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Please, please explain the part I have circled in the pic--I don't understand why the mols of H2SO4 have to be multiplied by 2!

Please, please explain the part I have circled in the pic--I don't understand why the mols of H2SO4 have to be multiplied by 2!

Chemistry
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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Please, please explain the part I have circled in the pic--I don't understand why the mols of H2SO4 have to be multiplied by 2!

Ammonium sulphate, an important fertilizer, can be prepared by the reaction of ammonia with sulphuric acid according to: 2NH, + H,SO, → (NH,),SO, - Calculate the volume of NH3 needed at 42°C and 15:6 atm to react with 870 g of H2SO4. Solution · First, the temperature must be changed to K. T(K) = T(° C) + 273.15 = 42°C + 273.15 %3D %3D = 315.15 K Now, you must convert the given mass into moles. mol (H2SO4) = mass x MM[H2SO4] = 870 g/ 98.0784 g/mol = 887 mol %3D %3D Find the number of moles of NH3 that will reaction with the H,SO4. From the balanced equation, each mole of H,SO, requires 2 mol of NH So, 8.87 mol x 2 = 17.74 mol of NH3 is needed. Fnally use the ideal gas law to calculate the volume of ammonia that will react. PV = nRT nRT V = (17.74 mol)(0.08206 L•atm (315.15 K) K«mol 15.6 atm = 29.41L %3D Therefore, 29.41 L of are needed.
Transcribed Image Text:Ammonium sulphate, an important fertilizer, can be prepared by the reaction of ammonia with sulphuric acid according to: 2NH, + H,SO, → (NH,),SO, - Calculate the volume of NH3 needed at 42°C and 15:6 atm to react with 870 g of H2SO4. Solution · First, the temperature must be changed to K. T(K) = T(° C) + 273.15 = 42°C + 273.15 %3D %3D = 315.15 K Now, you must convert the given mass into moles. mol (H2SO4) = mass x MM[H2SO4] = 870 g/ 98.0784 g/mol = 887 mol %3D %3D Find the number of moles of NH3 that will reaction with the H,SO4. From the balanced equation, each mole of H,SO, requires 2 mol of NH So, 8.87 mol x 2 = 17.74 mol of NH3 is needed. Fnally use the ideal gas law to calculate the volume of ammonia that will react. PV = nRT nRT V = (17.74 mol)(0.08206 L•atm (315.15 K) K«mol 15.6 atm = 29.41L %3D Therefore, 29.41 L of are needed.
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