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satela [25.4K]
2 years ago
7

If you doubled the volume of a sample of gas and

Chemistry
2 answers:
GREYUIT [131]2 years ago
6 0

Answer:

The absolute temperature  of the gas will be affected by a fourfold increase.

The pressure must be applied at 450 K should be 1,125 torr.

Explanation:

Charles's Law consists in the relationship between the volume and temperature of a certain amount of ideal gas, which is maintained at a constant pressure, by means of a constant of proportionality that is applied directly. For a given sum of gas at a constant pressure, as the temperature increases, the volume of the gas increases and when the temperature decreases, the volume of the gas decreases because the temperature is directly related to the energy of the movement of the gas molecules .

In summary, Charles's law is a law that says that when the amount of gas and pressure remain constant, the ratio between volume and temperature will always have the same value:

\frac{V}{T} =k (constant)

If you double the volume of a gas sample and  then doubled the volume again, then the volume was increased four times. To comply with Charles's Law and maintain the relationship between volume and constant temperature, the temperature must increase four times, in the same way as volume.

So <u><em> the absolute temperature  of the gas will be affected by a fourfold increase.</em></u>

Gay-Lussac's law can be expressed mathematically as follows:

\frac{P}{T} =k

Where P = pressure, T = temperature, K = Constant

This law indicates that the ratio between pressure and temperature is constant.

This law indicates that, as long as the volume of the container containing the gas is constant, as the temperature increases, the gas molecules move faster. Then the number of shocks against the walls increases, that is, the pressure increases. That is, the gas pressure is directly proportional to its temperature.

In short, when there is a constant volume, as the temperature increases, the gas pressure increases. And when the temperature decreases, gas pressure decreases.

When studying two different states of a gas, you have a gas that is at a pressure P1 and at a temperature T1 at the beginning of the experiment. When the temperature varies to a new T2 value, then the pressure will change to P2. This is true:

\frac{P1}{T1} =\frac{P2}{T2}

So in this case, as the volume is constant, Gay-Lussac's law can be applied as follows:

\frac{750 torr}{300 K} =\frac{P2}{450 K}

Then

P2=\frac{750 torr}{300 K} *450 K\\

P2=1,125 torr

<u><em>The pressure must be applied at 450 K should be 1,125 torr.</em></u>

Dimas [21]2 years ago
3 0

Answer:

1125mL

Explanation:

this can be done using general gas law

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The pKa of lactic acid is 3.9. A lactate buffer will be useful from pH values ________. The pKa of lactic acid is 3.9. A lactate
Vedmedyk [2.9K]

Answer:

Explanation:

The usefulness of a buffer is its ability to resist changes in pH when small quantities of base or acid are added to it. This ability is the consequence of having both the conjugate base and the weak acid present in solution which will consume the added base or acid.  

This capacity is lost if the ratio of the concentration of conjugate base to the concentration of weak acid differ by an order of magnitude. Since  buffers having ratios differing by more will have their pH driven by either the weak acid or its conjugate base .

From the Henderson-Hasselbach equation we have that

pH = pKa + log [A⁻]/[HA]

thus

0.1 ≤  [A⁻]/[HA] ≤ 10

Therefore the log of this range is -1 to 1, and the pH will have a useful range of within +/- 1 the pKa of the buffer.

Now we are equipped to answer our question:

pH range = 3.9 +/- 1 = 2.9 through 4.9

7 0
3 years ago
2. A 2.5 mol SAMPLE OF OXYGEN GAS (O2) INCREASES TO 3.2 mol
lana [24]

696.32 mmHg is the final pressure of the gas.

<h3>What is an ideal gas equation?</h3>

The ideal gas equation, pV = nRT, is an equation used to calculate either the pressure, volume, temperature or number of moles of a gas.

Given data:

P_1 = 720 mmHg              

P_2 = ?

n_1 = 2.5 mol                

n_2 = 3.2 mol

V_1 = 34 L            

V_2 = 45 L

Formula

Combined gas law

\frac{P_1 V_1}{n_1}  = \frac{P_2 V_2}{n_2}

P_2 = 696.32 mmHg

Hence, 696.32 mmHg is the final pressure of the gas.

Learn more about an ideal gas equation here:

brainly.com/question/19251972

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6 0
2 years ago
Geothermal energy helps to
disa [49]

Answer:A

Explanation:

4 0
3 years ago
Name the Scientist
IRISSAK [1]

Answer:

A. Ernest Rutherford

B.Bohr

C. Eugen Goldstein

D.. Santiago Ramon y cajal

E.john Dalton

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example.. argon 40

potassium 40

.two differences between isobars and isotopes.

isobars are those elements which have different atomic number but the same mass number. while isotopes are those elements having the same atomic number and different mass number..

two uses of isotopes.

uranium 235 - for nuclear fission and as fuel in unclear reactors.

# an isotope cobalt - used In the treatment for cancer

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7 0
3 years ago
If the mole fraction of sulfuric acid H2SO4 is 0.432 what is the percent by mass of H2SO4.
Sever21 [200]

Answer:

19.47%

Explanation:

<em>The percentage by mass of </em>H_2SO_4<em> would be </em><em>19.47%</em><em>.</em>

The percentage by mass of a substance in solution is calculated as:

   \frac{mass of substance}{mass of substance + water}  * 100%

Given that the mole fraction of H_2SO_4 = 0.432

The total number of mole fraction of a solution = 1

Hence, mole fraction of water = 1 - 0.432 = 0.568

Mass of water = molar mass x mole

                              = 98.079 x 0.432 = 42.37 g

Mass of H_2SO_4 = molar mass x mole

                          = 18.02 x 0.568 = 10.24 g

Hence,

<em>%mass of</em> H_2SO_4 = \frac{10.24}{10.24 + 42.37} * 100

                         = 19.47%

4 0
3 years ago
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