A 4.50-g sample of liquid water at 25.0 °C is heated by the addition of 133 J of energy.The final temperature of the water is ________ °C.The specific heat capacity of liquid water is
A)149
B)25.1
C)-17.9
D)32.1
E)7.07

Question

A 4.50-g sample of liquid water at 25.0 °C is heated by the addition of 133 J of energy.The final temperature of the water is ________ °C.The specific heat capacity of liquid water is 
A)149 
B)25.1 
C)-17.9 
D)32.1 
E)7.07

Quizplus · Accepted Answer

We can use the formula:

q = mcΔT

where q is the amount of heat absorbed by the water, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature.

We are given q = 133 J, m = 4.50 g, c = 4.18 J/g·°C (specific heat capacity of water), and the initial temperature is 25.0 °C.

Plugging in these values, we can solve for ΔT:

133 J = (4.50 g)(4.18 J/g·°C)ΔT

ΔT = 7.07 °C

Therefore, the final temperature of the water is:

25.0 °C + 7.07 °C = 32.1 °C

So the correct answer is D) 32.1.

A 450-G Sample of Liquid Water at 25