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irakobra [83]
3 years ago
8

A sample of cl2 gas has a volume of 15.0 l at a pressure of 1.50 atm and a temperature of 23 °c. What volume, in liters, will th

e gas occupy at 3.50 atm and 286 °c? Assume ideal behavior.
Chemistry
2 answers:
kotegsom [21]3 years ago
8 0

Volume of Cl₂ gas at 3.5 atm and 286°C = <u>12.14 L</u>

<h3>Further explanation </h3>

Some of the laws regarding gas, can apply to ideal gas (volume expansion does not occur when the gas is heated), among others  

• Boyle's law at constant T, P = 1 / V  

• Charles's law, at constant P, V = T  

• Avogadro's law, at constant P and T, V = n  

So that the three laws can be combined into a single gas equation, the ideal gas equation  

In general, the gas equation can be written  

\large{\boxed{\bold{PV=nRT}}}

where  

P = pressure, atm  

V = volume, liter  

n = number of moles  

R = gas constant = 0.082 l.atm / mol K  

T = temperature, Kelvin

State 1

V1= 15 L

P1 = 1.5 atm

T1 = 23°C +273 = 296 K

We can find mole(n)

\displaystyle n=\frac{PV}{RT}\\\\n=\frac{1.5.15}{0.082.296}\\\\n=0.927

State 2

P2=3.5 atm

T = 286°C +273 = 559 K

n (from state 1) = 0.927

\displaystyle V=\frac{n.R.T}{P}\\\\V=\frac{0.927.0.082.559}{3.5}\\\\V=\boxed{\bold{12.14~L}}

<h3>Learn more  </h3>

Which equation agrees with the ideal gas law  

brainly.com/question/3778152  

brainly.com/question/1056445  

Which law relates to the ideal gas law  

brainly.com/question/6534096  

Keywords : ideal gas law, Cl₂

olganol [36]3 years ago
4 0

Given: Initial volume of CO_{2} gas= 15.0 L

Pressure=1.50 atm

Temperature=23°C

Use ideal gas equation as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature in Kelvin.

First convert the given temperature in Kelvin.

0°C=273.15 K

Thus, 23 °C=296.15 K

Rearranging ideal gas equation to calculate the value of nR as follows:

nR=\frac{PV}{T}=\frac{(1.50 atm)(15.0 L)}{(296.15 K)}=0.0760 atm LK^{-1}

Now, final pressure is 3.50 atm and temperature is 286°C, converting the temperature into Kelvin,

0°C=273.15 K

Thus, 286 °C=559.15 K

Volume can be calculated using the ideal gas equation as follows:

V=\frac{nRT}{P}

Putting the value of given pressure and temperature and the above calculated value of nR,

V=\frac{(0.0760 atmLK^{-1})(559.15 K)}{(3.50 atm)}=12.14 L

Therefore, volume of CO_{2} at 3.50 atm and 286°C is 12.14 L.

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The first Slater rule says that we need to group:

(1s^{2}) (2s, 2p)^{8} (3s, 3p)^{8} (3d^{10}) (4s, 4p)^{8} (4d^{10}) (5s, 5p)^{8} (4f^{14}) (5d^{9}) (6s^{1})

The second rule says that the electrons to the right are not shielding, but we are going to solve the exercise for the last level (6s), so we don't have electrons to the right.

For the third rule we have two considerations, if is ns or np and if is nd or nf:

For our case, we have an electro that is in ns, so the rule says that

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Now we can proceed with the calculation:

The first consideration in the third rule does not apply as we only have one electron on this level.

The second consideration will be as follow for the level 5, where we have 17 electrons.

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So the result for S=(60*1.00 + 17*0.85) = 74.45

And the equation is: Z* = 78 - 74.45

So Z* = 3.55

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