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TEA [102]
3 years ago
12

A 2.81 μF capacitor is charged to 1220 V and a 6.61 μF capacitor is charged to 560 V. These capacitors are then disconnected fro

m their batteries, and the positive plates are now connected to each other and the negative plates are connected to each other. What will be the potential difference across each?
Physics
1 answer:
fenix001 [56]3 years ago
8 0

Answer:

756.88 Volts will be the potential difference across each capacitor.

Explanation:

Q=C\times V

Q = Charge on capacitor

C = Capacitance

V = Voltage across capacitor

Capacitance of first capacitor = C_1=2.81 \mu F=2.81\times 10^{-6} F

Charge of first capacitor = Q_1

Voltage across first capacitor = V_1=1220 V

Q_1=C_1V_1

Q_1=2.81\times 10^{-6} F\times 1220 V=0.0034282 C

Capacitance of first capacitor = C_2=6.61\mu F=6.61\times 10^{-6} F

Charge of second capacitor = Q_2

Voltage across first capacitor = V_2=560 V

Q_2=C_2V_2

Q_1=6.61\times 10^{-6} F\times 560 V=0.0037016 C

Both the capacitors are disconnected and positive plates are now connected to each other and the negative plates are connected to each other. These capacitors are connected in parallel combination.

Total charge = Q

Q =Q_1+Q_2=0.0034282 C+ 0.0037016 C=0.0071298 C

Total capacitance in parallel combination:

C_p=C_1+C_2=2.81\times 10^{-6} F+6.61\times 10^{-6} F=9.42\times 10^{-6} F

Potential across both capacitors = V

V=\frac{Q}{C}=\frac{0.0071298 C}{9.42\times 10^{-6} F}=756.88 V

756.88 Volts will be the potential difference across each capacitor.

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2 years ago
What quantity of heat is needed to convert 1 kg of ice at -13 degrees C to steam at 100 degrees C?
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Answer:

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Explanation:

We have

     heat of fusion of water = 334 J/g

     heat of vaporization of water = 2257 J/g

     specific heat of ice = 2.09 J/g·°C

     specific heat of water = 4.18 J/g·°C

     specific heat of steam = 2.09 J/g·°C

Here wee need to convert 1 kg ice from -13°C to vapor at 100°C

First the ice changes to -13°C from 0°C , then it changes to water, then its temperature increases from 0°C to 100°C, then it changes to steam.

Mass of water = 1000 g

Heat energy required to change ice temperature from -13°C to 0°C

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Heat energy required to change ice from 0°C to water at 0°C

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Heat energy required to change water temperature from 0°C to 100°C  

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Heat energy required to change water from 100°C to steam at 100°C  

          H₄ = mL = 1000 x 2257 = 2257 kJ    

Total heat energy required

          H = H₁ +  H₂ + H₃ + H₄ = 27.17 + 334 + 418 +2257 = 3036.17 kJ

Heat energy needed = 3036.17 kJ

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