Respuesta :
The final temperature after absorbing the energy of 990 J is 25.014 °C.
Explanation:
The specific heat capacity formula can be used to solve the given problem.
So here the heat absorbed or the Q value is given as 990 J. Then the mass of the sample of water m is given as 59 g. The initial temperature is said to be 21 °C and the final temperature has to be determined.
The specific heat capacity is given as 4.18 J/g°C.
Then, [tex]Q = m*c* del T[/tex]
So, the difference in temperature or the change in temperature has to be determined first.
[tex]del T = \frac{Q}{mc} = \frac{990}{59*4.18} = \frac{990}{246.62} \\\\del T =4.014[/tex]
So, the change in temperature = ΔT = T₂-T₁ = 4.014 °C
T₂-21 = 4.014
T₂ = 4.014+21 = 25.014 °C.
So, the final temperature after absorbing the energy of 990 J is 25.014 °C.
25 degrees celsius will be the final temperature of this sample be after absorbing this energy
Explanation:
data given:
q (heat absorbed) = 990 J
m (mass) = 59 gram
T2 (final temperature) = ?
c (specific heat capacity of water) = 4.18 J/g °C).
T1 (initial temperature) = 21
ΔT = T2 -T1
applying the formula for heat absorbed
q = mcΔT
putting the values in the equation
ΔT = [tex]\frac{q}{mc}[/tex]
T2 - 21 = [tex]\frac{990}{59 X4.18}[/tex]
T2 -21 = 4.01
T2 = 4.01 + 21
= 25.01 degrees
The final temperature of water sample is 25 degrees when initial temperature was 21 degrees and heat absorbed was 900 J
