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The balanced reaction taking place is given as, => CO (g) + 2 H2 (g) → CH3OH (g) Given: Volume of vessel = 1.95 L. Temperature = 305 K Partial pressure of CO = 232 mm Hg. And partial pressure of hydrogen = 396 mm Hg. From the balanced reaction, we can say that 1 mm Hg of CO will require 2 mm Hg of H2 at constant volume and temperature to completely react. Hence pressure of H2 required = pressure of CO × 2 = 232 × 2 = 464 mm Hg. Since the pressure of hydrogen taken is much less than required. Hence the limiting reagent is hydrogen. Since the limiting reactant will react completely theoretically. And 2 mm Hg of hydrogen is reacting to produce 1 mm Hg of methanol. Hence pressure of methanol produced = Pressure of hydrogen reacting2 = 3962 = 198 mm Hg According to ideal gas law (applying for methanol to get moles), => PV = nRT where P = pressure in atm = 198760 = 0.2605263 atm approx. (Since 1 atm = 760 mm Hg) V = volume of flask = 1.95 L n = moles of methanol produced theoretically R = gas constant = 0.0821 atm.L/K.mol T = temperature in K = T in °C + 273 = 305 K Hence substituting the values we get, => 0.2605263 × 1.95 = n × 0.0821 × 305=> n = 0.0202882 mol approx.Since molar mass of methanol is 32 g/mol.Hence the theoretical yield of methanol = moles × molar mass =0.0202882 × 32 = 0.649 g approx. Hence the answer is hydrogen gas and 0.649 g.

Science

Chemistry

I Review | Constants | MISSED THIS? Watch IWE 10.14; Read Section 10.10. You can click on the Review link to access the section in your e Text. Part A Carbon monoxide gas reacts with hydrogen gas to form methanol via the following reaction: Identify the limiting reactant and determine the theoretical yield of methanol in grams. CO(g) + 2H,(5)->CH,OH(g) Express your answer with the appropriate units. A 1.95 L reaction vessel, initially at 305 K, contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 396 mmHg > View Available Hint(s) HA

I Review | Constants | MISSED THIS? Watch IWE 10.14; Read Section 10.10. You can click on the Review link to access the section in your e Text. Part A Carbon monoxide gas reacts with hydrogen gas to form methanol via the following reaction: Identify the limiting reactant and determine the theoretical yield of methanol in grams. CO(g) + 2H,(5)->CH,OH(g) Express your answer with the appropriate units. A 1.95 L reaction vessel, initially at 305 K, contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 396 mmHg > View Available Hint(s) HA

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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