Class 11 Exam > Class 11 Questions > 50 kg of N2(g) and 10 kg of H2(g) are mixed t...
Start Learning for Free
50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this?
Most Upvoted Answer
50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calcula...
No. of moles of N2 = 50/28 = 1.78
no. of moles of H2 = 10/2 = 5
because we know the formula to find the mole i.e.,
no.of moles = weight / molarmass
i.e., n = w/m
H2 is the limiting reagent because it have lesser amount....
no. of moles of H2 = 10/2 = 5
because we know the formula to find the mole i.e.,
no.of moles = weight / molarmass
i.e., n = w/m
H2 is the limiting reagent because it have lesser amount....
Community Answer
50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calcula...
Calculating moles of NH3(g) formed:
- Given:
- Mass of N2 = 50 kg
- Mass of H2 = 10 kg
- Molar mass of N2 = 28 g/mol
- Molar mass of H2 = 2 g/mol
- Molar mass of NH3 = 17 g/mol
Step 1: Calculate moles of N2 and H2:
- Moles of N2 = 50 kg / 28 g/mol = 1785.71 mol
- Moles of H2 = 10 kg / 2 g/mol = 500 mol
Step 2: Identify the limiting reagent:
- To determine the limiting reagent, we compare the moles of N2 and H2 with the stoichiometry of the reaction:
- N2 + 3H2 → 2NH3
- From the balanced equation, 1 mol of N2 reacts with 3 mol of H2 to produce 2 mol of NH3.
- Moles of H2 required to react with all N2 = 1785.71 mol N2 * (3 mol H2 / 1 mol N2) = 5357.14 mol H2
- Since we have only 500 mol of H2, it is the limiting reagent.
Step 3: Calculate moles of NH3 formed:
- Moles of NH3 formed = 500 mol H2 * (2 mol NH3 / 3 mol H2) = 333.33 mol NH3
Therefore, 333.33 moles of NH3(g) are formed. The limiting reagent in this reaction is H2 because it is completely consumed in the reaction before all the N2 can react.
- Given:
- Mass of N2 = 50 kg
- Mass of H2 = 10 kg
- Molar mass of N2 = 28 g/mol
- Molar mass of H2 = 2 g/mol
- Molar mass of NH3 = 17 g/mol
Step 1: Calculate moles of N2 and H2:
- Moles of N2 = 50 kg / 28 g/mol = 1785.71 mol
- Moles of H2 = 10 kg / 2 g/mol = 500 mol
Step 2: Identify the limiting reagent:
- To determine the limiting reagent, we compare the moles of N2 and H2 with the stoichiometry of the reaction:
- N2 + 3H2 → 2NH3
- From the balanced equation, 1 mol of N2 reacts with 3 mol of H2 to produce 2 mol of NH3.
- Moles of H2 required to react with all N2 = 1785.71 mol N2 * (3 mol H2 / 1 mol N2) = 5357.14 mol H2
- Since we have only 500 mol of H2, it is the limiting reagent.
Step 3: Calculate moles of NH3 formed:
- Moles of NH3 formed = 500 mol H2 * (2 mol NH3 / 3 mol H2) = 333.33 mol NH3
Therefore, 333.33 moles of NH3(g) are formed. The limiting reagent in this reaction is H2 because it is completely consumed in the reaction before all the N2 can react.
Attention Class 11 Students!
To make sure you are not studying endlessly, EduRev has designed Class 11 study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in Class 11.
|
Explore Courses for Class 11 exam
|
|
Similar Class 11 Doubts
Top Courses for Class 11View all
50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this?
Question Description
50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about 50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this?.
50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about 50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this?.
Solutions for 50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this? in English & in Hindi are available as part of our courses for Class 11.
Download more important topics, notes, lectures and mock test series for Class 11 Exam by signing up for free.
Here you can find the meaning of 50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this? defined & explained in the simplest way possible. Besides giving the explanation of
50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this?, a detailed solution for 50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this? has been provided alongside types of 50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this? theory, EduRev gives you an
ample number of questions to practice 50 kg of N2(g) and 10 kg of H2(g) are mixed to produce NH3(g). Calculate the moles of NH3(g) formed.identify the limiting reagent in this? tests, examples and also practice Class 11 tests.
|
|
Explore Courses for Class 11 exam
|
|
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
Follow Us
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup