(a)
1.3 g H2O (molar mass 18 g/mol) =
2.0 g Cl2O (molar mass 87 g/mol)
x moles of H2O will react with x moles of Cl2O to form 2x moles of HOCl.
The equilibrium concentrations are
This is quadratic equation with solution
or
The negative value is discarded since the number of moles cannot be negative.
The equilibrium concentrations are
(b)
1.5 mol pure HOCl is placed in the flask
2x moles of HOCl will give x moles of H2O and x moles of Cl2O
The equilibrium concentrations are
The equilibrium concentrations are
At 25°C, K = 0.090 for the following reaction. H20(g) Cl20(g)2 HOCI(g) Calculate the concentrations of...
Reaction Quotients and Direction of Reaction The equilibrium constant is 0.090 at 25°C for the reaction: H20(g)Cl20(g) 2HOCI(g) + For each of the following sets of initial conditions, at 25°C, in which direction will the reaction position shift (significantly)? = 240.0 torr, P(Cl20) = 56.60 torr, P(HOCI) P(H20) 34.97 torr. Neither P(H20) 123.0 torr, P(Cl20) = 86.50 torr, P(HOCI) 30.94 torr. Neither P(H20) 536.0 torr, P(Cl20) = 53.80 torr, P(HOCI) 76.42 torr. Right A 5.0-L flask contains 6.725x 102 mol...
121.sp2020_quiz5_4.pdf (page 4 of 4) 4. The following reaction has a K value of 0.090 at 25 °C. If 2.00 mol of H20 and 2.00 mol of Cl20 are placed in a 5.00 L flask at 25 °C and the mixture comes to equilibrium, what are the equilibrium concentrations of all species? H2O(g) + Cl20 (g) 2HOCI(g)
This question has multiple parts. Work all the parts to get the most points. At 25°C, K 0.090 for the reaction H, 0(g) + C,O(g) ? 2 HOCl(g) Calculate the concentrations of all species at equilibrium for each of the following cases. aL0g H0 and 2.0 g Cl,O are mixed in a 1.0-L flask. H2O] C20 [HOC?]- b 1.0 mole of pure HOCl is placed in a 20-L flask. [H20] = [C101 =
Please explain and show steps! Thanks! At 35°C, K = 1.6×10-5 for the following reaction 2 NOCI(g)2 NO(g) + Cl2(g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures (a) 2.0 mol of pure NOCl in a 1.7-L flask [NOCI] [Cl2l (b) 7.2 mol of NO and 3.6 mol of Cl2 in a 1.2-L flask [NOCI] [NO] [Cl2l (c) 1.7 mol of NOCI and 1.7 mol of NO in a 2.0-L flask [NOCI] [NO]...
Find the equilibrium concentration of HOCI in the decomposition equilibrium reaction if the initial concentrations of H20 and Cl20 are both 0.980 M, and that Kc = 0.0900. 2HOCI(g) = H2O(g) +C120(g)
14. For the reaction: 2NOCI(g) 2NO(g) + Club), K = 1.6 x 10. What are the equilibrium concentrations of each species it tions of each species if 1.0 mole of NOCI is initially placed in an empty 2.0 L flask? 14. For the reaction: 2NOCI(B) = 2NO(g) + Cl2(g), K = X 1.6*10 What are the equilibrium concentrations of each species if 1.0 mole of NOCI is initially placed in an empty 2.0 L flask?
63. At 35°C, K = 1.6 x 10-6 for the reaction 2NOCI(9) = 2NO(g) + Cl2 (9) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.0 moles of pure NOCI in a 2.0-L flask Answer b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask Answer c. 2.0 moles of NOCI and 1.0 mole of Cl, in a 1.0-L flask
At 35°C, K =2.0 x 10-8 for the reaction 2 NOCI(9) = 2 NO(g) + Cl2(9) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.2 moles of pure NOCI in a 2.0-L flask [NOCI) = M [NO] = | М [Cl] = M b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask [NOCI) = M [NO] = M (Cl2] = 1 M c. 2.0 mole of NOCl...
At 35°C, K = 2.3 x 10-5 for the reaction 2 NOCI(9) – 2 NO(g) + Cl (9) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.4 moles of pure NOCl in a 2.0-L flask [NOCI) - t t M t [NO] - M t [Cl] - M b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask [NOCI] - M [NO] - M (Cl) - M c....
At 35°C, K = 1.6 10-5 for the reaction 2 NOCI(g) 52 NO(g) + Cl2(8) If 3.6 mol NO and 1.8 mol Cl2 are placed into a 1.0-L flask, calculate the equilibrium concentrations of all species. [NOCI) - [NO] - м [C12] - Submit Answer Try Another Version 1 item attempt remaining