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3 years ago

Consider the following chemical reaction.

Chemistry

1 answer:

Ede4ka [16]3 years ago

5 0

The concentration of the zinc acetate, Zn(C₂H₃O₂) solution is 1.067 M

We'll begin by calculating the number of mole in 20.5 g of Zn(C₂H₃O₂)₂

Mass of Zn(C₂H₃O₂)₂ = 20.5 g

Molar mass of Zn(C₂H₃O₂)₂ = 65 + 2[(12×2) + (3×1) + (16×2)]

= 65 + 2[59]

= 183 g/mol

Mole = mass / molar mass

Mole of Zn(C₂H₃O₂)₂ = 20.5 / 183

Finally, we shall determine concentration of Zn(C₂H₃O₂). This can be obtained as follow:

Mole of Zn(C₂H₃O₂)₂ = 0.112 mole

Volume = 105 mL = 105 / 1000 = 0.105 L

<h3>Concentration of Zn(C₂H₃O₂)₂ =? </h3>

Concentration = mole / Volume

Concentration of Zn(C₂H₃O₂)₂ = 0.112 / 0.105

<h3>Concentration of Zn(C₂H₃O₂)₂ = 1.067 M</h3>

Therefore, the concentration of the zinc acetate, Zn(C₂H₃O₂) solution is 1.067 M

Learn more: brainly.com/question/25511880

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How much heat will be absorbed by a 26.3 g piece of aluminum (specific heat = 0.930 J/g･°C) as it changes temperature from 23.0°

kotykmax [81]

Answer:

$\boxed {\boxed {\sf 1076.196 \ Joules}}$

Explanation:

Since we are given the mass, specific heat, and temperature, we should use the following formula for heat energy.

$q=mc\Delta T$

The mass of the aluminum is 26.3 grams. Its specific heat is 0.930 Joules per gram degree Celsius. We need to find the change in temperature.

The change in temperature is the difference between the initial temperature to the final temperature.
The temperature changes <em>from</em> 23.0°C <em>to</em> 67.0°C, so the initial is 23 degrees and the final is 67 degrees.
ΔT= final temperature - initial temperature
ΔT= 67°C - 23°C
ΔT= 44°C

Now we know all the values.

m= 26.3 g
c= 0.930 J/g °C
ΔT= 44°C

Substitute the values into the formula.

$q= (26.3 \ g}) \times (0.930 \ J/g \textdegree C) \times (44 \textdegree C)$

Multiply the first two numbers together. The units of grams cancel.

$q= 24.459 \ J/ \textdegree C \times 44 \textdegree C$

Multiply again. This time, the units of degrees Celsius cancel.

$q=1076.196 \ J$

<u>1076.196 Joules</u> of heat will be absorbed by the piece of aluminum.

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Well, human bodies differ from all those animals.

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4 years ago

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Define saturated and unsaturated fats

pav-90 [236]

Answer:

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Explanation:

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A 25.0 g bold made of an alloy absorbed 250 J of heat as its temperature changed from 25.0 °C to 78.0 °C. What is the specific h

nata0808 [166]

Answer:

Specific heat of alloy = 0.2 j/ g.°C

Explanation:

Specific heat capacity:

It is the amount of heat required to raise the temperature of one gram of substance by one degree.

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

Given data:

Mass of bold = 25 g

Heat absorbed = 250 J

Initial Temperature = 25°C

Final temperature = 78°C

Specific heat of alloy = ?

Solution:

Change in temperature:

ΔT = 78°C - 25°C

ΔT = 53°C

Now we will put the values in formula.

Q = m.c. ΔT

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250 j = 1325 g.°C × c

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alexdok [17]

<h3>Explanation;</h3>

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