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2 years ago

Calculate the mass (grams) of 0.750 moles of Al2(Cr2O7)3

Chemistry

1 answer:

garik1379 [7]2 years ago

8 0

Answer:

526g is the mass of this sample

Explanation:

To solve this question we must, as first, find the <em>molar mass </em>of Al₂(Cr₂O₇)₃ using the periodic table. The molar mass is defined as the mass of this compound per mole. With this value we can find the mass in 0.750 moles as follows:

<em>Molar mass Al₂(Cr₂O₇)₃</em>

2Al = 2*26.98g/mol = 53.96g/mol

6 Cr = 6*51.9961g/mol = 311.9766g/mol

21 O = 21*15.999g/mol = 335.979g/mol

53.96g/mol + 311.9766g/mol + 335.979g/mol

= 701.9156g/mol

The mass of 0.750 moles is:

0.750 moles * (701.9156g / mol) =

<h3>526g is the mass of this sample</h3>

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3 years ago

Cars run on gasoline, where octane (C8H18) is the principle component. This combustion reaction is responsible for generating en

Bezzdna [24]

Answer:

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Explanation:

The combustion reaction of Octane is:

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We calculate the mass of Octane from the given volume and density, using the following <em>conversion factors</em>:

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1 L = 1000 mL

Now we<u> convert 1.24 gallons to mL</u>:

1.24 gallon * $\frac{3.785L}{1gallon} *\frac{1000mL}{1L} =$ 4693.4 mL

We <u>calculate the mass of Octane</u>:

4693.4 mL * 0.703 g/mL = 3.30 g Octane

Now we use the <em>stoichiometric ratios</em> and <em>molecular weights</em> to <u>calculate the mass of CO₂ and H₂O</u>:

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3 years ago

How many moles of oxygen are there in 3 moles of Zn(NO3)2? (2 points)

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2 years ago

35.0 mL of 12.0 M HCl is added to enough water to have a final volume of 1.20 L. What is the molarity of the final solution?

creativ13 [48]

<h3>Answer:</h3>

0.35 M

<h3>Explanation:</h3>

<u>We are given;</u>

Initial volume as 35.0 mL or 0.035 L
Initial molarity as 12.0 M
Final volume is 1.20 L

We are required to determine the final molarity of the solution;

Dilution involves adding solvent to a solution to make it more dilute which reduces the concentration and increases the solvent while maintaining solute constant.

Using dilution formula we can determine the final molarity.

M1V1 = M2V2

Rearranging the formula;

M2 = M1V1 ÷ V2

= (12.0 M × 0.035 L) ÷ 1.2 L

= 0.35 M

Thus, the final concentration of the solution is 0.35 M

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3 years ago