Answer:
a. Theoretical yield = 8.81 g
b. 77 %
Explanation:
We begin from the reaction:
2Fe (s) + 3Cl₂ (g) → 2FeCl₃ (s)
and the excess is the iron, so the limiting reagent is the chlorine.
We convert mass to moles → 5.78 g / 70.90 g/mol = 0.0815 mol
Ratio is 3:2 so we think this:
From 3 moles of chlorine, I can produce 2 moles of Iron (III) chloride
Then 0.0815 moles would produce (0.0815 . 2) /3 = 0.0543 moles
This is the theoretical yield. We convert the moles to mass:
0.0543 mol . 162.2 g /mol = 8.81 g
If the reaction yields 6.79 g of FeCl₃ and the theoretical yield is 8.81 g ,we can obtain the percent yield: (6.79 / 8.81) . 100 = 77 %
To calculate the molar mass of substance, divide the number of moles by the given mass of substance.
The quantity of a substance is known as a mole. You can measure it in terms of grams, liters, atoms, molecules, or particles.
Use the substance's molar mass to convert between grams and moles. Divide the given mass by the number of moles to convert from moles to molar mass.
Using the formula, Number of moles = Given mass/ molar mass
The molar mass of a substance can be calculated as-
Molar mass = Given mass/number of moles
Learn more about mole -
brainly.com/question/26416088
#SPJ4
Answer:
222.30 L
Explanation:
We'll begin by calculating the number of mole in 100 g of ammonia (NH₃). This can be obtained as follow:
Mass of NH₃ = 100 g
Molar mass of NH₃ = 14 + (3×1)
= 14 + 3
= 17 g/mol
Mole of NH₃ =?
Mole = mass /molar mass
Mole of NH₃ = 100 / 17
Mole of NH₃ = 5.88 moles
Next, we shall determine the number of mole of Hydrogen needed to produce 5.88 moles of NH₃. This can be obtained as follow:
N₂ + 3H₂ —> 2NH₃
From the balanced equation above,
3 moles of H₂ reacted to produce 2 moles NH₃.
Therefore, Xmol of H₂ is required to p 5.88 moles of NH₃ i.e
Xmol of H₂ = (3 × 5.88)/2
Xmol of H₂ = 8.82 moles
Finally, we shall determine the volume (in litre) of Hydrogen needed to produce 100 g (i.e 5.88 moles) of NH₃. This can be obtained as follow:
Pressure (P) = 95 KPa
Temperature (T) = 15 °C = 15 + 273 = 288 K
Number of mole of H₂ (n) = 8.82 moles
Gas constant (R) = 8.314 KPa.L/Kmol
Volume (V) =?
PV = nRT
95 × V = 8.82 × 8.314 × 288
95 × V = 21118.89024
Divide both side by 95
V = 21118.89024 / 95
V = 222.30 L
Thus the volume of Hydrogen needed for the reaction is 222.30 L
- Endothermic reaction means the reactant side takes heat from surrounding and get decomposed i.e ∆H=-ve
- If the equation is exothermic then it means the reactant is happy to decompose .But it's not as it's endothermic
Now
- HgO is Omitted from our solution option.
Hg is a atom so no bonds hence no bond strength occurs.
- O_2 is a molecule and so it's our answer .