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andrezito [222]
3 years ago
6

Potassium chloride and oxygen gas are formed upon heating potassium

Chemistry
1 answer:
sattari [20]3 years ago
3 0

Answer:

4 mol KClO3

Explanation:

6 mol O2 (2 mol KClO/3 mol O2) =4 mol KClO3

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Beaker A contains 100.0 g of water initially at 10EC. Beaker B contains 100.0 g of water initially at 20°C. The contents of the
Korvikt [17]

Answer:

(A) 15.0 °C

Explanation:

The water in beaker A gains heat because its initial temperature (10 °C) is less than the initial temperature of the water in beaker B (20 °C) which loses heat.

Let T3 be the final temperature

Heat gained by beaker A = heat loss by beaker B

mc(T3 - T1) = mc(T2 - T3)

The mass and specific heat of water in both beakers are the same. Therefore, (T3 - T1) = (T2 - T3)

T1 is initial temperature of beaker A = 10 °C

T2 is initial temperature of beaker B = 20 °C

T3 - 10 = 20 - T3

T3 + T3 = 20 + 10

2T3 = 30

T3 = 30/2 = 15 °C

7 0
3 years ago
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Match the mixture with its description.
Fiesta28 [93]

Solution – A. 

Emulsions – B.

Colloid – C.

Homogenous – D.

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3 years ago
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Why is it important for us to study outer space?
AleksAgata [21]

Answer:

So you know the things about outer space like facts that you might not know

8 0
3 years ago
Lead will float in water.
Fed [463]

Actually, no. While their mass may be the same (1kg), the volume of lead is a lot smaller than that of feathers. As there is the same mass stuffed in a smaller space, it must be denser. The density of water is 1 g/cm3, so if the density of the lead is more than 1g/cm3, it has to sink

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3 years ago
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If 12.5 grams of strontium hydroxide is reacted with 150 mL of 3.5 M carbonic acid, identify the limiting reactant.
vesna_86 [32]

Answer:

Sr(OH)2

Explanation:

We'll begin by calculating the number of mole of carbonic acid in 150mL of 3.5 M carbonic acid solution. This is illustrated below:

Molarity = 3.5M

Volume = 150mL = 150/1000 = 0.15L

Mole of carbonic acid, H2CO3 =..?

Mole = Molarity x Volume

Mole of carbonic acid, H2CO3 = 3.5 x 0.15 = 0.525 mole.

Next, we shall convert 0.525 mole of carbonic acid, H2CO3 to grams.

Mole of H2CO3 = 0.525 mole

Molar mass of H2CO3 = (2x1) + 12 + (16x3) = 62g/mol.

Mass of H2CO3 =..?

Mass = mole x molar mass

Mass of H2CO3 = 0.525 x 62 = 32.55g

Next, we shall write the balanced equation for the reaction. This is given below:

Sr(OH)2 + H2CO3 → SrCO3 + 2H2O

Next, we shall determine the mass of Sr(OH)2 and H2CO3 that reacted from the balanced equation. This is illustrated below:

Molar mass of Sr(OH)2 = 88 + 2(16 + 1) = 88 + 2(17) = 122g/mol

Mass of Sr(OH)2 from the balanced equation = 1 x 122 = 122g

Molar mass of H2CO3 = (2x1) + 12 + (16x3) = 62g/mol.

Mass of H2CO3 from the balanced equation = 1 x 62 = 62g.

From the balanced equation above, 122g of Sr(OH)2 reacted with 62g of H2CO3.

Finally, we shall determine the limiting reactant as follow:

From the balanced equation above, 122g of Sr(OH)2 reacted with 62g of H2CO3.

Therefore, 12.5g of Sr(OH)2 will react with = (12.5 x 62)/122 = 6.35g.

We can see evidently from the calculations made above that it will take 6.35g out 32.55g of H2CO3 to react with 12.5g of Sr(OH)2. Therefore, Sr(OH)2 is the limiting reactant and H2CO3 is the excess reactant

5 0
3 years ago
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