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2 years ago

How many moles of KCl will be produced from 15.0 g of KClO3?

Chemistry

2 answers:

slega [8]2 years ago

7 0

Answer:

0.12 mol KCl

Explanation:

2 KClO3 (s) 2 KCl (s) + 3 O2 (g)

15 g x mol

x g KCl = 15 g KClO3 x[ (1 mol KClO3)/ (122.5 g KClO3) ] x [(2 mol KCl)/ (2 mol KClO3)]

x g KCl = 0.12 mol KCl

MAXImum [283]2 years ago

7 0

Answer:

0.1224 moles

Explanation:

this is a decompostion reaction

Equation of reaction

2KClO₃ → 2KCl + 3O₂

molar mass of KClO₃ =

molar mass of K = 39.09g/mol

Molar mass of Cl = 35.5g/mol

Molar mass of O = 15.99g/mol

Molar mass of KClO3 = [39 + 35.5 + (3*15.99)]

Molar mass of KClO3 = 122.47g/mol

From the equation of reaction,

2 moles of KClO₃ produces 2 moles of KClO₃

But 1 mole = molar mass

1 mole of KClO₃= 122.47g

2 moles of KClO₃ = 2 * 122.47 = 244.94g

If 244.94g of KClO₃ produces 2 moles of KCl

15 g of KClO₃ will produce x mole of KCl

x = (15 * 2) / 244.94

x = 0.1224moles

15g of KClO₃ will produce 0.1224moles of KCl

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How many grams of NH3 are needed to provide the same number of molecules as in 0.35 g of SF6 ?

Strike441 [17]

Answer:

There are 0.041 g of NH₃ in the same number of molecules as in 0.35 g of SF₆.

Explanation:

Using the molar mass of the chemical formula SF₆ you can find the number of moles of molecules in 0.35 g of such substance. Then, using the molar mass of NH₃, you can find mass in grams corresponding to the same number of molecules.

1. Find the molar mass of SF₆:

Atom atomic mass number of atoms total mass in 1 mole

S 32.065 g/mol 1 32.065 g

F 18.998 g/mol 6 6 × 18.998 = 113.988 g

=====================

molar mass of SF₆ = 146.053 g/mol

2. Find the number of moles in 0.35 g of SF₆:

number of moles = mass in grams / molar mass

number of moles = 0.35 g / 146.053 g / mol = 0.0024 mol

3. Find the molar mass of NH₃:

Atom atomic mass number of atoms total mass 1 mole

N 14.007 g/mol 1 14.007 g

H 1.008 g/mol 3 3 × 1.008 g = 113.988 g

=====================

molar mass of NH₃ = 17.031 g/mol

4. Find the mass in 0.0024 mol of NH₃:

mass in grams = number of moles × molar mass

mass = 0.0024 mol × 17.031 g/mol ≈ 0.041 grams

5. Conclusion:

There are 0.041 g of NH₃ in the same number of molecules as in 0.35 g of SF₆.

6 0

2 years ago

Perform the following operation

xxMikexx [17]

Explanation:

3.4000x 10-6 +5.7000x 10-3

$3.4000 \times {10}^{ - 6} = 3.4 \times {10}^{ - 6}$

$5.7000 \times {10}^{ - 3} = 5700 \times {10}^{ - 6}$

now we can add them

$3.4 + 5700 = 5703.4 \\ = 5703.4 \times {10}^{ - 6}$

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2 years ago

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2 years ago

Chlorine gas can be made from the reaction of manganese dioxide with hydrochloric acid. MnO2(s) + 4HCl(aq) → MnCl2(aq) + 2H2O(l)

Marina CMI [18]

Answer:

Please see the complete formt of the question below

Chlorine gas can be made from the reaction of manganese dioxide with hydrochloric acid.

MnO₂(s) + HCl(aq) → MnCl₂(aq) + H₂O(l) + Cl₂(g)

According to the above reaction, determine the limiting reactant when 5.6 moles of MnO₂ are reacted with 7.5 moles of HCl.

The answer to the above question is

The limiting reactant is the MnO₂

Explanation:

To solve this, we note that one mole of MnO₂ reacts with one mole of HCl to produce one mole of MnCl₂, one mole of H₂O and one mole of Cl₂

Molar mass of MnO₂ = 86.9368 g/mol

Molar mass of HCl = 36.46 g/mol

From the stoichiometry of the reaction, 5.6 moles of MnO₂ will react with 5.6 moles of HCl to produce 5.6 moles of H₂O and 5.6 moles of Cl₂

However there are 7.5 moles of HCL therefore there will be an extra 7.5-5.6 or 1.9 moles of HCl remaining when the reaction is completed

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2 years ago

Suggest why sodium and hydrogen ions do not diffuse at the same rate

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Answer:

sodium has got ionic bonds that are weak

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2 years ago