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Gekata [30.6K]
3 years ago
10

the pressure on a 205 mL volume of gas is decreased from 985 mm hg to 615 mm hg while constant temperature is maintained, What i

s the new volume of the gas?
Chemistry
2 answers:
Softa [21]3 years ago
7 0
The new volume of gas should be 328.33 mL
viktelen [127]3 years ago
4 0

Answer:

\boxed {\boxed {\sf 328 \ mL}}

Explanation:

The pressure on the gas changes, while the temperature remains constant, and we want to find the new volume. So, we will use Boyle's Law, which states there is an inverse relationship between the pressure on a gas and the volume of the gas. The formula is:

{P_1V_1}= P_2V_2

The pressure of the gas is originally 985 mm Hg and the volume is 205 milliliters.

985 \ mm \ Hg * 205 \ mL = P_2V_2

The pressure is decreased to 615 mm Hg, but the new volume is unknown.

985 \ mm \ Hg * 205 \ mL = 615 \ mm \ Hg * V_2

We are solving for the new volume, so we must isolate the variable V₂. It is being multiplied by 615 millimeters of mercury.. The inverse of multiplication is division, so we divide both sides of the equation by 615 mm Hg.

\frac {985 \ mm \ Hg * 205 \ mL}{615 \ mm \ Hg} = \frac{615 \ mm \ Hg * V_2}{615 \ mm \ Hg}

\frac {985 \ mm \ Hg * 205 \ mL}{615 \ mm \ Hg} = V_2

The units of millimeters of mercury (mm Hg) cancel.

\frac {985 \  * 205 \ mL}{615 } = V_2

\frac{201925 }{ 615} \ mL = V_2

328.3333333 \ mL = V_2

The original measurements have 3 significant figures, so our answer must have the same. For the number we calculated, that is the ones place.

The 3 to the right in the tenths place tells us to leave the 8 in the ones place.

328 \ mL \approx V_2

The new volume of the gas is approximately <u>328 milliliters.</u>

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Answer:

90.99 or 91.0

Explanation:

Using the balanced equation, you convert 38.5g of ethanol to moles of water. From there, you plug the values into the Ideal Gas Equation: PV=nRT.

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Answer is: beryllium-10.

The diagram shows that atom has 4 protons, 5 neutrons and 2 valence electrons.

Atomic number is the number of protons, which is characteristic of a chemical element, beryllium (Be) is an element with atomic number 4.

Two valence electrons means that atom is from 2. group of periodic table, only beryllium is from that group; sodium (1. group), boron (13. group) and carbon (14. group).

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1. If the frequency of a wave increases from 2 Hz to 4 Hz without the wavelength changing, how will the wave speed change?
maw [93]

Answer:

Given expression: 6(2b-4). To find the value of 6(2b-4) at b= 5, we need to substitute the b=5 in the expression, we get….Therefore, the value of 6(2b-4) is 36, when b=5.

Explanation:

Given expression: 6(2b-4). To find the value of 6(2b-4) at b= 5, we need to substitute the b=5 in the expression, we get….Therefore, the value of 6(2b-4) is 36, when b=5.

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Calculate the mass of khc8h4o4 that reacts with 15 ml of the naoh solution
dlinn [17]
The balanced chemical reaction would be:

 KHC8H4O4<span> (aq) + </span>NaOH<span> (aq) → NaKC8H4O4 (aq) + H2O.

The concentration of the NaOH is equal 0.1 M. We use this and the volume given above to determine the mass of KH</span>C8H4O4. We do as follows:

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3 years ago
At a certain temperature, the vapor pressure of pure benzene ‍ is atm. A solution was prepared by dissolving g of a nondissociat
erastova [34]

Answer:

Molar mass of solute: 300g/mol

Explanation:

<em>Vapor pressure of pure benzene: 0.930 atm</em>

<em>Assuming you dissolve 10.0 g of the non-volatile solute in 78.11g of benzene and vapour pressure of solution was found to be 0.900atm</em>

<em />

It is possible to answer this question based on Raoult's law that states vapor pressure of an ideal solution is equal to mole fraction of the solvent multiplied to pressure of pure solvent:

P_{sln} = X_{solvent}P_{solvent}^0

Moles in 78.11g of benzene are:

78.11g benzene × (1mol / 78.11g) = <em>1 mol benzene</em>

Now, mole fraction replacing in Raoult's law is:

0.900atm / 0.930atm = <em>0.9677 = moles solvent / total moles</em>.

As mole of solvent is 1:

0.9677× total moles = 1 mole benzene.

Total moles:

1.033 total moles. Moles of solute are:

1.033 moles - 1.000 moles = <em>0.0333 moles</em>.

As molar mass is the mass of a substance in 1 mole. Molar mass of the solute is:

10.0g / 0.033moles = <em>300g/mol</em>

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