You burn a 1.5 g jellybean to warm 150 g of water. The temperature of the water increases by 15 °C. Water has a specific heat of 4.184 J/g • °C. How many joules does the jellybean have? A) 94.14 J B) 941.4 J C) 9414 J D) 14124 J

9414.0 J.

Explanation:

The amount of heat absorbed by water through burning a 1.5 g jellybean can be calculated from the relation:

Q = m. c.ΔT.

where, Q is the amount of heat absorbed by water,

m is the mass of water (m = 150.0 g),

c is the specific heat of water (c = 4.184 J/g °C),

ΔT is the temperature difference (final T - initial T) (ΔT = 15.0 °C).

∴ Q = m. c.ΔT = (150.0 g) (4.184 J/g °C) (15.0 °C) = 9414.0 J.

So, the jellybean have 9414.0 J that is releases to water.