Please explain them also
H2 + I2 = 2HI
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Please explain them also H2 + I2 = 2HI Write the equilibrium constant expression for the...
9. The equilibrium constant for the reaction H2(g) + I2(g) 2HI(g) has a value of 54.6 at 699K. What are the equilibrium concentrations of H2, I2, and HI if the initial concentrations at this temperature are 0.0800M H2 and 0.0700 M I2. 10. Find the pH and pOH of a solution prepared by dissolving 9.85 grams of NaOH into a total aqueous solution volume of 75.0 ml. 11. Using the data in Appendix B of your text, calculate the values...
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.
EXPLAIN PLENSE 4. Consider the reaction which is at equilibrium: Fe203(s) +2 H2(g) List all ways to drive the equilibrium to the right. 2 Fe(s) +3 H20(g), AH > 0 5. A chemist makes a saturated solution of Ga S and determines [Ga3Tley to be 0.00542 M. What is (4 pts.) the value,for Ksp of Ga2S3 at this 6. A certain weak acid has a Ka of 3.82 x 104 What is the pH and % ionization of a 6.00...
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,...
Given the equilibrium reaction: 2HI(g) H2(g) + I2(g) A sample mixture of HI, H2, and 12, at equilibrium, was found to have [H2]- 1.4 x 102 Mand [HI 4.0 x 102 M. If Keq 1.0 x 10, calculate the molar concentration of I2 in the equilibrium mixture, Enter your answer in the provided box. ]= м
The equilibrium constant for the following reaction is 1.80x102 at 698K 2HI(8)H2( ) +I2(g) If an equilibrium mixture of the three gases at 698K contains 2.35x102 M HI(g) and 2.63x10-2 M H, what is the equilibrium concentration of I? Submit Answer Retry Entire Group 9 more group attempts remaining
Consider the following chemical reaction: H2 (g) + I2 (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.02, 0.021 and 0.160 M respectively. The value of Keq for this reaction is __________.
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...
Given the following information calculate the equilibrium concentrations of all species. H2 + I2 = 2HI Kc=54.3 Initial [H2]=[I2]=.500 M, [HI]=0