gases. What are the partial pressures of all species once equilibrium is reestablished?
A) the calculations are given below
We would create an ICE table to calculate the change in concentration and euilibrium concentrations of all the species
----------------------------------------------------------------------
Reaction : H2 + Br2 -------------------> 2HBr
Initial 0.00623 0.00414 0.0244
change -0.0015 -0.0015 +0.0030
Equilibrium 0.00467 0.00276 0.0274
----------------------------------------------------------------------------
Thus, the equilibrium concentrations of the species are,
Molarity of H2 = 0.00467/1.5 = 0.00311 M
molarity of Br2 = 0.00276/1.5 = 0.00176 M
molarity of HBr = 0.0274/1.5 = 0.018 M
B.
Kc = [H2][Br2]/[HBr]^2
= (0.018)^2/(0.00311)(0.00176)
= 59.20
pH2 = 0.00311 x 0.0821 x 550 = 0.14
pBr2 = 0.0794
pHBr = 0.812
Kp = (0.812)^2/(0.14)(0.0794)
= 59.31
C. When 0.00209 mol of Br2 was added at equilibrium,
new concentration of Br2 = 0.00176 + 0.00209 / 1.5 = 0.00315
pBr = 0.142
Kp = 33.17
A sealed 1.5-L container initially holds 0.00623 mol H2, 0.00414 mol Br2, and 0.0244 mol of...
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]
A mixture of 1.374 g of H2 and 70.31 g of Br2 is heated in a 2.00 L vessel at 700 K . These substances react as follows: H2(g)+Br2(g)⇌2HBr(g) At equilibrium the vessel is found to contain 0.566 g of H2. 1A) Calculate the equilibrium concentration of H2. 1B) Calculate the equilibrium concentration of Br2. 1C) Calculate the equilibrium concentration of HBr. 1D) Calculate Kc.
A mixture of 0.01341 mol of CH4, 0.01170 mol of H2S, 0.02118 mol of CS2, and 0.02835 mol of H2 is placed in a 1.0-L steel pressure vessel at 3416 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g) 1 CS2(g) + 4 H2(g) At equilibrium 0.003198 mol of H2S is found in the reaction mixture. - Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2. - Calculate KP for this reaction.
For the following reaction, Kp = 2.8 ✕ 104 at 1630 K. H2(g) + Br2(g) equilibrium reaction arrow 2 HBr(g) What is the value of Kp for the following reactions at 1630 K? (a) HBr(g) equilibrium reaction arrow 1/2 H2(g) + 1/2 Br2(g) (b) 2HBr(g) equilibrium reaction arrow H2(g) + Br2(g) (c) 1/2H2(g) + 1/2 Br2(g) equilibrium reaction arrow HBr(g)
The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.20 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 9.20 atm of HBr is introduced into a sealed container at this temperature.
The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.35 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 5.70 atm of HBr is introduced into a sealed container at this temperature.
The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.90 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 14.50 atm of HBr is introduced into a sealed container at this temperature.
5. A mixture of H2 gas (PH2 2.05 atm), CO2 gas (Pco2 4.10 atm) and water vapor (PH20-3.28 atm) are allowed to come to equilibriurm in a closed container. The temperature is 500. K. The equilibrium represented by the equation below is established and the equilibrium partial pressure of H20 is determined to be 3.51 atm. a) Find the equilibrium partial pressures of the CO2, H2, and CO gases. CO2 (g) H2 (g) ←→ CO (g) H2O (g) + +...
The value of the equilibrium constant for the reaction 2HBr(g)<....>H2(g)+Br2(g) is Kc=1.26*10^-12 at 500k. A. what would be the value of the equilibrium constant K'c for the related reaction written in the following fashion? 1/2 H2(g)+1/2 Br2(g)<....>HBr(g). B. what will be the corresponding value for Kp, the pressure form of the equilibrium constant? (R=0.08206)
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) ---------->2HI(g) 1) Calculate the equilibrium concentrations of reactants and product when 0.309 moles of H2 and 0.309 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M? [I2] = M? [HI] = M? 2.The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K: PCl5(g)------->PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a...