Respuesta :
Q=MCdeltaT
*make sure you change celcius into Kelvin*
Q=20(4.18)(20)
Q=1,672
It requires 1,672 Joules
*make sure you change celcius into Kelvin*
Q=20(4.18)(20)
Q=1,672
It requires 1,672 Joules
Answer : The amount of heat required is, 1672 J
Solution :
Formula used :
[tex]Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})[/tex]
where,
Q = heat required = ?
m = mass of water = 20 g
c = specific heat of water = [tex]4.18J/g^oC[/tex]
[tex]\Delta T=\text{Change in temperature}[/tex]
[tex]T_{final}[/tex] = final temperature = [tex]30^oC[/tex]
[tex]T_{initial}[/tex] = initial temperature = [tex]10^oC[/tex]
Now put all the given values in the above formula, we get the amount of heat required.
[tex]Q=20g\times 4.18J/g^oC\times (30-10)^oC[/tex]
[tex]Q=1672J[/tex]
Therefore, the amount of heat required is, 1672 J
