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Oksi-84 [34.3K]

2 years ago

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1. A 250g chunk of metal is heated with 400 joules of energy and the temperature goes from 20 °C to 25°C. What is its specific h

eat ?
pls help me

1 answer:

Paha777 [63]2 years ago

5 0

The specific heat capacity of this chunk of metal is equal to 0.32 J/g°C.

<u>Given the following data:</u>

Mass of metal = 250g

Quantity of energy = 400 Joules

Initial temperature = 20°C

Final temperature = 20°C

To determine the specific heat capacity of this chunk of metal:

<h3>The formula for quantity of heat.</h3>

Mathematically, quantity of heat is given by the formula;

$Q = mc\theta$

<u>Where:</u>

Q represents the quantity of heat.

m represents the mass of an object.

c represents the specific heat capacity.

∅ represents the change in temperature.

Making c the subject of formula, we have:

$c = \frac{Q}{m\theta}$

Substituting the given parameters into the formula, we have;

$c = \frac{400}{250 \times (25-20)}\\\\c = \frac{400}{250 \times 5}\\\\c = \frac{400}{1250 }$

Specific heat, c = 0.32 J/g°C.

Read more on specific heat here: brainly.com/question/2834175

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Calculate the total energy, in kilojoules, that is needed to turn a 46 g block

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<u>Answer:</u> The amount of heat absorbed is 141.004 kJ.

<u>Explanation:</u>

In order to calculate the amount of heat released while converting given amount of steam (gaseous state) to ice (solid state), few processes are involved:

(1): $H_2O (s) (-25^oC, 248K) \rightleftharpoons H_2O(s) (0^oC,273K)$

(2): $H_2O (s) (0^oC, 273K) \rightleftharpoons H_2O(l) (0^oC,273K)$

(3): $H_2O (l) (0^oC, 273K) \rightleftharpoons H_2O(l) (100^oC,373K)$

(4): $H_2O (l) (100^oC, 373K) \rightleftharpoons H_2O(g) (100^oC,373K)$

Calculating the heat absorbed for the process having the same temperature:

$q=m\times \Delta H_{(f , v)}$ ......(i)

where,

q is the amount of heat absorbed, m is the mass of sample and $\Delta H_{(f , v)}$ is the enthalpy of fusion or vaporization

Calculating the heat released for the process having different temperature:

$q=m\times C_{s,l}\times (T_2-T_1)$ ......(ii)

where,

$C_{s,l}$ = specific heat of solid or liquid

$T_2\text{ and }T_1$ are final and initial temperatures respectively

<u>For process 1:</u>

We are given:

$m=46g\\C=2.108J/g^oC\\T_2=0^oC\\T_1=-25^oC$

Putting values in equation (i), we get:

$q_1=46g\times 2.108J/g^oC\times (0-(-25))\\\\q_1=2424.2J$

<u>For process 2:</u>

We are given:

$m=46g\\\Delta H_{fusion}=334J/g$

Putting values in equation (i), we get:

$q_2=46g\times 334J/g\\\\q_2=15364J$

<u>For process 3:</u>

We are given:

$m=46g\\C=4.186J/g^oC\\T_2=100^oC\\T_1=0^oC$

Putting values in equation (i), we get:

$q_3=46g\times 4.186J/g^oC\times (100-0)\\\\q_3=19255.6J$

<u>For process 4:</u>

We are given:

$m=46g\\\Delta H_{vap}=2260J/g$

Putting values in equation (i), we get:

$q_4=46g\times 2260J/g\\\\q_4=103960J$

Calculating the total amount of heat released:

$Q=q_1+q_2+q_3+q_4$

$Q=[(2424.2)+(15364)+(19255.6)+(103960)]$

$Q=141003.8J=141.004kJ$ (Conversion factor: 1 kJ = 1000J)

Hence, the amount of heat absorbed is 141.004 kJ.

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