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nikklg [1K]
2 years ago
8

What is the specific heat capacity of an unknown metal if 75.00 g of the metal absorbs 418.6J of heat and the temperature rises

25.0°C?
Chemistry
1 answer:
EleoNora [17]2 years ago
3 0

Answer:

The specific heat capacity of the unknown metal is 0.223 \frac{J}{g*C}

Explanation:

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

There is a direct proportional relationship between heat and temperature. The constant of proportionality depends on the substance that constitutes the body as on its mass, and is the product of the specific heat by the mass of the body. So, the equation that allows calculating heat exchanges is:

Q = c * m * ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

In this case, you know:

  • Q= 418.6 J
  • c= ?  
  • m= 75 g
  • ΔT= 25 C

Replacing:

418.6 J= c* 75 g* 25 C

Solving:

c=\frac{418.6 J}{75 g*25 C}

c= 0.223 \frac{J}{g*C}

<u><em>The specific heat capacity of the unknown metal is 0.223 </em></u>\frac{J}{g*C}<u><em></em></u>

<u><em> </em></u>

<u><em></em></u>

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Step 1:

The balanced equation for the reaction. This is given below:

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Step 2:

Data obtained from the question. This includes the following:

Volume (V) of Cl2 obtained = 235mL

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Pressure (P) = 805 Torr

Step 3:

Conversion to appropriate unit.

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Temperature (Kelvin) = 25°C + 273 = 298K

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760 Torr = 1 atm

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Determination of the number of mole of Cl2 produced. This is illustrated below:

The number of mole (n) of Cl2 produced can be obtained by using the ideal gas equation as follow:

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Step 5:

Determination of the number of mole MnO2 that produce 0.01 mole of Cl2. This is illustrated below:

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From the balanced equation above,

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Number of mole MnO2 = 0.01 mole

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Mass of MnO2 = 0.01 x 87

Mass of MnO2 = 0.87g

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