3). 150°C and 100 kPa
Gases behave ideally at high temperatures and low pressures (less intermolecular forces)
Answer:
0.440 moles of NH₃ are produced
Explanation:
First of all, we need to determine the limiting reactant by the stoichiometry.
Equation reaction is: N₂(g) + 3H₂(g) ⟶ 2 NH₃(g)
1 mol of nitrogen needs 3 moles of hydrogen to react
Therefore 0.220 moles of N₂ will need (0.220 . 3) / 1 = 0.660 moles of H₂
As we have 0.717 moles of H₂ and we need 0.660, the hydrogen is the excess reagent, therefore, the N₂ is the limiting reactant
3 moles of H₂ need 1 mol of N₂ to react
Then, 0.717 moles of H₂ will react with (0.717 . 1) / 3 = 0.239 moles of N₂
We do not have enough N₂
After complete reaction → ratio is 1:2
1 mol of N₂ reacts to produce 2 moles of ammonia
Therefore 0.220 moles of N₂ will produce (0.220 . 2) / 1 = 0.440 moles of NH₃
Answer:
9x+y+8
Explanation:
We know this because you add 3x and 6x to get 9x
then we only have one y so put y by itself then subtract 15 and y which gets us 8
Answer:
See explanation
Explanation:
According to the law of conservation of energy; energy is neither created nor destroyed but is converted from one form to another.
This means that energy can not be lost, we can trace the transfer of energy between a system and its surroundings.
When a pot of water at 25°C is placed over a flame until it has boiled away, energy is transferred from the pot (the system) to the surroundings hence the temperature of the surroundings rises accordingly.
