Question

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

Answer 1

Answer : The heat required is 1160 J.

Explanation :

Formula used :

$Q=m\times c\times \Delta T$

or,

$Q=m\times c\times (T_2-T_1)$

where,

Q = heat required = ?

m = mass of iron = 100.0 g

c = specific heat of iron = $0.46J/g^oC$

$T_1$ = initial temperature  = $15.0^oC$

$T_2$ = final temperature  = $40.2^oC$

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

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

$Q=1159.2J\approx 1160J$

Therefore, the heat required is 1160 J.

Answer 2

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.