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harina [27]
3 years ago
9

When the volume of a gas is changed from 11.5 cm3 to ?cm the temperature will change from 415 K to 200 K

Chemistry
1 answer:
Sonja [21]3 years ago
4 0

Assuming that the gas acts like an ideal gas, we can calculate for the final volume using the ideal gas law:

PV = nRT

Where P = pressure, V = volume, n = number of moles, R = gas constant, and T = temperature

Assuming that P, n, and R are constant throughout the process, we can define another constant K:

V / T = K               where K = nR / P

Equating the initial and final states:

Vi / Ti = Vf / Tf

Substituting the given values:

11.5 cm^3 / 415 K = Vf / 200 K

Vf = 5.54 cm^3

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neonofarm [45]
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5 0
3 years ago
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Determine the pH of a solution of 0.00278 M of HClO4. Report the answer to two digits past the decimal.
aleksandrvk [35]

Answer:

The pH of a solution of 0.00278 M of HClO₄ is 2.56

Explanation:

pH is a measure of acidity or alkalinity that indicates the amount of hydrogen ions present in a solution or substance and is calculated as:

pH= - log [H⁺]= - log [H₃O⁺]

On the other hand , a Strong Acid is that acid that in an aqueous solution dissociates completely. In other words, a strong acid completely dissociates into hydrogen ions and anions in solution.

HClO₄ is a strong acid, so in aqueous solution it will be  totally dissociated. Then, the concentration of protons is equal to the initial concentration of  acid and the pH will be calculated:

pH= - log 0.00278

pH= 2.56

<u><em>The pH of a solution of 0.00278 M of HClO₄ is 2.56</em></u>

8 0
3 years ago
Which element has the same number of valence electrons as hydrogen (H)? A. helium (He). . B. oxygen (O). . C. nitrogen (N). . D.
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7 0
2 years ago
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If an ice cube weighing 25.0 g with an initial
riadik2000 [5.3K]

Answer:

11

∘

C

Explanation:

As far as solving this problem goes, it is very important that you do not forget to account for the phase change underwent by the solid water at

0

∘

C

to liquid at

0

∘

C

.

The heat needed to melt the solid at its melting point will come from the warmer water sample. This means that you have

q

1

+

q

2

=

−

q

3

(

1

)

, where

q

1

- the heat absorbed by the solid at

0

∘

C

q

2

- the heat absorbed by the liquid at

0

∘

C

q

3

- the heat lost by the warmer water sample

The two equations that you will use are

q

=

m

⋅

c

⋅

Δ

T

, where

q

- heat absorbed/lost

m

- the mass of the sample

c

- the specific heat of water, equal to

4.18

J

g

∘

C

Δ

T

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

and

q

=

n

⋅

Δ

H

fus

, where

q

- heat absorbed

n

- the number of moles of water

Δ

H

fus

- the molar heat of fusion of water, equal to

6.01 kJ/mol

Use water's molar mass to find how many moles of water you have in the

100.0-g

sample

100.0

g

⋅

1 mole H

2

O

18.015

g

=

5.551 moles H

2

O

So, how much heat is needed to allow the sample to go from solid at

0

∘

C

to liquid at

0

∘

C

?

q

1

=

5.551

moles

⋅

6.01

kJ

mole

=

33.36 kJ

This means that equation

(

1

)

becomes

33.36 kJ

+

q

2

=

−

q

3

The minus sign for

q

3

is used because heat lost carries a negative sign.

So, if

T

f

is the final temperature of the water, you can say that

33.36 kJ

+

m

sample

⋅

c

⋅

Δ

T

sample

=

−

m

water

⋅

c

⋅

Δ

T

water

More specifically, you have

33.36 kJ

+

100.0

g

⋅

4.18

J

g

∘

C

⋅

(

T

f

−

0

)

∘

C

=

−

650

g

⋅

4.18

J

g

∘

C

⋅

(

T

f

−

25

)

∘

C

33.36 kJ

+

418 J

⋅

(

T

f

−

0

)

=

−

2717 J

⋅

(

T

f

−

25

)

Convert the joules to kilojoules to get

33.36

kJ

+

0.418

kJ

⋅

T

f

=

−

2.717

kJ

⋅

(

T

f

−

25

)

This is equivalent to

0.418

⋅

T

f

+

2.717

⋅

T

f

=

67.925

−

33.36

T

f

=

34.565

0.418

+

2.717

=

11.026

∘

C

Rounded to two sig figs, the number of sig figs you have for the mass of warmer water, the answer will be

T

f

=

11

∘

C

Explanation:

3 0
2 years ago
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