**Chemical Reaction and Gas Volume Calculation**Magnesium burns in air to produce magnesium oxide, \( \text{MgO} \), and magnesium nitride, \( \text{Mg}_3\text{N}_2 \). Magnesium nitride reacts with water to give ammonia.\[ \text{Mg}_3\text{N}_2 (s) + 6\text{H}_2\text{O} (l) \rightarrow 3\text{Mg(OH)}_2 (s) + 2\text{NH}_3 (g) \]**Problem Statement:**What volume of ammonia gas at \( 25^\circ \text{C} \) and \( 740 \, \text{mmHg} \) will be produced from \( 3.51 \, \text{g} \) of magnesium nitride?**Solution:**Volume = \(\_\_\_\_\_\_\_\_\_\_\_\_\) LThis exercise involves using stoichiometry and the ideal gas law to calculate the volume of ammonia gas produced.

Magnesium burns in air to produce magnesium oxide MgO. and magnesium nitride reacts with water to give ammonia (Ma3N2) . Reaction : Mg3N2 (s) + 6H2O ------> 3Mg(OH)2(s) + 2NH3(g). We have to calculate the volume of ammonia gas at 25°C and 740 mmHg will be produced from 3.51 g of ammonia nitride .Now, We know , Molar mass of NH3 = 17.0306 g/mol. Molar mass of Mg3N2 = 100.9494 g/mol Pressure (P) = 740mmHg = 753 Torr = 0.973684 atm Temperature (T) = 25°C = 298.15 K. Mass of Mg3N2 is = 3.51 g. First calculate the moles of ammonia from the given mass.... (3.51 g Mg3N2).(1 mol Mg3N2 /100.9494 g Mg3N2).(2 mol NH3 / 1 mol Mg3N2) = 0.0702 mol NH3 Now by using the equation PV=nRT => V = nRT/ P putting the value and we have.. V = nRT / P = (0.0702 mol).(0.08206 L atmmol- K-).(297.15K) / 0.973684 atm. = 1.74 L. Final ans : the volume is 1.74 L

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Magnesium burns in air to produce magnesium oxide, MgO, and magnesium nitride, Mg3N2. Magnesium nitride reacts with water to give ammonia. Mg3 N2 (s) + 6H20(1) → 3Mg(OH)2 (s) + 2NH3 (g) What volume of ammonia gas at 25°C and 740. mmHg will be produced from 3.51 g of magnesium nitride? Volume =

Magnesium burns in air to produce magnesium oxide, MgO, and magnesium nitride, Mg3N2. Magnesium nitride reacts with water to give ammonia. Mg3 N2 (s) + 6H20(1) → 3Mg(OH)2 (s) + 2NH3 (g) What volume of ammonia gas at 25°C and 740. mmHg will be produced from 3.51 g of magnesium nitride? Volume =

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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