A student ran the following reaction in the laboratory at 698 K: H₂(g) + I₂(g) 2HI(g) When she introduced H₂(g) and I₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of H₂ was 4.70 atm and the initial partial pressure of I₂ was 3.47 atm, she found that the equilibrium partial pressure of 1₂ was 0.411 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction.

A student ran the following reaction in the laboratory at 698 K: H₂(g) + I₂(g) 2HI(g) When she introduced H₂(g) and I₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of H₂ was 4.70 atm and the initial partial pressure of I₂ was 3.47 atm, she found that the equilibrium partial pressure of 1₂ was 0.411 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction.

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...

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||| Microsoft O W OCHEMICAL REACTIONS Dilution A chemist must prepare 500. mL of 1.00 M aqueous silver perchlorate (AgCIO4) working solution. She'll do this by pouring out some 1.94 silver perchlorate stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the silver perchlorate stock solution that the chemist should pour out. Be sure your answer has the correct number of significant digits. 00 mL Microsoft Microsoft 6.52.210... Explanation Check 9,180 ☐ X 285 S C Q NOV 10 ||| tv SO17 A mol L ( aqueous 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility P eBook W 1 0
13. Nitric acid, HNO3, is a strong acid in aqueous solutions. It is sold commercially as a concentrated solution with a density of 2.14 kg.L-¹ and containing 58% mass of HNO3. We introduce 10.0 mL of this solution in a 250.00 mL volumetric flask which is then filled to the mark with distilled water. This solution is called S. S is then diluted 100 times to afford solution S'. a. What is the definition of a strong acid? | b. What is the concentration of solution S"? c. What is the pH of solution S'?
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OCHEMICAL REACTIONS Dilution A chemist must prepare 875. ml. of 335. M aqueous copper (11) fluoride (CuF) working solution. She'll do this by pouring out some 407. µμM aqueous copper (11) fluoride stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in ml. of the copper (11) fluoride stock solution that the chemist should pour out. Round your answer to 3 significant digits. 0 04 0/5 Y
10 Ethylene (CH,CH,) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 10º kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH,CH,) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 60.0 L reaction tank with 22.0 atm of ethane gas and raises the temperature to 500. °C. She believes K =0.050 at this temperature. Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken about the correct value of K , and the mass percent of ethylene you calculate may not be what she actually observes. %
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A chemistry student must write down in her lab notebook the concentration of a solution of sodium thiosulfate. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: • The label on the graduated cylinder says: empty weight: 6.0 g • She put some solid sodium thiosulfate into the graduated cylinder and weighed it. With the sodium thiosulfate added, the cylinder weighed 94.86 g. • She added water to the graduated cylinder and dissolved the sodium thiosulfate completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 122.28 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. 山。 g.mL 1 x10 X Ś
PbCrO4 is a common pigment called chrome yellow (or school bus yellow). It has a solubility of 1.71 x 10-4 g/L. The solubility product of PbCrO4, Ksp = ________. Enter the result in scientific notation to 1 decimal. e.g. enter 5.6x10-5 as 5.6E-5.
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