Homework Help is Here – Start Your Trial Now!
Science
Chemistry
2 NH3(g) → N2(g) + 3 H2(g) the average rate of disappearance of NH3 over the time period from t = 0 s to t = 5.07x103 s is found to be 1.50x10-6 M/s. What is the average rate of appearance of H2 over the same time period? M/s. Submit Examine the balanced chemical eguation, Is the rate of formation of Ha faster than or slower than the rate of disappearance of NHa?

2 NH3(g) → N2(g) + 3 H2(g) the average rate of disappearance of NH3 over the time period from t = 0 s to t = 5.07x103 s is found to be 1.50x10-6 M/s. What is the average rate of appearance of H2 over the same time period? M/s. Submit Examine the balanced chemical eguation, Is the rate of formation of Ha faster than or slower than the rate of disappearance of NHa?

Chemistry
Chemistry
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question
100%

help me asap pls less than 30 mins with shortcuts only

TUTOR Relative Reaction Rates and Stoichiometry The average rate of appearance of a product is proportional to the rate of disappearance of a reactant. The proportionality constant is derived from the balanced chemical equation. For example, if 2 mol product is formed for each 1 mol reactant, the rate of product appearance will be twice the rate of reactant disappearance. Step 1. Use the balanced chemical equation to determine the relationship between the rates of reactant disappearance and product appearance. Step 2. Calculate the rate of product appearance using the rate of reactant disappearance and the proportion between the two rates. For the decomposition of ammonia on a platinum surface at 856 °C 2 NH3(g) → N2(g) + 3 H2(g) the average rate of disappearance of NH3 over the time period from t = 0 s to t = 5.07x103 s is found to be 1.50×10-6 M/s. What is the average rate of appearance of H2 over the same time period? M/s. Submit Examine the balanced chemical equation. Is the rate of formation of H2 faster than or slower than the rate of disappearance of NH3? O faster O slower Submit The average rate of appearance of H2 is 3/2 the rate of disappearance of NH3. What is the average rate of appearance of H2 from t = 0 to 5.07x103 s? Rate of disappearance of NH3 = 1.50×10-6 M/s. M H2/s
Transcribed Image Text:TUTOR Relative Reaction Rates and Stoichiometry The average rate of appearance of a product is proportional to the rate of disappearance of a reactant. The proportionality constant is derived from the balanced chemical equation. For example, if 2 mol product is formed for each 1 mol reactant, the rate of product appearance will be twice the rate of reactant disappearance. Step 1. Use the balanced chemical equation to determine the relationship between the rates of reactant disappearance and product appearance. Step 2. Calculate the rate of product appearance using the rate of reactant disappearance and the proportion between the two rates. For the decomposition of ammonia on a platinum surface at 856 °C 2 NH3(g) → N2(g) + 3 H2(g) the average rate of disappearance of NH3 over the time period from t = 0 s to t = 5.07x103 s is found to be 1.50×10-6 M/s. What is the average rate of appearance of H2 over the same time period? M/s. Submit Examine the balanced chemical equation. Is the rate of formation of H2 faster than or slower than the rate of disappearance of NH3? O faster O slower Submit The average rate of appearance of H2 is 3/2 the rate of disappearance of NH3. What is the average rate of appearance of H2 from t = 0 to 5.07x103 s? Rate of disappearance of NH3 = 1.50×10-6 M/s. M H2/s
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Reaction Rates
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS