-
Engineering and Architecture
Exams
Colleges
Predictors
Resources
-
Computer Application and IT
Quick Links
Colleges
-
Pharmacy
Colleges
Resources
-
Hospitality and Tourism
Colleges
Resources
Diploma Colleges
-
Competition
Other Exams
Resources
-
School
Exams
Top Schools
Products & Resources
-
Study Abroad
Top Countries
Resources
-
Arts, Commerce & Sciences
Exams
Colleges
Upcoming Events
Resources
-
Management and Business Administration
Colleges & Courses
Predictors
-
Learn
Law Preparation
MBA Preparation
Engineering Preparation
Medical Preparation
-
Online Courses and Certifications
Top Streams
Specializations
- Digital Marketing Certification Courses
- Cyber Security Certification Courses
- Artificial Intelligence Certification Courses
- Business Analytics Certification Courses
- Data Science Certification Courses
- Cloud Computing Certification Courses
- Machine Learning Certification Courses
- View All Certification Courses
Resources
-
Medicine and Allied Sciences
Colleges
Predictors
Resources
-
Law
Resources
Colleges
-
Animation and Design
Exams
Predictors & Articles
Colleges
Resources
-
Media, Mass Communication and Journalism
Colleges
Resources
-
Finance & Accounts
Top Courses & Careers
Colleges
Get Answers to all your Questions
- Home
- Engineering
- A gaseous compound of nitrogen and hydrogen contains 12.5%(by mass) of hydrogen. The density of the compound relative to hydrogen is 16. The molecular formula of the compound is :  
- #Chemistry
- #Class 11
- #National Eligilibility Cum Entrance Test
- #Some basic concepts in chemistry
- #Engineering
- #Joint Entrance Examination Main
A gaseous compound of nitrogen and hydrogen contains 12.5%(by mass) of hydrogen. The density of the compound relative to hydrogen is 16. The molecular formula of the compound is :
Answers (1)
In the given compound, let the total weighht of the compound is 100 g.
Therefore, the weight of hydrogen = 12.5 g and weight of nitrogen = 87.5 g.
Now, moles of hydrogen = 12.5 /1 = 12.5 moles
moles of nitrogen = 87.5 / 14 = 6.25 moles
Now the atomic ratio of hydrogen to nitrogen = 12.5 / 6.25
= 2:1
According to question, vapour density of the compound = 16
Therefore, molecular weight = 2 x vapour density
= 32g
Now, from the atomic ratio, we can say that the empirical formula of the compound is NH2.
Thus, the molecular formula of the compound = n x empirical formula
Now, molecular mass = 32g and empirical mass = 16g
Thus, the molecular formula of the compound = 2 x NH2
= N2H4
Therefore, Option (4) is correct
JEE Main high-scoring chapters and topics
Study 40% syllabus and score up to 100% marks in JEE
