Question

how much energy must be transferred to raise the temperature of a cup of coffee 250ml from 20.5 degree celsius to 95.6 degree Celsius.Assume that water and coffee has same density 1g per ml and specific heat capacity 4.148 j per g per k​

Answer 1

Answer:

77878.7calories

Explanation:

t1=20.5

y2=95.6

∆t=t2-t1

=95.6-20.5

=75.1

• ∆t is the temperature for the coffee to rise

• 1g per ml is given
• 250ml is given
• so
• Mass(m)=250
• c(specific heat capacity)=4.148..(given)

1. we know the formula of heat,

Q(heat)=mc∆t

=250 x 4.148 x 75.1

=77878.7 calories