Professor Ndekele asks you to test a new low temperature catalyst for the decomposition of ammonia, NH3. With previously existing catalysts decomposing ammonia requires a temperature of 450 ºC, but this new catalyst is said to be effective at a temperature of 100 ºC!
Professor Ndekele asks you to test a new low temperature catalyst for the decomposition of ammonia, NH3. With previously existing catalysts decomposing ammonia requires a temperature of 450 ºC, but this new catalyst is said to be effective at a temperature of 100 ºC!
Professor Ndekele asks you to test a new low temperature catalyst for the decomposition of ammonia, NH3. With previously existing catalysts decomposing ammonia requires a temperature of 450 ºC, but this new catalyst is said to be effective at a temperature of 100 ºC!
Professor Ndekele asks you to test a new low temperature catalyst for the decomposition of ammonia, NH3. With previously existing catalysts decomposing ammonia requires a temperature of 450 ºC, but this new catalyst is said to be effective at a temperature of 100 ºC!
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
Vflask = 1.00 L
Patm = 630.5 mmHg
TRoom = 23.2 ºC
Before heating h = 0.00
As you heat the flask, the mercury falls on the flask side of the manometer and rises on the open end.
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!
Use the ideal gas equation to determine the number of moles of gas present before heating.
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%.
Use h and the atmospheric pressure to calculate in the flask to calculate the pressure inside the flask at 100 ºC.
Use the ideal gas equation and the result from Q3 to determine the number of moles of gas in the flask at 100 ºC
Compare the results from Q4 and Q2 to quantify how far the reaction progressed - is the catalyst 100% effective at this temperature?
Definition Definition Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
