1. Ammonium carbamate, NH CONH,. reversibly decomposes into CO2 and NH3 as shown
ID: 1031020 • Letter: 1
Question
1. Ammonium carbamate, NH CONH,. reversibly decomposes into CO2 and NH3 as shown by the balanced equation below: NHCO2NH2(s) = 2NH3(g) + CO2(g) K, = ? A student places 0.50 g of solid NH, CONH, in a previously evacuated, rigid 0.750 L container that is held at a constant temperature of 298 K. The student monitors the total pressure in the container as a function of time and obtains the graph shown below: Pressure (tor) 100 i 150 150 Time (s) (a) Based on the information in the graph and the reaction above, determine: i. The final partial pressure of NH3 (g) in the 0.750 L container. ii. The value of K, for the decomposition of NHA CO2NH2. iii. The mass of solid NH4CO2NH2 (rnolar mass 78.09 g/mol) that decomposed. The student is asked to perform the experiment a second time with one of the following changes to the experimental conditions: • Perform the experiment at a higher temperature of 325 K. • Perform the experiment with 1.00 g of solid NH4CO2NH2. • Perform the experiment in a 1.00 L container. • Perform the experiment in a 0.500 L container. (b) Which of the changes to the experimental conditions listed above will result in a greater mass of NH,CO2NH2 decomposing than was calculated in part (a) iii? Justify your answer.Explanation / Answer
1. As this is an decomposition reaction increasing temp will move reaction forward.
2. Increasing conc of reactant will also result in more decomposition.
3. Increasing volumn moves reaction towards more no og mole side. Hence more decomposition.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.