2. A chemist reacts 0.51 mole H₂ with 0.36 moles of N₂ to make NH, If the total pressure before the reaction begins is 1.07 atm find the partial pressure of N₂ and H₂. She then runs the reaction until it stops and measures the final pressure to be 1.23 atm. Find the partial pressure of all gases at the end of the reaction. N₂ (g) + H₂ (g) NH3 (g)

2. A chemist reacts 0.51 mole H₂ with 0.36 moles of N₂ to make NH, If the total pressure before the reaction begins is 1.07 atm find the partial pressure of N₂ and H₂. She then runs the reaction until it stops and measures the final pressure to be 1.23 atm. Find the partial pressure of all gases at the end of the reaction. N₂ (g) + H₂ (g) NH3 (g)

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

Chapter5: Gases

Section: Chapter Questions

Problem 102E: Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated...

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

2. A chemist reacts 0.51 mole H₂ with 0.36 moles of N₂ to make
NH, If the total pressure before the reaction begins is 1.07
atm find the partial pressure of N₂ and H₂. She then runs the
reaction until it stops and measures the final pressure to be
1.23 atm. Find the partial pressure of all gases at the end of
the reaction.
N₂ (g) + H₂ (g)
NH3 (g)

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