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boyakko [2]
3 years ago
14

Which equation obeys the law of conservation of mass?

Chemistry
2 answers:
DanielleElmas [232]3 years ago
9 0

4Fe + 3O2 → 2Fe2O3

i believe this is the answer

Jlenok [28]3 years ago
8 0

Answer:- 4Fe+3O_2\rightarrow 2Fe_2O_3

Explanations:- A balanced equation obeys the law of conservation of mass.

First equation is not balanced as it has two Fe on left side and four Fe on right side.

Second equation is not balanced as it has two O on left side and six O on right side.

Third equation is not balanced as it has one Fe on left side and two fe on right side.

Fourth equation is balanced as it has four Fe and six O on both sides. So, it obeys the law of conservation of mass.

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If 75 g of liquid water in a calorimeter changes temperature from 25 degrees C to 75 degrees C how much heat was transferred
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An atom that has 13 protons and 15 neutrons is isotope of the element A.) nickel B.) silicon C.) aluminum D.) phosphorus. Why?
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An atom that has 13  protons and 15  neutrons  is isotope  of Aluminium (answer C)

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Enter your answer in the provided box. When mixed, solutions of barium chloride, BaCl2, and potassium chromate, K2CrO4, form a y
ira [324]

Answer:

35.42g

Explanation:

Step 1:

The balanced equation for the reaction

BaCl2(aq) + K2CrO4(aq) → BaCrO4(s) + 2KCl(aq)

Step 2:

Determination of the limiting reactant.

It is important to determine which of the reactant is limiting the reaction as the limiting reactant is used to determine the maximum yield of the reaction. The limiting reactant can be determined as follow:

From the balanced equation above,

1 mole of BaCl2 reacted with 1 mole of K2CrO4.

Therefore, 0.7 mole of BaCl2 will also react with 0.7 mol of K2CrO4.

From the above illustration, we can see that it requires a higher amount of K2CrO4 to react with 0.7 mol of BaCl2. This simply means that K2CrO4 is the limiting reactant.

Step 3:

Determination of the number of mole of BaCrO4 produced from the reaction.

The limiting reactant is used in this case.

From the balanced equation above,

1 mole of K2CrO4 produced 1 mole of BaCrO4.

Therefore, 0.14 mole of K2CrO4 will also produce 0.14 mole of BaCrO4.

Step 4:

Converting 0.14 mole of BaCrO4 to grams.

This is illustrated below:

Molar Mass of BaCrO4 = 137 + 52 + (16x4) = 137 + 52 + 64 = 253g/mol

Number of mole BaCrO4 = 0.14 mole

Mass of BaCrO4 =?

Mass = number of mole x molar Mass

Mass of BaCrO4 = 0.14 x 253

Mass of BaCrO4 = 35.42g

Therefore, 35.42g of BaCrO4 is produced from the reaction.

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