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zvonat [6]
3 years ago
5

4. The volume of a sample of a gas at STP is 200.0 ml. If the pressure is increased to 4.00 atmospheres (temperature constant),

what is the new volume?
Chemistry
1 answer:
Elina [12.6K]3 years ago
6 0

Answer : The value of new volume is, 50.0 mL

Explanation :

Boyle's Law : It is defined as the pressure of the gas is inversely proportional to the volume of the gas at constant temperature and number of moles.

P\propto \frac{1}{V}

or,

P_1V_1=P_2V_2

where,

P_1 = initial pressure at STP = 1 atm

P_2 = final pressure =  4.00  atm

V_1 = initial volume at STP = 200.0 mL

V_2 = final volume = ?

Now put all the given values in the above equation, we get:

1atm\times 200.0mL=4.00atm\times V_2

V_2=50.0mL

Therefore, the value of new volume is, 50.0 mL

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A sample of an ideal gas in a cylinder of volume 2.67 L at 298 K and 2.81 atm expands to 8.34 L by two different pathways. Path
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Since, we are not given the number of moles here. Therefore, we assume the number of moles, n = 1 mol.

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              R = 8.314 J/(K mol),          T = 298 K ,

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Now, putting the given values into the above formula as follows.

            W = -2.303 nRT log(\frac{V_2}{V_1})

   = -2.303 \times 1 \times 8.314 J/K mol \times 298 log(\frac{8.34}{2.67})

     = -2.303 \times 1 \times 8.314 J/K mol \times 298 \times 0.494

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Hence, work for path A is -2818.68 J.

  • For path B, the calculation will be as follows.

Step 1: When there is no change in volume then W = 0

Hence, for step 1, W = 0

Step 2: As, the gas is allowed to expand against constant external pressure P_{external} = 1.00 atm.

So,              W = -P_{external} \times \Delta V

Now, putting the given values into the above formula as follows.

               W = -P_{external} \times \Delta V

                   = -1 atm \times (8.34 L - 2.67 L)  

                    = -5.67 atm L

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Hence, work will be calculated as follows.

       W = -\frac{101.33 J}{1 atm L} \times 5.67 atm L

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Therefore, total work done by path B = 0 + (-574.54 J)

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Hence, work for path B is -574.54 J.

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Answer:

Explanation:

To find the density of nitrogen gas at STP which is standard temperature and pressure, certain parameters must be known.

The mass of the gas must be given or its volume.

Density  of a substance is the mass per unit area;

           Volume of gas at STP  = number of moles x 22.4

Using the volume obtained here,

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Then we can find the density.

The mass is very important.

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