**Question 27**A 1.81 mol sample of hydrogen gas occupies 23.1 L. How many moles of hydrogen are needed to fill a 100.7 L container at the same pressure and temperature? Enter your answer in the provided box.[Answer Box]**Explanation:**This question involves the use of the Ideal Gas Law, where the relationship between the volume (V), number of moles (n), temperature (T), and pressure (P) of a gas can be expressed as:\[ PV = nRT \]In this case, since the pressure and temperature are constant, you can use the direct relationship between the volume and the number of moles:\[ \frac{n_1}{V_1} = \frac{n_2}{V_2} \]Where:- \( n_1 = 1.81 \) mol (initial moles of hydrogen)- \( V_1 = 23.1 \) L (initial volume)- \( V_2 = 100.7 \) L (final volume)- \( n_2 \) is the moles of hydrogen needed to findRearrange the relationship to solve for \( n_2 \):\[ n_2 = n_1 \times \frac{V_2}{V_1} \]After calculation, enter the result in the provided answer box.

As there is no change in temperature and pressure , therefore using Avogadro's law "At same…

Answered: A 1.81 mol sample of hydrogen gas…

A 1.81 mol sample of hydrogen gas occupies 23.1 L. How many mol of hydrogen are needed to fill a 100.7 L container at the same pressure and temperature? Enter your answer in the provided box.

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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