Ammonium carbamate will decompose into ammonia and carbon dioxide gasas. A 780.7 g sample of ammonium carbamate was allowed to decompose at a certain elevated temperature on a 10.0 L sealed container. A 25.0 mL sample of the headspace gas (i.e. the gas above the solid) was removed, and 0.0545 g ammonia could be isolated from that sample. NH4(NH2CO2)(s) = 2NH3(g) + CO2(g). (a) what cncenteration of ammonia, in mol/L was present in the headspace gas? (b) How many moles of ammonium carbamate had evaporated? Assume that the container volume is in addition to the volume of the solid (0.57 L) and that you may neglect the change in the volume occupied by the solid due to decomposition. (c) Calculate Kc for the decomposition of ammonium carbamate under these conditions.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Ammonium carbamate will decompose into ammonia and carbon dioxide gasas. A 780.7 g sample of ammonium carbamate was allowed to decompose at a certain elevated temperature on a 10.0 L sealed container. A 25.0 mL sample of the headspace gas (i.e. the gas above the solid) was removed, and 0.0545 g ammonia could be isolated from that sample. NH4(NH2CO2)(s) = 2NH3(g) + CO2(g). (a) what cncenteration of ammonia, in mol/L was present in the headspace gas? (b) How many moles of ammonium carbamate had evaporated? Assume that the container volume is in addition to the volume of the solid (0.57 L) and that you may neglect the change in the volume occupied by the solid due to decomposition. (c) Calculate Kc for the decomposition of ammonium carbamate under these conditions.
Answer:
Decomposition reaction of Ammonium Carbamate is given and we have to find out the number of moles of Ammonia and its concentration produced due to decomposition of Ammonium Carbamate.
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