1) Answer is: c) The reaction will proceed right.
Balanced chemical reaction: N₂(g) + 3H₂(g) ⇄ 2NH₃(g) ΔH = +92 kJ.
Reducing the volume of the system increase the partial pressures of the products and reactants.
With a pressure increase due to a decrease in volume, the side of the equilibrium with fewer moles is more favorable, there are 4 moles at the left side (three moles of hydrogen and one mole of nitrogen) and 2 moles (ammonia) at the right side of the reaction.
2) Answer is: d) The partial pressure of ammonia will increase.
This reaction is endothermic (enthalpy is higher than zero), which means that heat is added.
According to Le Chatelier's principle when the reaction is endothermic heat is included as a reactant and when the temperature increased, the heat of the system increase, so the system consume some of that heat by shifting the equilibrium to the right, producing more ammonia.
Answer:
37.5 L
Explanation:
Initial Volume, V1 = 15L
Initial Pressure P1 = 4.5 atm
Final Pressure, P2 = 1.8 atm
Final Volume V2 = ?
The relationship between these variables is given as;
P1V1 = P2V2
V2 = PIV1 / P1
Inserting the values;
V2 = 4.5 * 15 / 1.8
V2 = 37.5 L
Answer:
bc the cup system is a system that keeps everything cold
Explanation:
