The reaction for the industrial production of hydrogen cyanide is given below.
2CH4 + 2NH3 + 3O2 -->2HCN + 6H2O
What mass of NH3 is required for the synthesis of 1.5 x 105 kg of HCN if the reaction has a 97.5% yield?
Subjects
Sections | |||
---|---|---|---|
Metal Alloys | 7 mins | 0 completed | Learn |
Polyatomic Ions | 15 mins | 0 completed | Learn Summary |
Naming Covalent Compounds | 6 mins | 0 completed | Learn |
Naming Ionic Compounds | 36 mins | 0 completed | Learn |
Naming Acids | 14 mins | 0 completed | Learn |
Empirical Formula | 14 mins | 0 completed | Learn Summary |
Combustion Analysis | 13 mins | 0 completed | Learn |
Mass Percent Formula | 17 mins | 0 completed | Learn Summary |
Balancing Chemical Equations | 8 mins | 0 completed | Learn |
Functional Groups in Chemistry | 13 mins | 0 completed | Learn |
Stoichiometry | 61 mins | 0 completed | Learn Summary |
Additional Practice |
---|
Ionic and Covalent Bonds |
Molecular Models |
Limiting Reagent |
Percent Yield |
Additional Guides |
---|
Molecular Formula |
Balancing Chemical Equations Worksheet |
Theoretical Yield |
Limiting Reactant |
The reaction for the industrial production of hydrogen cyanide is given below.
2CH4 + 2NH3 + 3O2 -->2HCN + 6H2O
What mass of NH3 is required for the synthesis of 1.5 x 105 kg of HCN if the reaction has a 97.5% yield?
Enter your friends' email addresses to invite them:
Join thousands of students and gain free access to 46 hours of Chemistry videos that follow the topics your textbook covers.