Expression for equilibrium constant (k) for reversible reaction H2 + I2 <-> 2HI is:
Expression for equilibrium constant (k) for reversible reaction H2 + I2 <-> 2HI is:
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K. A mixture of H2, I2 and HI, each at 0.020 M, was introduced into a container at 700 K. Which of the following is true? At equilibrium, [H2] = [I2] = [HI]. No net change occurs because the system is at equilibrium. The reaction proceeds to the left producing more H2(g) and I2(g). The reaction proceeds to the right producing more HI(g). At equilibrium,...
The equilibrium constant K for the reaction H2(g) + I2(g) 2HI(g) is 51 at 300oC. A 2 L flask was filled with 1 mol H2 and 1 mol I2 at 300oC and the reaction was allowed to come to equilibrium. (i) Calculate the equilibrium concentrations of all three species. If this reaction was performed with the same quantities but at a higher pressure what would be the effect on the position of equilibrium? (ii) If an equilibrium reaction as drawn...
Please explain them also H2 + I2 = 2HI Write the equilibrium constant expression for the equilibrium: N2(g) +3 H2(g)2 NH,(g) What is the K for the following reaction at 427 °C if the equilibrium concentrations are [H20.20 M, [l2l0.20 M and [HI] = 1.47 M? Identify the direction in which the equilibrium is favored The chloride ion concentration of a saturated solution of silver chloride is 1.3 x 105M. Calculate Ksp for silver chloride A 0.13 M solution of...
Given that the reaction H2 (g) + I2 (g) <--> 2HI (g) is at equilibrium and the measured concentrations of each component of the reaction are [H2] = 0.22 M, [I2] = 0.22 M, and [HI] = 1.56 M, write the equilibrium expression and then calculate Keq.
The equilibrium constant, Kc, for the following reaction is 2.02×10-2 at 745 K. 2HI(g) <--> H2(g) + I2(g) Calculate Kc at this temperature for: H2(g) + I2(g) <--> 2HI(g) Kc =
The equilibrium constant, Kc, for the following reaction is 1.68×10-2 at 672 K. 2HI(g) <---> H2(g) + I2(g) Calculate Kc at this temperature for: H2(g) + I2(g) <---> 2HI(g) Kc =
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.293 moles of H2 and 0.293 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M [I2] = M [HI] = M
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.276 moles of H2 and 0.276 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = _____M [I2] =______M [HI] =______M
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium partial pressures of all species when H2 and I2, each at an intitial partial pressure of 1.65 atm, are introduced into an evacuated vessel at 698 K.
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) H2(g) + I2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.329 M HI, 4.41×10-2 M H2 and 4.41×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 2.54×10-2 mol of H2(g) is added to the flask? [HI] = M [H2] = M [I2] = M