**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

Science

Chemistry

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...

See similar textbooks

Similar questions

A sample of aluminum metal was reacted with hydrochloric acid, producing AlCl3AlCl3 (aq) and H2H2 gas. If 143 mL of H2H2 gas was formed at 397 torr and 55.1 °C, calculate the grams of aluminum reacted.2Al(s)+6HCl(aq)→2AlCl3(aq)+3H2(g) A. 0.0499 B. 0.349 C. 16.4 D. 0.0955 E. 0.00414
Given the following reaction, if 1.7 L of nitrogen completely react with an excess of охygen, how many liters of N2O5 are produced, assuming no change in pressure or temperature? 2N2(g) + 5O2(g) → 2N2O5(g)
The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4590 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 , measured at STP, would be produced? Assume the reaction goes to completion. N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)
Potassium is a very reactive metal. It reacts violently with water according to the reaction: 2K(s)+2H2O(l)→2KOH(aq)+H2(g) If 0.497 grams of potassium reacts with an excess amount of water, what volume of H2 gas will be produced at 28 oC and 0.980 atm? mL
Zinc reacts with aqueous HCl to produce hydrogen gas (H2) according to the following reaction equation:Zn (s) + HCl (aq) → ZnCl2 (aq) + H2 (g)The hydrogen gas is collected over water. If you collected 260 mL of H2 at 25 oC, and the total pressure was 745 mm Hg, calculate the mass of H2 collected over water.
A self-contained underwater breathing apparatus uses canisters containing potassium superoxide. The superoxide consumes the CO2 exhaled by a person and replaces it with oxygen. 4 KO2 (s) + 2 CO2 (g) → 2 K₂CO3 (s) + 3 O2(g) What mass of KO2, in grams, is required to react with 12.4 L of CO2 at 22.0°C and 872 mm Hg? Mass= g
The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4240 L of hydrogen gas at STP, heat the mixture to run the reaction, then separate the ammonia from the reaction mixture. What volume of reactant, measured at STP, is left over? Assume the reaction goes to completion. N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)
Pp
Ammonia is not the only possible fertilizer. Others include urea, which can be produced by the reaction: CO: (g) + 2 NH3 (g) → cO(NH2)2 (s) + H,0(g) A scientist has 72 g of dry ice to provide the carbon dioxide. If 4.50 L of ammonia at 15°C and a pressure of 1.2 atm is added, which reactant is limiting? Limiting reactant: carbon dioxide What mass of urea ammonia Mass = bl)
Sulfur dioxide, a gas that plays a central role in the formation of acid rain is found in the exhaust of automobiles and power plants. Consider a 1.53 L sample of SO2 at a pressure of 5.6 * 103 Pa. If the pressure is changed to 1.5 * 104 Pa, at constant temperature, what will be the new volume of the gas?
The hydrogen gas evolved in a reaction between solid zinc and hydrochloric acid has been collected over water. The volume of water displaced is equal to 0.587 L. Given that the gas was collected at a temperature of 30.0°C and the atmospheric pressure was 738 torr, what mass (in mg) of hydrogen gas was collected? (3 sf) =
When copper metal is added to nitric acid, the following reaction takes place Cu (s) + 4 HNO3 (aq) → Cu(NO3)2 (aq) + 2 H,0 (I) + 2 NO2 (g) Calculate the volume in liters of NO2 gas collected over water at 25.0 °C when 4.71 g of copper is added to excess nitric acid if the total pressure is 726.0 mmHg. The vapor pressure of water at 25.0 °C is 23.8 mm Hg. | L