Homework Help is Here – Start Your Trial Now!
Engineering
Chemical Engineering
3H2(g)+N2rg)t)2NH3rg) +Heat -what is the Keqif the coscentratiors atequilibr'um are (Hz]=01 Mi [Nz]= 0.250 M and CNH3]=1.5om? PHow many gramsofnitrogen gas are needecd to produce 5OL of ammonia at STP?チら1

3H2(g)+N2rg)t)2NH3rg) +Heat -what is the Keqif the coscentratiors atequilibr'um are (Hz]=01 Mi [Nz]= 0.250 M and CNH3]=1.5om? PHow many gramsofnitrogen gas are needecd to produce 5OL of ammonia at STP?チら1

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
See similar textbooks
icon
Related questions
Question
--- ### Chemical Equilibrium and Reaction Stoichiometry #### Problem 1: Consider the reaction: \[ \text{3H}_2\text{(g)} + \text{N}_2\text{(g)} \rightleftharpoons \text{2NH}_3\text{(g)} + \text{heat} \] **Question:** What is the equilibrium constant \( K_c \) if the concentrations at equilibrium are \([H_2] = 1.00 \, M\), \([N_2] = 0.250 \, M\) and \([NH_3] = 1.50 \, M\)? --- #### Solution: To find the equilibrium constant \( K_c \), we use the expression: \[ K_c = \frac{[\text{products}]}{[\text{reactants}]} \] For the given reaction: \[ K_c = \frac{[\text{NH}_3]^2}{[\text{H}_2]^3 [\text{N}_2]} \] Substituting the given concentrations: \[ K_c = \frac{(1.50 \, M)^2}{(1.00 \, M)^3 \cdot (0.250 \, M)} \] Doing the math: \[ K_c = \frac{2.25}{1 \cdot 0.25} \] \[ K_c = \frac{2.25}{0.25} \] \[ K_c = 9 \] Thus, the equilibrium constant \( K_c \) is 9. --- #### Problem 2: **Question:** How many grams of nitrogen gas (\( \text{N}_2 \)) are needed to produce 5.0 L of ammonia (\( \text{NH}_3 \)) at STP (Standard Temperature and Pressure)? --- #### Solution: At STP, 1 mole of any gas occupies 22.4 liters. First, we find the moles of ammonia produced: \[ \text{moles of NH}_3 = \frac{5.0 \, L}{22.4 \, L/mol} \] \[ \text{moles of NH}_3 = 0.223 \, mol \] From the balanced equation, 1 mole of \( \text{N}_2 \) produces 2 moles of \( \
Transcribed Image Text:--- ### Chemical Equilibrium and Reaction Stoichiometry #### Problem 1: Consider the reaction: \[ \text{3H}_2\text{(g)} + \text{N}_2\text{(g)} \rightleftharpoons \text{2NH}_3\text{(g)} + \text{heat} \] **Question:** What is the equilibrium constant \( K_c \) if the concentrations at equilibrium are \([H_2] = 1.00 \, M\), \([N_2] = 0.250 \, M\) and \([NH_3] = 1.50 \, M\)? --- #### Solution: To find the equilibrium constant \( K_c \), we use the expression: \[ K_c = \frac{[\text{products}]}{[\text{reactants}]} \] For the given reaction: \[ K_c = \frac{[\text{NH}_3]^2}{[\text{H}_2]^3 [\text{N}_2]} \] Substituting the given concentrations: \[ K_c = \frac{(1.50 \, M)^2}{(1.00 \, M)^3 \cdot (0.250 \, M)} \] Doing the math: \[ K_c = \frac{2.25}{1 \cdot 0.25} \] \[ K_c = \frac{2.25}{0.25} \] \[ K_c = 9 \] Thus, the equilibrium constant \( K_c \) is 9. --- #### Problem 2: **Question:** How many grams of nitrogen gas (\( \text{N}_2 \)) are needed to produce 5.0 L of ammonia (\( \text{NH}_3 \)) at STP (Standard Temperature and Pressure)? --- #### Solution: At STP, 1 mole of any gas occupies 22.4 liters. First, we find the moles of ammonia produced: \[ \text{moles of NH}_3 = \frac{5.0 \, L}{22.4 \, L/mol} \] \[ \text{moles of NH}_3 = 0.223 \, mol \] From the balanced equation, 1 mole of \( \text{N}_2 \) produces 2 moles of \( \
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Distillation
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemical-engineering and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Introduction to Chemical Engineering Thermodynami…
Introduction to Chemical Engineering Thermodynami…
Chemical Engineering
ISBN:
9781259696527
Author:
J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:
McGraw-Hill Education
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemical Engineering
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
Elements of Chemical Reaction Engineering (5th Ed…
Elements of Chemical Reaction Engineering (5th Ed…
Chemical Engineering
ISBN:
9780133887518
Author:
H. Scott Fogler
Publisher:
Prentice Hall
Process Dynamics and Control, 4e
Process Dynamics and Control, 4e
Chemical Engineering
ISBN:
9781119285915
Author:
Seborg
Publisher:
WILEY
Industrial Plastics: Theory and Applications
Industrial Plastics: Theory and Applications
Chemical Engineering
ISBN:
9781285061238
Author:
Lokensgard, Erik
Publisher:
Delmar Cengage Learning
Unit Operations of Chemical Engineering
Unit Operations of Chemical Engineering
Chemical Engineering
ISBN:
9780072848236
Author:
Warren McCabe, Julian C. Smith, Peter Harriott
Publisher:
McGraw-Hill Companies, The
SEE MORE TEXTBOOKS