For the reaction H2(g)+I2(g)⇌2HI(g), K= 57.0 at 700 K what can be said about this reaction...
For the reaction H2(g)+I2(g)⇌2HI(g), K= 57.0 at 700 K what can be said about this reaction at this temperature? For the reaction , at 700 what can be said about this reaction at this temperature? The equilibrium lies far to the right. The reaction will proceed very slowly. The reaction contains significant amounts of products and reactants at equilibrium. The equilibrium lies far to the left.
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For the reaction H2(g)+I2(g)⇌2HI(g), K= 57.0 at 700 K what can
be said about this reaction...
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K....
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,...
Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations...
Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations are [H2] = 0.200 M and [I2] = 0.400 M. The equilibrium constant Kc for the reaction following reaction is 57.0 at 700 K. (Show Work) H2(g)+I2(g)<--- ---->2HI(g)
For the reaction H2(g)+I2(g)⇌2HI(g), Kc= 55.3 at 700 K. In a 2.00-L flask containing an equilibrium...
For the reaction H2(g)+I2(g)⇌2HI(g), Kc= 55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.053 g H2 and 4.38 g I2. What is the mass of HI in the flask? Express your answer to two significant figures and include the appropriate units.
H2(g)+I2(g)⇌2HI(g) For the above reaction, Kc=55.3 at 700 K. In a 2.00-L flask containing an equilibrium...
H2(g)+I2(g)⇌2HI(g) For the above reaction, Kc=55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.053 g of H2 and 4.39 g of I2. What is the mass of HI in the flask?
Consider this reaction: H 2 (g)+ I 2 (g)⇌2HI(g) H2(g)+I2(g)⇌2HI(g) A rxn mixture in a 3.73...
Consider this reaction: H 2 (g)+ I 2 (g)⇌2HI(g) H2(g)+I2(g)⇌2HI(g) A rxn mixture in a 3.73 L flask at a certain temperature initially contains 0.766 g H2 and 96.7 g I 2 I2 . At equilibrium, the flask holds 90.3 g HI . Calculate the equilibrium constant (Kc)(Kc) for the reaction at this temperature. Record your answer using two significant figures.
. Consider the reaction: H2(g) + I2(g) ? 2HI(g) A reaction mixture at equilibrium at 175...
. Consider the reaction: H2(g) + I2(g) ? 2HI(g) A reaction mixture at equilibrium at 175 K contains PH2 = 0.958 , PI2 = 0.877 , and PHI= 0.020 . A second mixture not equilibrium, but at the same temperature,contains PH2 = PI2 = 0.621 , and PHI = 0.101 . a) For the second mixture, calculate Q. b) Determine whether the reaction in the second mixture will shift right or shift left.c) Construct an ICE table. Keep in mind your...
The equilibrium constant K for the reaction H2(g) + I2(g) 2HI(g) is 51 at 300oC. A...
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...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g)...
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)...
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
A student ran the following reaction in the laboratory at 673 K: H2(g) + I2(g) 2HI(g)...
A student ran the following reaction in the laboratory at 673 K: H2(g) + I2(g) 2HI(g) When she introduced 0.228 moles of H2(g) and 0.256 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.53×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
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