Verified answer

In order to know, we must determine the final temperature. Answer a and c could be eliminated initially since decomposition is not possible at this conditions and the temperature is higher than 0C for water to be frozen.

Let assume the conditions is at atmospheric pressure and the specific heat of water is 4.184 J/g C

Heat added = 5 kJ = 5000 J

Heat absorbed by water = mass x specific heat x temperature difference = 15.5 x 4.184 x (T - 10)

Solve for T = 87 C. So the water is still a liquid since it is below the boiling temperature of 100 C.

You know that energy released = energy absorbed = m x delta T x heat capacity

So delta T = energy / m x Heat Capacity

= 5 x 10^3 / (15.5 x 4.18 ). Ie . 4.18 is heat capacity

For water

So delta T = 77.17 c

Tf - Ti = 77.17

Tf = 87 C

So the water is still liquid. E. Is the correct answer

I'm no expert, but I think it's [e. still a liquid] because you know at 10C, water is a liquid. At 100C, it is boiling. I calculated the amount of energy it would take to boil that much water:

H= 4.18J/g*15.5g*90C(how many degrees it needs to rise to get to 100C)

H=5813J

Since you're only applying 5000J, water is not boiling, far from vaporized, wasn't solid to begin with, and not decomposed. So it is still liquid water.

Hope I helped!