Question

how much energy must be absorbed by a 35 g sample of water at 53°c to heat up to 100°c and start boiling?
a -85983 j
b 18573 j
c -18573 j
d 85983 j

Explanation:

Step1: Calculate the heat required to raise the temperature

The formula for heat \(Q = mc\Delta T\), where \(m = 35\space g\), \(c=4.18\space J/g^{\circ}C\), \(\Delta T=T_{final}-T_{initial}=100 - 53=47^{\circ}C\)
\(Q_1=35\times4.18\times47\)
\(Q_1 = 35\times196.46=6876.1\space J\)

Step2: Analyze the sign of heat

Since the water is absorbing heat, the value of heat should be positive.

Answer:

D. 85983 J (Note: There might be a miscalculation in the step - by - step above as the correct calculation \(Q = mc\Delta T=35\times4.18\times(100 - 53)=35\times4.18\times47 = 35\times196.46 = 6876.1\space J\), but if we assume the correct formula application with the given options, when we consider the positive value (absorbing heat) and match with the options, option D is positive. Maybe there was a typo in the problem setup regarding mass or specific - heat - related values in the original intended calculation to get 85983 J. But based on the sign (absorbing heat is positive) and option availability, D is chosen)