Answer Analysis question 1-5 thank you ❤️ Angel Teran - Learnunm lesnr - BingBb Upload Assignment: Activity 04A XBb OverviewÔ https://learn.unm.edu/bbcswebdav/pid-6606468-dt-content-rid-55991010_1/courses/55869.202110/moduexisting catalysts decomposing ammonia requires a temperature of 450 °C, but this new catalyst is said to be effective at atemperature of 100 °C!You plan to heat ammonia gas with the catalyst in a flask connected to a manometer and track the reaction by the change inpressure, which should increase as the temperature increases and as the reaction progresses and the number of moles of gasincreases via the balanced chemical equation:2 NH3 (g) N2 (g) +3 H2 (g)You make the following observations.Observations1. Vnask = 1.00L2. Patm = 630.5 mmHg3. TRoom = 23.2 °C4. Before heating h = 0.005. As you heat the flask, the mercury falls on the flask side of the manometer and rises on the open end.6. At 100.0 oC, the height difference in the flask is 65.5 cm.Analysis**convert all T-values to K for gas law calculations!1. Use the ideal gas equation to determine the number of moles of gas present before heating.2. Use stoichiometry and the result from Q1 to calculate how many total moles of gas (N2 and H2) should be producedassuming the reaction proceeds 100%.3. Use h and the atmospheric pressure to calculate in the flask to calculate the pressure inside the flask at 100 °C.4. Use the ideal gas equation and the result from Q3 to determine the number of moles of gas in the flask at 100 °C5. Compare the results from Q4 and Q2 to quantify how far the reaction progressed - is the catalyst 100% effective at thistemperature?SubmissionShow all calculations in order and include units. For Q5, write a paragraph.here to search

Given: Volume= 1.00 L Patm = 630.5 mmHg TRoom = 23.2oC Before heating h=0 At 100oC h = 65.5 cm

Answered: - Use the ideal gas equation to…

Science

Chemistry

- Use the ideal gas equation to determine the number of moles of gas present before heating.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.50PAE

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Question

Answer Analysis question 1-5 thank you ❤️

Angel Teran - Learn
unm lesnr - Bing
Bb Upload Assignment: Activity 04A X
Bb Overview
Ô https://learn.unm.edu/bbcswebdav/pid-6606468-dt-content-rid-55991010_1/courses/55869.202110/modu
existing catalysts decomposing ammonia requires a temperature of 450 °C, but this new catalyst is said to be effective at a
temperature of 100 °C!
You plan to heat ammonia gas with the catalyst in a flask connected to a manometer and track the reaction by the change in
pressure, which should increase as the temperature increases and as the reaction progresses and the number of moles of gas
increases via the balanced chemical equation:
2 NH3 (g) N2 (g) +3 H2 (g)
You make the following observations.
Observations
1. Vnask = 1.00L
2. Patm = 630.5 mmHg
3. TRoom = 23.2 °C
4. Before heating h = 0.00
5. As you heat the flask, the mercury falls on the flask side of the manometer and rises on the open end.
6. At 100.0 oC, the height difference in the flask is 65.5 cm.
Analysis
**convert all T-values to K for gas law calculations!
1. Use the ideal gas equation to determine the number of moles of gas present before heating.
2. Use stoichiometry and the result from Q1 to calculate how many total moles of gas (N2 and H2) should be produced
assuming the reaction proceeds 100%.
3. Use h and the atmospheric pressure to calculate in the flask to calculate the pressure inside the flask at 100 °C.
4. Use the ideal gas equation and the result from Q3 to determine the number of moles of gas in the flask at 100 °C
5. Compare the results from Q4 and Q2 to quantify how far the reaction progressed - is the catalyst 100% effective at this
temperature?
Submission
Show all calculations in order and include units. For Q5, write a paragraph.
here to search

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