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VMariaS [17]
2 years ago
8

What is the molar mass of al (clo2)3

Chemistry
1 answer:
frozen [14]2 years ago
4 0
The molar mass is 229.33
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Increased motion in the particles in a liquid allows the particles to
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Particles in a liquid are more loosely packed there for they have more room to move and can flow around eachother . Hope this helps XD
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When C2H5Cl(g) is burned in oxygen, chlorine gas is produced in addition to carbon dioxide and water vapor. 5145 kJ of heat are
Arisa [49]

<u>Answer:</u> The chemical equation is written below.

<u>Explanation:</u>

Combustion reaction is defined as the chemical reaction in which a hydrocarbon reacts with oxygen gas to produce carbon dioxide gas and water molecule.

\text{hydrocarbon}+O_2\rightarrow CO_2+H_2O

The chemical equation for the combustion of ethyl chloride follows:

4C_2H_5Cl+13O_2\rightarrow 2Cl_2+8CO_2+10H_2O

We are given:

When 4 moles of ethyl chloride is burnt, 5145 kJ of heat is released.

For an endothermic reaction, heat is getting absorbed during a chemical reaction and is written on the reactant side.

A+\text{heat}\rightleftharpoons B

For an exothermic reaction, heat is getting released during a chemical reaction and is written on the product side

A\rightleftharpoons B+\text{heat}

So, the chemical equation follows:

4C_2H_5Cl+13O_2\rightarrow 2Cl_2+8CO_2+10H_2O+5145kJ

Hence, the chemical equation is written above.

7 0
2 years ago
A chemist heats 100.0 g of FeSO4 x 7H2O in a crucible to drive off the water. If all the water is driven off, what is the mass o
Ierofanga [76]
FeSO₄*7H₂O(s) = FeSO₄(s) + 7H₂O(g)

M(FeSO₄*7H₂O)=278.0 g/mol
M(FeSO₄)=151.9 g/mol

m(FeSO₄*7H₂O)/M(FeSO₄*7H₂O)=m(FeSO₄)/M(FeSO₄)

m(FeSO₄)=M(FeSO₄)m(FeSO₄*7H₂O)/M(FeSO₄*7H₂O)

m(FeSO₄)=151.9*100.0/278.0=54.6 g

m(FeSO₄)=54.6 g


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What is the identity of a sample that has a mass of 2.44 g and a volume of 0.34 cm3?
borishaifa [10]
The answer would be zinc
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What is the mass of 3.35 mol Hg(IO3)2? 1,700 g 1,840 g 1,960 g 2,110 g
Tema [17]

Answer:- 1840 g.

Solution:- We have been given with 3.35 moles of Hg(IO_3)_2 and asked to calculate it's mass.

To convert the moles to grams we multiply the moles by the molar mass of the compound. Molar mass of the compound is the sum of atomic masses of all the atoms present in it.

molar mass of Hg(IO_3)_2 = atomic mass of Hg + 2(atomic mass of I) + 6(atomic mass of O)

= 200.59+2(126.90)+6(16.00)

= 200.59+253.80+96.00

= 550.39 gram per mol

Let's multiply the given moles by the molar mass:

3.35mol(\frac{550.39g}{1mol})

= 1843.8 g

Since, there are three sig figs in the given moles of compound, we need to round the calculated my to three sig figs also. So, on rounding off to three sig figs the mass becomes 1840 g.

8 0
2 years ago
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