Consider mixing 5.00 moles of hydrogen gas and 5.00 moles of iodine in a 2.0 L container in the following reaction: H2(g) + I2(g) 2HI(g) After the reaction at a high temperature, the amounts are measured to be 1.00 moles of hydrogen gas, 3.00 moles of iodine, and 8.40 moles of hydrogen iodide at equilibrium. Is there any problem with this question?Can you calculate K and if yes what is the answer?
Consider mixing 5.00 moles of hydrogen gas and 5.00 moles of iodine in a 2.0 L container in the following reaction: H2(g) + I2(g) 2HI(g) After the reaction at a high temperature, the amounts are measured to be 1.00 moles of hydrogen gas, 3.00 moles of iodine, and 8.40 moles of hydrogen iodide at equilibrium. Is there any problem with this question?Can you calculate K and if yes what is the answer?
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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Consider mixing 5.00 moles of hydrogen gas and 5.00 moles of iodine in a 2.0 L container in the following reaction:
H2(g) + I2(g) 2HI(g)
After the reaction at a high temperature, the amounts are measured to be 1.00 moles of hydrogen gas, 3.00 moles of iodine, and 8.40 moles of hydrogen iodide at equilibrium. Is there any problem with this question?Can you calculate K and if yes what is the answer?
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