Answer:
- <u><em>The leftover reactant is the nitrogen gas, N₂.</em></u>
Explanation:
As per your description:
<u>1. Square on the left: N₂(g)</u>
- 3 units of two joint circles: this represents 3 molecules of nitrogen gas, N₂(g).
<u>2. Square on the right: H₂(g)</u>
- 3 units of two joint circles: this represents 3 molecules of hydrogen gas, H₂(g).
<u>3. Reaction</u>
If the maximum possible amount of NH₃ is formed during the reaction, you assume that the reaction goes to completion.
The chemical equation that represents the reaction is:
Which must be balanced:
That means that 1 molecule (or 1 mol) of N₂(g) reacts with 3 molecules (or 3 moles ) of H₂(g) to produce 2 molecules (or 2 moles) of NH₃(g).
Since, the squares show that there are 3 molecules of each reactant, the 3 molecules of hydrogen gas will be able to react with 1 molecule of nitrogen gas. When that happens, all the hydrogen gas is consumend and yet two molecules of nitrogen gas will remain unreacted. Hence, the nitrogen gas is the leftover reactant.
Answer:
O FX will be greater than FY
Explanation:
<em>Surface tension</em> can be defined as the force required to stretch one film of a given fase (usually with liquids).
This required force is proportional to the liquid's surface tension. This means that the higher the surface tension, the higher the required force to stretch it is.
Answer:
- 7.48
Explanation:
Given:
Concentration of the sugar solution, C = 0.3 M
Temperature, T = 27° C = 273 + 27 = 300 K
Now,
The solute potential is given as:
solute potential = - iCRT
where,
i is the number of particles the particular molecule will make in water
i = 1 for sugar
R is the universal gas constant = 0.0831 liter bar/mole-K
on substituting the respective values, we get
solute potential = - 1 × 0.3 × 0.0831 × 300
or
The solute potential = - 7.479 ≈ - 7.48
1) Balanced chemical reaction:
2H2 + O2 -> 2H20
Sotoichiometry: 2 moles H2: 1 mol O2 : 2 moles H2O
2) Reactant quantities converted to moles
H2: 5.00 g / 2 g/mol = 2.5 mol
O2: 50.0 g / 32 g/mol = 1.5625 mol
Limitant reactant: H2 (because as per the stoichiometry it will be consumed with 1.25 mol of O2).
3) Products
H2 totally consumed -> 0 mol at the end
O2 = 1.25 mol consumed -> 1.5625 mol - 1.25 mol = 0.3125 mol at the end
H2O: 2.5 mol H2 produces 2.5 mol H2O -> 2.5 mol at the end.
Total number of moles: 0.3125mol + 2.5 mol = 2.8125 mol
4) Pressure
Use pV = nRT
n = 2.8125
V= 9 liters
R = 0.082 atm*lit/K*mol
T = 35 C + 273.15 = 308.15K
p = nRT/V = 7.9 atm
Those are the correct steps, young chemist. Don't be discouraged by an insane answer.
