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professor190 [17]
3 years ago
5

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Br2 and OH- in the ba

lanced reaction?
Br2(l) → BrO3-(aq) + Br(aq)
Possible answers:
Br2 = 3, OH- = 3
Br2 = 2, OH- = 5
Br2 = 3, OH- = 6
Br2 = 1, OH- = 6
Br2 = 1, OH- = 2
Chemistry
1 answer:
Nataly [62]3 years ago
4 0

Answer:

Br2(l) → BrO3-(aq) + Br-(aq)

A) Br2 = 3, OH - = 6

B) Br2 = 3, OH - = 3

C) Br2 = 2, OH - = 5

D) Br2 = 1, OH - = 2

E) Br2 = 1, OH - = 6

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Answer:

q = 14049 J

Explanation:

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q = 350 * 0.892 * (70-25) =

312.2 * 45 = 14049 J

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3 years ago
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3 years ago
Calculate the molarity of each of the following
Alenkasestr [34]

Answer:

a. 1.21M

b. 0.119M

c. 0.00496M

Explanation:

Molarity, M, is an unit of concentration defined as the ratio between moles of solute and liters of solution:

a. 4.35 mol LiCl / 3.60L = 1.21M

b. 29.43gC6H12O6 * (1mol / 180.16g) = 0.1634moles / 1.37L = 0.119M

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8 0
3 years ago
What is the limiting reactant for the following balanced equation when 9 moles of AlF3 are mixed with 12 miles of O2?
tamaranim1 [39]
<h2>Answer:AlF_{3} </h2>

Explanation:

The chemical equation of the reaction that occurs when AlF_{3} reacts with O_{2} is

4AlF_{3}+3O_{2}→2Al_{2}O_{3}+6F_{2}

4 moles of AlF_{3} requires 3 moles of O_{2}.

1 mole of AlF_{3} requires \frac{3}{4} moles of O_{2}.

Given that we have 9 moles of AlF_{3}.

9 moles of AlF_{3} requires \frac{3}{4}\times 9=6.75 moles of O_{2}.

But we have 12 moles of O_{2}.

So,AlF_{3}  will be consumed first.

So,AlF_{3}  is the limiting reagent.

3 0
3 years ago
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