In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K. Part B The following reaction was performed in a sealed vessel at 750 °C: H2 (g) + I(g) = 2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]= 3.70M and [I] = 2.45M. The equilibrium concentration of I, is 0.0200 M . What is the equilibrium constant, Kc, for the reaction at this temperature? Express your answer numerically. > View Available Hint(s) ? ΑΣφ Ke = 8:05 AM 3/1/2021

In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K. Part B The following reaction was performed in a sealed vessel at 750 °C: H2 (g) + I(g) = 2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]= 3.70M and [I] = 2.45M. The equilibrium concentration of I, is 0.0200 M . What is the equilibrium constant, Kc, for the reaction at this temperature? Express your answer numerically. > View Available Hint(s) ? ΑΣφ Ke = 8:05 AM 3/1/2021

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

7. A technician is setting up a laboratory to standardise ~0.0200 mol dm–3 KMnO4. What mass of Mohr’s salt [FeSO4(NH4)2SO4·6H2O] would the technician be required to weigh out to produce a 5.00 L solution of Mohr’s salt such that 25.0 cm3 aliquots of the salt would require a titre of 20.0 cm3 to standardise the KMnO4 solution?
please and thank you!
When zinc reacts with hydrochloric acid, zinc chloride and hydrogen gas are formed. After writing a balanced a equation, determine how many mL of 0.50 M HCl are required, with excess zinc, to produce 128 mL of hydrogen gas at 1.00 bar and 20.oC. Balanced equation: Zn + 2HCL --> ZnCl2 + H2
8-7. Suppose a 185 gram sample of hydrogen reacts with an excess of nitrogen dioxide as follows: 2 NO2 (g) + 7 H2 (g) → 2 NH3 (g) + 4 H2O(g) Both products are collected together (separate from any remaining reactants) in a 325 liter vessel at 512 K. a. How many moles of ammonia gas are produced? b. How many moles of water vapor are produced? c. What is the total pressure in the product collection vessel after the reaction is complete? 8-8. Suppose 93.4 grams of aluminum sulfide are added to 5.00 liters of a 0.844 M hydrochloric acid solution and the following reaction takes place: 6 HCl (aq) + Al2S3 (s) → 3 H2S (g) + 2 AlCl3 (aq) a. Which reactant is the limiting reactant? b. Briefly explain how you know which reactant is limiting. Be specific. Use complete sentences. c. What volume of hydrogen sulfide gas is collected at STP? d. How many grams of aluminum sulfide will be left over at the end? e. What is the final molarity of HCl?
Time Left:0:55:00 A student completes the experiment The Universal Gas Constant and obtains the following data for one trial. mass of magnesium (g): Initial gas volume (ml): Final Volume (mL): Temperature (°C): Atmospheric pressure (inHg): Ah (cm of water): F3 80 모 Calculate the partial pressure of hydrogen, PH2, for this trial. Give your answer in torr (mmHg). 1 in Hg = 25.4 mmHg 1 cm water = 0.735559 mmHg 1 mol Mg = 24.305 g Mg TABLE D-4 TEMP 1_DEG₁_C_1 1 3 I 1 1 Q F4 0 1 = 2 3 4 5 6 7 8 10 11 12 13 14 0.0 0.1 0.0326 0.00 35.30 21.3 30.21 16 17.13 F5 6.100 | 6.143 1 6.544 1 6.589 0.2 1 VAPOR PRESSURE OF HATER 0-30 DEG. C IN MM HG 1 4.579 4.612 4.646 | 4.924 | 4.959 4.995 15.291 4.660 4.714 5.0315.068 5.329 5.367 5.406 5.445 4.7484.783 4.818 5.104 | 5.141 | 5.178 5.484 5.523 5.563 5.888 5.930 6.230 16.274 6.318 5.363 15.683 15.723 | 5.764 | 5.8051 5.146 6.186 6.636 5.972 1 6.0141 6.057 1 6.407 1 6.453 6.498 1 6.82 | 6.729 6.776 6.823 | 6.871 | 6.919 | 6.967 1 T T 1 I T I 1 17.0167,064…
Mid-latitude ozone depletion can happen because of denitrification that occurs on cold sulfuric acid droplets. O True O False
5. The barometric pressure is generally given in units of inHg. Convert inHg to atm. Recall that 2.54cm = linch. Use dimensional analysis.
4
In a biology laboratory, the teacher provided the each student group with two long bones (chicken) without the flesh. Following teacher's guidance, one of the long bone was placed in a beaker containing vinegar (7% acetic acid), a weak acid and let it sit for 3 days at 370 C in an incubator. The other long bone was left in beaker containing distilled water and placed in the same incubator. The students were very curious - on the 4th day, they used gloves and removed the bones from respective jars with utmost care. The teacher asked them to write their observations (what happened) and the explanation (why did it happen) in the lab notebook in view of the structure-function relationship of bone. Assuming we are doing this lab activity. describe the observation in the vinegar treated long bone compared to the control set and explain  what actually happened to justify observation
How many are in 2.50 L of CO2 @ STP? Group of answer choices 1.11 X 10-5 1.11 x 10 10 1.12 x 10 5 1.11 X 108
Argon diffuses at a rate of 1.45 meters in 8.65 minutes. How long will it take helium to diffuse 5.86 meters under the same conditions? (I should see the calculation of rates first.)
8,9