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How much heat is required to increase the temperature of 100.0 grams of iron from 15.0oC to 40.2oC? (The specific heat of iron is 0.46 J/g xoC) 2520 J 46 J 1160 J 1850 J 690 J

Respuesta :

Dejanras
Answer is: 1160 J of heat Is required to increase the temperature.
m(Fe) = 100 g.
∆T = 40,2 - 15 = 25,2°C.
C(Fe) = 0,46 J/g•°C.
Q = m(Fe) • C • ∆T.
Q = 100 g • 0,46 J/g•°C • 25,2°C
Q = 1160 J.
C - specific heat.

Answer : The heat required is 1160 J.

Explanation :

Formula used :

[tex]Q=m\times c\times \Delta T[/tex]

or,

[tex]Q=m\times c\times (T_2-T_1)[/tex]

where,

Q = heat required = ?

m = mass of iron = 100.0 g

c = specific heat of iron = [tex]0.46J/g^oC[/tex]

[tex]T_1[/tex] = initial temperature  = [tex]15.0^oC[/tex]

[tex]T_2[/tex] = final temperature  = [tex]40.2^oC[/tex]

Now put all the given value in the above formula, we get:

[tex]Q=100.0g\times 0.46J/g^oC\times (40.2-15.0)^oC[/tex]

[tex]Q=1159.2J\approx 1160J[/tex]

Therefore, the heat required is 1160 J.

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