Answer: 0.771 g of will be produced
Explanation:
To calculate the moles :
The balanced chemical reaction is:
According to stoichiometry :
2 moles of produce = 3 moles of
Thus 0.257 moles of will produce=
of
Mass of
Thus 0.771 g of will be produced
Answer:
Explanation:
Given that:
The chemical equation for the reaction is:
Br2(g) ⇌ 2Br(g)
Initially 0.0345M 0.0416M
Thus, the given reaction will proceed in the backward direction
The I.C.E table is as follows:
Br2(g) ⇌ 2Br(g)
I 0.0345 0.0416
C +x -2x
E (0.0345+x) (0.0416 -2x)
= 0.00173056 - 0.0832x - 0.0832x + 4x² = 0.00584 (0.0345 +x)
= 0.00173056 - 0.166x + 4x² = 2.0148× 10⁻⁴ + 0.00584x
= 0.00173056 - 2.0148× 10⁻⁴ - 0.166x - 0.00584x + 4x²
= 0.00152908 - 0.17184x + 4x²
Solving by using Quadratic formula
x = 0.03038 or 0.0126
For x = 0.03038
At equilibrium
[Br₂] = (0.0345 + 0.03038) = 0.06488 M
[Br] = (0.0416 -2(0.03038)) = - 0.01916 M
Since we have a negative value for [Br], we discard the value for x
For x = 0.0126
At equilibrium
[Br₂] = (0.0345 + 0.0126) = 0.0471 M
[Br] = (0.0416 -2(0.0126)) = 0.0164 M
5.00 mol O₂
<h3>General Formulas and Concepts:</h3><u>Math</u>
<u>Pre-Algebra</u>
Order of Operations: BPEMDAS
<u>Chemistry</u>
<u>Atomic Structure</u>
<u>Stoichiometry</u>
<u>Step 1: Define</u>
3.01 × 10²⁴ atoms O₂
<u>Step 2: Identify Conversions</u>
Avogadro's Number
<u>Step 3: Convert</u>
<u>Step 4: Check</u>
<em>Follow sig fig rules and round. We are given 3 sig figs.</em>
4.99834 mol O₂ ≈ 5.00 mol O₂