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Calculate the mass of ammonia (NH3) produced when 3.5 g of nitrogen (N2) react with 2.5 g hydrogen (H2). What is the excess and limiting reactant and how much of it will be left over when the reaction is complete. Given the balanced chemical equation. N2 (g)+ 3H2ig) - 2NH3 (9) H 14.00 1.00 1. What is the Mass of Ammonia: grams NH3 2. What is the Limiting reactant: ONITROGEN OHYDROGEN 3. What is the Excess reactant: OHYDROGEN ONITROGEN 4. How much is in excess: grams

Calculate the mass of ammonia (NH3) produced when 3.5 g of nitrogen (N2) react with 2.5 g hydrogen (H2). What is the excess and limiting reactant and how much of it will be left over when the reaction is complete. Given the balanced chemical equation. N2 (g)+ 3H2ig) - 2NH3 (9) H 14.00 1.00 1. What is the Mass of Ammonia: grams NH3 2. What is the Limiting reactant: ONITROGEN OHYDROGEN 3. What is the Excess reactant: OHYDROGEN ONITROGEN 4. How much is in excess: grams

Chemistry
Chemistry
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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
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Calculate the mass of ammonia (NH3) produced when 3.5 g of nitrogen (N2) react with 2.5 g hydrogen (H2). What is the excess and limiting reactant and how much of it will be left over when the reaction is complete. Given the balanced chemical equation. N2 (g)+ 3H2ig) – 2NH3 (g) H 14.00 1.00 1. What is the Mass of Ammonia: grams NH3 2. What is the Limiting reactant: ONITROGEN OHYDROGEN 3. What is the Excess reactant: OHYDROGEN ONITROGEN 4. How much is in excess: grams
Transcribed Image Text:Calculate the mass of ammonia (NH3) produced when 3.5 g of nitrogen (N2) react with 2.5 g hydrogen (H2). What is the excess and limiting reactant and how much of it will be left over when the reaction is complete. Given the balanced chemical equation. N2 (g)+ 3H2ig) – 2NH3 (g) H 14.00 1.00 1. What is the Mass of Ammonia: grams NH3 2. What is the Limiting reactant: ONITROGEN OHYDROGEN 3. What is the Excess reactant: OHYDROGEN ONITROGEN 4. How much is in excess: grams
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