The answer is d: Combustion, because it is the so-called combustion of methan. (Check your lesson)
Probably very negative or sightless negative
Answer:
168.4 mL
Explanation:
Data Given
initial volume V1 of gas in balloon = 100 mL
initial pressure P1 of gas in balloon = 3.2 atm
final pressure P2 of gas in balloon = 1.9 atm
final volume V2 of gas in balloon = ?
Solution:
This problem will be solved by using Boyle's law equation at constant Temperature.
The formula used
P1V1 = P2V2
As we have to find out Volume, so rearrange the above equation
V2 = P1V1 / P2
Put value from the data given
V2 = 100 mL x 3.2 atm / 1.9 atm
V2 = 168.4 mL
So the final Volume of gas in baloon = 168.4 mL
Hello! Your question seems incomplete, still I will try to answer it in a general way. As shown in in equation 22 KJ heat is absorbed during the reaction so it is endothermic reaction.
Effect of Temperature:
According to Le Chatelier's principle, by increasing temperature the equilibrium will shift in the forward direction hence more nitrogen and hydrogen will produce.
Effect of Pressure:
It is evident from the reaction that there is an increase in volume in the formation of N2 and H2 (4 moles in whole), Hence, decrease in pressure on this system in equilibrium state will adjust itself in a direction in which the volume is increased i.e. formation of N2 and H2.
Effect of Concentration:
Increasing concentration of NH3, removal of N2 or removal of H2 will shift the equilibrium in forward direction, Hence more product is formed.
