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3 years ago

Convert the following pressures to pressure in standard atmosphere 151.98 kPa 456 torr

Chemistry

1 answer:

Korolek [52]3 years ago

5 0

Answer:

Kpa to atm = 1.5 atm

torr to atm = 0.6 atm

Explanation:

Atmospheric pressure:

It is the pressure exerted by atmosphere at a sea level with the means value of 101.325 pascal.

It is also known as barometric pressure.

It is denoted as "atm"

The value of standard atmospheric pressure is 1.

Kpa to atm:

To convert the kilopascal into atm we would divide the given value by 101.

151.98 kpa × 1 atm /101.325 kpa

1.5 atm

torr to atm:

To convert the torr into atm we would divide the given value by 760.

456 torr × 1 atm /760 torr

0.6 atm

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Answer

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This is a redox reaction (oxidation-reduction reaction) which involves the transfer of electrons between two species. i.e

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C) An electron has a negative charge and is located outside the nucleus.

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4 years ago

Calculate the molar mass of Fe2(SO4)3. Then Calculate the mass of iron(III) sulfate of 4.05x10^23 formula units. Work must be sh

Talja [164]

Answer:

Molar mass: 399.9 g/mol

The mass of iron(III) sulfate is 269 grams.

Explanation:

First of all, you have to find the molar mass of Fe2(SO4)3.

So you find the molar first for each element

However, there are 2 iron atoms, 3 sulfur atoms, and 12 oxygen atoms.(Don't forget the 3 outside the parenthesis of SO4).

So you do this

So the final answer is 399.9 g/mol

Second of all, if you want to find the mass of Fe2(SO4)3, you have to convert from formula units to moles. After that, then you convert from moles to grams.

If you want to convert from molecules to molecules, you have to use Avogadro's number. Avogadro's number is 6.02 x 10^23. Then if you want to convert from moles to grams, you use the molar mass. We already know that the molar mass is 399.9 g/mol.

Therefore, now use dimensional analysis to show your work.

<h3>(4.05 x 10^23) formula units of Fe2(SO4)3 * 1 mol/ 6.02 x 10^23 formula units * 399.9 g/mol / mol</h3>

Formula units in the beginning and the moles will cancel out.

But we need to use significant figures with the least digits(which is 4.05) So we round to the nearest whole number.

So the final answer for the mass of iron(III) sulfate is 269 grams(don't forget the units).

Hope it helped!

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3 years ago

A sample of 9.27 g9.27 g of solid calcium hydroxide is added to 38.5 mL38.5 mL of 0.500 M0.500 M aqueous hydrochloric acid. Writ

navik [9.2K]

<u>Answer:</u> The excess reagent for the given chemical reaction is calcium hydroxide and the amount left after the completion of reaction is 0.115375 moles. The amount of calcium chloride formed in the reaction is 1.068 grams.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ....(1)

<u>For calcium hydroxide:</u>

Given mass of calcium hydroxide = 9.27 g

Molar mass of calcium hydroxide = 74.093 g/mol

Putting values in above equation, we get:

$\text{Moles of calcium hydroxide}=\frac{9.27g}{74.093g/mol}=0.125mol$

To calculate the moles of a solute, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

We are given:

Volume of hydrochloric acid = 38.5mL = 0.0385 L (Conversion factor: 1 L = 1000 mL)

Molarity of the solution = 0.500 moles/ L

Putting values in above equation, we get:

$0.500mol/L=\frac{\text{Moles of hydrochloric acid}}{0.0385L}\\\\\text{Moles of hydrochloric acid}=0.01925mol$

For the given chemical equation:

$2HCl(aq.)+Ca(OH)_2(s)\rightarrow CaCl_2(s)+2H_2O(l)$

Here, the solid salt is calcium chloride.

By Stoichiometry of the reaction:

2 moles of hydrochloric acid reacts with 1 mole of calcium hydroxide.

So, 0.01925 moles of hydrochloric acid will react with = $\frac{1}{2}\times 0.01925=0.009625moles$ of calcium hydroxide.

As, given amount of calcium hydroxide is more than the required amount. So, it is considered as an excess reagent.

Thus, hydrochloric acid is considered as a limiting reagent because it limits the formation of product.

Amount of excess reagent (calcium hydroxide) left = 0.125 - 0.01925 = 0.115375 moles

By Stoichiometry of the reaction:

2 moles of hydrochloric acid produces 1 mole of calcium chloride.

So, 0.01925 moles of hydrochloric acid will produce = $\frac{1}{2}\times 0.01925=0.009625moles$ of calcium chloride.

Now, calculating the mass of calcium chloride from equation 1, we get:

Molar mass of calcium chloride = 110.98 g/mol

Moles of calcium chloride = 0.009625 moles

Putting values in equation 1, we get:

$0.009625mol=\frac{\text{Mass of calcium chloride}}{110.98g/mol}\\\\\text{Mass of calcium chloride}=1.068g$

Hence, the excess reagent for the given chemical reaction is calcium hydroxide and the amount left after the completion of reaction is 0.115375 moles. The amount of calcium chloride formed in the reaction is 1.068 grams.

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Answer:

True

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