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3 years ago

How many moles are equivalent to 365 g of aluminum chloride? Using the dimensions analysis. Show work

Chemistry

1 answer:

frosja888 [35]3 years ago

3 0

Answer:

≈ 2.74 mol $AlCl_{3}$

(I rounded to 3 sig figs because the starting amount has 3 sig figs.)

Explanation:

$\frac{365g AlCl_{3}}{1}*\frac{1 mol AlCl_{3}}{133.34g AlCl_{3}} =$ 2.73736313184 mol $AlCl_{3}$ ≈ 2.74 mol $AlCl_{3}$

Hope this helps!

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What volume (L) will 3.56 mol NH3 occupy at STP. (1 point)

mart [117]

Answer:

Explanation:

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3 years ago

How many milliliters of water are needed to prepare a 3.5M solution of NaOH if you have .5mol of the solute

Mamont248 [21]

Answer:

1335.12 mL of H2O

Explanation:

To calculate the mililiters of water that the solution needs, it is necessary to know that the volume of the solution is equal to the volume of the solute (NaOH) plus the volume of the solvent (H2O).

From the molarity formula we can first calculate the volume of the solution:

$M=\frac{solute moles}{solution volume}$

$Solutionvolume=\frac{solute moles}{M} =\frac{5mol}{3.5\frac{mol}{L} } =1.429L$

The volume of the solution as we said previously is:

Solution volume = solute volume + solvent volume

To determine the volume of the solute we first obtain the grams of NaOH through the molecular weight formula:

$MW=\frac{mass}{mol}$

$Mass=MW*mol=39.997\frac{g}{mol} *5mol=199.985g$

Now with the density of NaOH the milliliters of solute can be determined:

$d=\frac{mass}{volume}$

$Volume=\frac{mass}{d} =\frac{199.985g}{2.13\frac{g}{mL} } =93.88mL of NaOH$

Having the volume of the solution and the volume of the solute, the volume of the solvent H2O can be calculated:

Solvent volume = solution volume - solute volume

Solvent volume = 1429 mL - 93.88 mL = 1335.12 mL of H2O

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3 years ago

What is the charge of oxygen in Na2O?

Nuetrik [128]

In Na2O, what is the oxidation state of oxygen? In Na2O oxidation state of Na is 1+

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3 years ago

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Balance the equation by ion electron method

irina1246 [14]

Answer:i believe you are to decompose the formula (i think)

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3 years ago

How many milliliters of 0.50 M KOH are needed

spayn [35]

Answer:

Option D. 30 mL.

Explanation:

Step 1:

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

HNO3 + KOH —> KNO3 + H2O

From the balanced equation above,

The mole ratio of the acid, nA = 1

The mole ratio of the base, nB = 1

Step 2:

Data obtained from the question. This include the following:

Volume of base, KOH (Vb) =.?

Molarity of base, KOH (Mb) = 0.5M

Volume of acid, HNO3 (Va) = 10mL

Molarity of acid, HNO3 (Ma) = 1.5M

Step 3:

Determination of the volume of the base, KOH needed for the reaction. This can be obtained as follow:

MaVa / MbVb = nA/nB

1.5 x 10 / 0.5 x Vb = 1

Cross multiply

0.5 x Vb = 1.5 x 10

Divide both side by 0.5

Vb = (1.5 x 10) /0.5

Vb = 30mL

Therefore, the volume of the base, KOH needed for the reaction is 30mL.

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3 years ago