H2 + Cl2
2HCl
H2 | Cl2 | 2HCl | |
Initial | 0.5/2 | 0.5/2 | 0 |
Change | -x | -x | 2x |
Equilibrium | 0.5/2-x | 0.5/2-x | 0.11 |
Keq = [HCl]2 /[H2][Cl2]
[HCl] = 0.11 = 2x therefore ,x = 0.11/2 = 0.055
[H2] = 0.5/2 - 0.055 = 0.195
[Cl2] = 0.5/2 - 0.055 = 0.195
Keq = (0.055)2/(0.195)2 = 0.079
Suppose that a 2.00L glass flask is 0.500 mol of H2 and 0.500 mol Cl2 are...
Suppose a 250. mL flask is filled with 0.10 mol of Cl2 and 1.4 mol of HCl. The following reaction becomes possible: H2(g)+Cl2(g)=2HCl(g) The equilibrium constant for this reaction is 0.414 at the temperature of the flask. Calculate the equilibrium molarity of . Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 1.9 mol of Cl2, 0.70 mol of HCl and 1.7 mol of CCI4. The following reaction becomes possible Cl2(g)+ CHCI3)HCI (g)+CCI4g) The equilibrium constant K for this reaction is 7.09 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places
Suppose a 250. mL. flask is filled with 1.8 mol of Cl2 and 0.60 mol of HCl. The following reaction becomes possible: H(+Cl()2HCI) The equilibrium constant K for this reaction is 8.25 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 1.3 mol of H2 and 0.10 mol of HC1. The following reaction becomes possible: H2(g) + Cl2(g)-2HCl (g) The equilibrium constant K for this reaction is 3.03 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places.
Suppose a 500. ml flask is filled with 1.2 mol of Cl, and 0.80 mol of HCl. The following reaction becomes possible: H2(g) + Cl2(g) = 2HCl (g) The equilibrium constant K for this reaction is 0.419 at the temperature of the flask. Calculate the equilibrium molarity of Cl. Round your answer to two decimal places. xs ?
Suppose a 250. ml flask is filled with 0.50 mol of H, and 0.40 mol of HCl. The following reaction becomes possible: H2(g) + Cl2(g) = 2HCl (g) The equilibrium constant K for this reaction is 5.61 at the temperature of the flask. Calculate the equilibrium molarity of Cl. Round your answer to two decimal places. TOM xo?
Suppose a 250. ml flask is filled with 1.5 mol of Cl, and 1.3 mol of HCl. The following reaction becomes possible: H2(g) + Cl2(g) 2HCl (8) The equilibrium constant K for this reaction is 0.560 at the temperature of the flask. Calculate the equilibrium molarity of H. Round your answer to two decimal places. OM * 5 ?
the reaction 2HCl=H2(g)+Cl2(g) has a Kc=3.2x10^-32.A 0.500-L
reaction vessel initially contains 0.025 mol of HC
The reaction 2HCI(g)Hlg) + Cl(e) has a K 0.025 mol of HCI. 3.2x103. A 0.500-L reaction vessel initially contains A. Write an equation for Ke using the chemical entities. B. Set up and complete an ICE table C. Determine the equilibrium concentrations of H2 and Ch. To receive full credit, you must show any appropriate substitutions and all of your algebra work. Use the attached...
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.
2IBrig), K.-280 at 150°C. Suppose that 0.500 mol IBr in a 1.00 1(g) + Bn(g) 4. For the reaction L flask is allowed to reach equilibrium at equilibrium at 150°C. What are the equilibrium concentrations of IBr, h, and Br2?
2IBrig), K.-280 at 150°C. Suppose that 0.500 mol IBr in a 1.00 1(g) + Bn(g) 4. For the reaction L flask is allowed to reach equilibrium at equilibrium at 150°C. What are the equilibrium concentrations of IBr, h, and Br2?