**The Haber Process and Ammonia Synthesis**The Haber Process synthesizes ammonia at elevated temperatures and pressures. In this process, nitrogen gas (N₂) reacts with hydrogen gas (H₂) to produce ammonia (NH₃). The balanced chemical equation for this reaction is:\[ \text{N}_2 (\text{g}) + 3 \text{H}_2 (\text{g}) \rightarrow 2 \text{NH}_3 (\text{g}) \]Suppose you combine 1580 liters of nitrogen gas and 4245 liters of hydrogen gas at standard temperature and pressure (STP). The mixture is heated to facilitate the reaction, and then the ammonia is isolated from the reaction mixture. The question asks what volume of ammonia, measured at STP, would be produced given that the reaction goes to completion.This is a classic example of stoichiometry in chemical reactions where the volumes of reactants and products are calculated. Since volumes of gases at STP are directly proportional to moles (Avogadro's Law), the stoichiometric coefficients from the balanced equation can be used to determine the volume of ammonia produced.

Given; N2 (g) + 3 H2 (g) ➝ 2 NH3 (g) At STP, Volume of nitrogen gas (N2) reacts = 1580 L Volume of the hydrogen gas (H2) = 4245 L Volume of ammonia gas (NH3) produced = ? Note; At STP 1 mole of any gas occupies 22.4 L volumeCalculating the moles of N2 and H2 gas reacts; Determining the limiting reactant; N2 (g) + 3 H2 (g) ➝ 2 NH3 (g) According to the balanced chemical equation; Calculating the moles of Ammonia gas (NH3) produced: N2 (g) + 3 H2 (g) ➝ 2 NH3 (g) Number of moles of product depends on the number of moles of limiting reactant, so according to the the balance chemical equation;Calculating the volume of Ammonia gas (NH3) produced at STP:Conclusion; So, the volume of Ammonia gas (NH3) produced at STP is 2830 L. Answer: 2830 L

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The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4245 L of hydrogen gas at STP, heat the mixture to run the reaction, then isolate the ammonia from the reaction mixture. What volume of NH3 in liters, measured at STP, would be produced? Assume the reaction goes to completion. N2 (g) +3 H2 (g)→2 NHs (g)

The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4245 L of hydrogen gas at STP, heat the mixture to run the reaction, then isolate the ammonia from the reaction mixture. What volume of NH3 in liters, measured at STP, would be produced? Assume the reaction goes to completion. N2 (g) +3 H2 (g)→2 NHs (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

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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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.

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**The Haber Process and Ammonia Synthesis**

The Haber Process synthesizes ammonia at elevated temperatures and pressures. In this process, nitrogen gas (N₂) reacts with hydrogen gas (H₂) to produce ammonia (NH₃). The balanced chemical equation for this reaction is:

\[ \text{N}_2 (\text{g}) + 3 \text{H}_2 (\text{g}) \rightarrow 2 \text{NH}_3 (\text{g}) \]

Suppose you combine 1580 liters of nitrogen gas and 4245 liters of hydrogen gas at standard temperature and pressure (STP). The mixture is heated to facilitate the reaction, and then the ammonia is isolated from the reaction mixture. The question asks what volume of ammonia, measured at STP, would be produced given that the reaction goes to completion.

This is a classic example of stoichiometry in chemical reactions where the volumes of reactants and products are calculated. Since volumes of gases at STP are directly proportional to moles (Avogadro's Law), the stoichiometric coefficients from the balanced equation can be used to determine the volume of ammonia produced.

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