Answer:
We can see that at the boiling point, both liquid and gas are in equilibrium with one another. This is true for any applied pressure and boiling point temperature combination. As a result, we see liquid-gas equilibrium for every temperature and pressure combination on the graph in Figure 13.6.
Answer:
26.3 mol O₂
Explanation:
Step 1: Write the balanced equation
4 FeCl₃ + 3 O₂ ⇒ 2 Fe₂O₃ + 6 Cl₂
Step 2: Establish the appropriate molar ratio
According to the balanced equation, the molar ratio of FeCl₃ to O₂ is 4:3.
Step 3: Calculate how many moles of O₂ are needed to react completely with 35.0 mol of FeCl₃
We will use the previously established molar ratio.
35.0 mol FeCl₃ × 3 mol O₂/4 mol FeCl₃ = 26.3 mol O₂
Answer: 51.45 grams of excess reagent is left after the completion of reaction.
Explanation: For the calculation of moles, we use the formula:
....(1)
Given mass = 92 grams
Molar mass = 28g/mol
Putting values in equation 1, we get:
- For
Given mass = 112 grams
Molar mass = 116g/mol
Putting values in equation 1, we get:
The reaction follows:
By Stoichiometry,
2 moles of reacts with 3 moles of silicon
So, 0.965 moles of reacts with = = 1.4475 moles of Silicon.
As, the moles of silicon is more than the required amount and is present in excess.
So, the excess reagent for the reaction is Silicon.
Moles of silicon remained after reaction = 3.285 - 1.4475 = 1.8375 moles
To calculate the amount of Silicon left in excess is calculated by using equation 1:
Amount of Silicon in excess will be 51.45 grams.
Answer:
It's a Lithium atom
Explanation:
You can count the red particles in the nucleus, they're the protons. This atom have 3 protons. The atom that have 3 protons is the Lithium atom
Answer:
I believe it's qualitative and continuous.
Explanation: