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sergey [27]
3 years ago
8

An inventor claims to have developed a resistance heater that supplies 1.2 kWh of energy to a room for each kWh of electricity i

t consumes. Is this a reasonable claim, or is it true that the inventor has developed a perpetual-motion machine
Physics
1 answer:
mixas84 [53]3 years ago
3 0

Answer:

if we are to go by the first law of thermodynamics, the Inventors claims are not reasonable.

The inventor has developed a perpetual-motion machine { any device that violates the first law of thermodynamics}

Explanation:

Given that;

energy supplied to a room Qh= 1.2 kWh

for each for each kWh of electricity it consumes, i.e work input W = 1 kWh

W know that; the first law of thermodynamics says energy can neither be created nor destroyed but can flow from one body to another;

which means ∑Q should or must be equal to ∑W;  ∑Q = ∑W

but in the given system; Qh⇒1.2 kWh is NOT equal to W⇒1 kWh

i.e Qh⇒1.2 kWh ≠ W⇒1 kWh

which simply means his device create energy and that violate the first law of thermodynamics.

Therefore, if we are to go by the first law of thermodynamics, the Inventors claims are not reasonable.

The inventor has developed a perpetual-motion machine { any device that violates the first law of thermodynamics}

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Explanation:

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How much heat is needed to raise the temperature of 50.0 g of water by 25.0°C
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Answer:

Explanation:

In order to be able to solve this problem, you will need to know the value of water's specific heat, which is listed as

c

=

4.18

J

g

∘

C

Now, let's assume that you don't know the equation that allows you to plug in your values and find how much heat would be needed to heat that much water by that many degrees Celsius.

Take a look at the specific heat of water. As you know, a substance's specific heat tells you how much heat is needed in order to increase the temperature of

1 g

of that substance by

1

∘

C

.

In water's case, you need to provide

4.18 J

of heat per gram of water to increase its temperature by

1

∘

C

.

What if you wanted to increase the temperature of

1 g

of water by

2

∘

C

? You'd need to provide it with

increase by 1

∘

C



4.18 J

+

increase by 1

∘

C



4.18 J

=

increase by 2

∘

C



2

×

4.18 J

To increase the temperature of

1 g

of water by

n

∘

C

, you'd need to supply it with

increase by 1

∘

C



4.18 J

+

increase by 1

∘

C



4.18 J

+

...

=

increase by n

∘

C



n

×

4.18 J

Now let's say that you wanted to cause a

1

∘

C

increase in a

2-g

sample of water. You'd need to provide it with

for 1 g of water



4.18 J

+

for 1 g of water



4.18 J

=

for 2 g of water



2

×

4.18 J

To cause a

1

∘

C

increase in the temperature of

m

grams of water, you'd need to supply it with

for 1 g of water



4.18 J

+

for 1 g of water



4.18 J

+

,,,

=

for m g of water



m

×

4.18 J

This means that in order to increase the temperature of

m

grams of water by

n

∘

C

, you need to provide it with

heat

=

m

×

n

×

specific heat

This will account for increasing the temperature of the first gram of the sample by

n

∘

C

, of the the second gram by

n

∘

C

, of the third gram by

n

∘

C

, and so on until you reach

m

grams of water.

And there you have it. The equation that describes all this will thus be

q

=

m

⋅

c

⋅

Δ

T

, where

q

- heat absorbed

m

- the mass of the sample

c

- the specific heat of the substance

Δ

T

- the change in temperature, defined as final temperature minus initial temperature

In your case, you will have

q

=

100.0

g

⋅

4.18

J

g

∘

C

⋅

(

50.0

−

25.0

)

∘

C

q

=

10,450 J

Rounded to three sig figs and expressed in kilojoules, t

Explanation:

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