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Monica [59]
3 years ago
9

Given 6.25 mol H2O, determine the number of molecules

Chemistry
1 answer:
marissa [1.9K]3 years ago
8 0

No of molecules=No of moles× Avagadro no

\\ \sf\longmapsto 6.25\times 6.023\times 10^{23}

\\ \sf\longmapsto 37.6\times 10^{23}

\\ \sf\longmapsto 3.8\times 10^{24}molecules

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9, What is an Independent
stepan [7]

Answer:

Not influenced or controlled by others in matters of opinion

8 0
3 years ago
Natural gas (CH4) has a molar mass of 16.0 g/mole. You started out the day with a tank containing 200.0 g of natural gas. At the
hodyreva [135]

Considering the definition of molar mass, the moles of gas used are 10.625 moles.

<h3>Definition of molar mass</h3>

The molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.

<h3>Amount of moles used</h3>

Natural gas has a molar mass of 16.0 g/mole.

You started out the day with a tank containing 200.0 g of natural gas.  So, you can apply the following rule of three: If by definition of molar mass 16 grams are contained in 1 mole, 200 grams are contained in how many moles?

amount of moles at the beginning=\frac{200 gramsx1 mole}{16 grams}

<u><em>amount of moles at the beginning= 12.5 moles</em></u>

At the end of the day, your tank contains 30.0 g of natural gas. So, you can apply the following rule of three: If by definition of molar mass 16 grams are contained in 1 mole, 30 grams are contained in how many moles?

amount of moles at the end=\frac{30 gramsx1 mole}{16 grams}

<u><em>amount of moles at the end= 1.875 moles</em></u>

The number of moles used will be the difference between the number of moles used initially and the contents at the end of the day.

moles used= amount of moles at the beginning - amount of moles at the end

moles used= 12.5 moles - 1.875 moles

<u><em>moles used= 10.625 moles</em></u>

<u><em /></u>

Finally, the moles of gas used are 10.625 moles.

Learn more about molar mass:

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3 0
2 years ago
Im hvaing a hard time getting the right answer
Tanya [424]

Answer:

V=23.9mL

Explanation:

Hello!

In this case for the solution you are given, we first use the mass to compute the moles of CuNO3:

n=2.49g*\frac{1mol}{125.55 g}=0.0198mol

Next, knowing that the molarity has units of moles over liters, we can solve for volume as follows:

M=\frac{n}{V}\\\\V=\frac{n}{M}

By plugging in the moles and molarity, we obtain:

V=\frac{0.0198mol}{0.830mol/L}=0.0239L

Which in mL is:

V=0.0239L*\frac{1000mL}{1L}\\\\V=23.9mL

Best regards!

6 0
3 years ago
Fluorine gas reacts with aqueous iron (II) iodine to produce iron (II) fluoride and iodine liquid What is the balanced chemical
Andru [333]

Answer:

F₂ (g) + FeI₂ (aq) →  FeF₂ (aq) +  I₂ (l)

Explanation:

Our reactants are:

F₂ → Fluorine gas, a dyatomic molecule

FeI₂ → Iron (II) iodine

Our products are:

I₂ → Iodine

FeF₂ → Iron (II) fluoride

Then, the reaction is:

F₂ (g) + FeI₂ (aq) →  FeF₂ (aq) +  I₂ (l)

We see it is completely balanced.

6 0
2 years ago
Balance the equation 2kclo3 3o2 + kcl
sergij07 [2.7K]
Answer is 2KClO3 3O2 + 2KCl
5 0
3 years ago
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