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BigorU [14]
3 years ago
11

A sample of gas has a volume of 20.0 liters at 22.0° C. If the pressure remains constant, what is the volume at 100.0° C?

Chemistry
2 answers:
miv72 [106K]3 years ago
6 0
The problem applies Charles' law since constant pressure with varying volume and temperature are given. Assuming ideal gas law, the equation to be used is \frac{ V_{1} }{ T_{1} }=\frac{ V_{2} }{ T_{2} }. We make sure the temperatures are expressed in Kelvin, hence the given added with 273. The volume 2 is equal to 25.2881 liters.
padilas [110]3 years ago
4 0

Answer: The volume at 100.0^0C is 25.3 L

Explanation:

To calculate the final volume of the system, we use the equation given by Charles' Law. This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

\frac{V_1}{T_1}=\frac{V_2}{T_2}

where,

V_1\text{ and }T_1 are the initial volume and temperature of the gas.

V_2\text{ and }T_2 are the final volume and temperature of the gas.

We are given:

V_1=20.0L\\T_1=22.0^oC=(22.0+273)K=295.0K\\V_2=?\\T_2=100.0^oC=(100.0+273)K=373.0K

Putting values in above equation, we get:

\frac{20.0}{295.0K}=\frac{V_2}{373.0}\\\\V_2=25.3L

The volume at 100.0^0C is 25.3 L

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Note: Hope this helps, and I hope this is want it was asking. Good luck :)

8 0
3 years ago
In the PhET simulation window, click the radio button labeled Mystery in the Blocks menu on the right-hand side of the screen. U
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Answer:

B, D, E, C, A

Explanation:

We have 5 blocks with their respective masses and volumes.

Block            Mass            Volume

  A                65.14 kg       103.38 L

  B                0.64 kg         100.64 L

  C                4.08 kg         104.08 L

  D                3.10 kg          103.10 L

  E                 3.53 kg         101.00 L

The density (ρ) is an intensive property resulting from dividing the mass (m) by the volume (V), that is, ρ = m / V

ρA = 65.14 kg / 103.38 L = 0.6301 kg/L

ρB = 0.64 kg / 100.64 L = 0.0064 kg/L

ρC = 4.08 kg / 104.08 L = 0.0392 kg/L

ρD = 3.10 kg / 103.10 L = 0.0301 kg/L

ρE = 3.53 kg / 101.00 L = 0.0350 kg/L

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4 0
3 years ago
Fill in the left side of this equilibrium constant equation for the reaction of benzoic acid (HC_6H_5CO_2) with water.
il63 [147K]

Answer:

[C₆H₅COO⁻][H₃O⁺]/[C₆H₅COOH] = Ka

Explanation:

The reaction of dissociation of the benzoic acid in water is given by the following equation:

C₆H₅-COOH + H₂O  ⇄  C₆H₅-COO⁻  +  H₃O⁺    (1)

The dissociation constant of an acid is the measure of the strength of an acid:

HA ⇄ A⁻ + H⁺        (2)

K_{a} = \frac{[A^{-}][H^{+}]}{[HA]}      (3)

<em>Where the dissociation constant of the acid (Ka) is equal to the ratio of the concentration of the dissociated forms of the acid, [A⁻][H⁺], and the concentration of the acid, [HA].     </em>

So, starting from the equations (2) and (3), the constant equation for the dissociation reaction of benzoic acid in water, of the equation (1), is:

K_{a} = \frac{[C_{6}H_{5}COO^{-}][H_{3}O^{+}]}{[C_{6}H_{5}COOH]}

I hope it helps you!          

6 0
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Dvinal [7]

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Learn more:

hydrogen bond brainly.com/question/12408823

#learnwithBrainly

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