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3 years ago

What is the density of a bar of lead that weighs 173 g and has the following dimensions: l= 2.00 cm, w = 3.00 cm, h = 1.00 in?

Chemistry

1 answer:

oksano4ka [1.4K]3 years ago

8 0

Answer:

$\rho=7373.2g/cm^3$

Explanation:

Hello!

In this case, since the density is defined as the degree of compactness of a substance, and is defined as the mass over the volume:

$\rho= \frac{m}{V}$

Given the dimensions of the bar of lead, we can compute the volume as shown below:

$V=2.00cm*3.00cm*1.00in*\frac{1in}{2.54cm} \\\\V=2.36cm^3$

Thus, the density turns out:

$\rho=\frac{173g}{2.36cm^3} \\\\\rho=7373.2g/cm^3$

Best regards!

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Mrrafil [7]

Answer:

0.4694 moles of CrCl₃

Explanation:

The balanced equation is:

Cr₂O₃(s) + 3CCl₄(l) → 2CrCl₃(s) + 3COCl₂(aq)

The stoichiometry of the equation is how much moles of the substances must react to form the products, and it's represented by the coefficients of the balanced equation. So, 1 mol of Cr₂O₃ must react with 3 moles of CCl₄ to form 2 moles of CrCl₃ and 3 moles of COCl₂.

The stoichiometry calculus must be on a moles basis. The compounds of interest are Cr₂O₃ and CrCl₃. The molar masses of the elements are:

MCr = 52 g/mol

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So, the molar mass of the Cr₂O₃ is = 2x52 + 3x35.5 = 210.5 g/mol.

The number of moles is the mass divided by the molar mass, so:

n = 49.4/210.5 = 0.2347 mol of Cr₂O₃.

For the stoichiometry:

1 mol of Cr₂O₃ ------------------- 2 moles of CrCl₃

0.2347 mol of Cr₂O₃----------- x

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x = 0.4694 moles of CrCl₃

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What are Rhodium isotopes used for?

Lina20 [59]

Answer:

Rhodium is used to make electrical contacts, as jewelry and in catalytic converters, but is most frequently used as an alloying agent in other materials, such as platinum and palladium. These alloys are used to make such things as furnace coils, electrodes for aircraft spark plugs and laboratory crucibles.

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Akimi4 [234]

Answer:

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