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3 years ago

What mass of water is required to react completely with 157.35 g CO2?

Chemistry

2 answers:

dimulka [17.4K]3 years ago

8 0

Answer:64.43g H2O

Explanation: the other one is wrong

motikmotik3 years ago

3 0

Assuming that the question is about making glucose, then you need to know the equation for the reaction. The equation should be:

C6H12O6<span>(s) + 6O2(g) -->6CO2(g) + 6H2O(g)

In this equation, 6 molecules of CO2 would react with 6 molecules of H2O which mean it has 1:1 ratio. The molecular weight for CO2 should be 44g/mole and H2O is 18g/mole. Then the calculation would be: 6/6 * (157.35g/44g) * 18g= 64.37g</span>

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How many molecules are there in 0.45 moles of so3

vivado [14]

Answer:

2.71

Explanation:

6 0

2 years ago

To answer this question, you will need to write the balanced equation and set up a BCA table. Using appropriate rounding rules,

Elenna [48]

Water decomposes when electrolyzed to produce hydrogen and oxygen gas. If 2.5 grams of water were decomposed 1.04 grams of oxygen will be formed.

BCA table:

2 $H_{2}$ O ⇒ $H_{2}$ + $O_{2}$

B 0.13 0 + 0

C -0.13 0.065 + 0.065

A 0 0.065

Explanation:

Balanced equation for water decomposition into hydrogen and oxygen gases

2 $H_{2}$ O ⇒ $H_{2}$ + $O_{2}$

B 0.13 0 + 0

C -0.13 0.065 + 0.065

A 0 0.065

Number of moles of water = $\frac{mass}{atomic mass of 1 mole}$

mass = 2.5 grams

atomic mass= 18 grams

number of moles can be known by putting the values in the formula,

n = $\frac{2.5}{18}$

= 0.13 moles

2 moles of water gives one mole of oxygen on decomposition

so, 0.13 moles of water will give x moles of oxygen on decompsition

$\frac{1}{2}$ = $\frac{x}{0.13}$

x = 0.065 moles of oxygen will be formed.

moles to gram will be calculated as

mass =number of moles x atomic mass

= 0.065 x 16

= 1.04 grams of oxygen.

7 0

3 years ago

Iron and oxygen form rust. How many moles of rust should be produced if 1

kakasveta [241]

Answer:

1.387 moles

Explanation:

Step 1:

The balanced equation for the reaction. This is illustrated below:

4Fe + 3O2 —> 2Fe2O3

Step 2:

Determination of the number of mole of Fe in 155.321g of Fe. This can be achieved by doing the following:

Mass of Fe = 155.321g

Molar Mass of Fe = 56g/mol

Number of mole of Fe =?

Number of mole = Mass/Molar Mass

Number of mole of Fe = 155.321/56

Number of mole of Fe = 2.774 mol

Step 3:

Determination of the number of mole of rust (Fe2O3) produced. This is illustrated below:

From the balanced equation above,

4 moles of Fe produced 2 moles of Fe2O3.

Therefore, 2.774 moles of Fe will produce = (2.774 x 2)/4 = 1.387 moles of Fe2O3.

Therefore, 1.387 moles of rust (Fe2O3) is produced from the reaction

6 0

3 years ago

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igor_vitrenko [27]

Answer:

aqueous solution

Explanation:

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3 years ago

How to differ mixture and compound? What are their differences?

Roman55 [17]

Explanation:

"Compound: A substance that is made up of more than one type of atom bonded together.

Mixture: A combination of two or more elements or compounds which have not reacted to bond together; each part in the mixture retains its own properties."

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8 0

2 years ago

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