A beaker contains 115 g of ethanol at 18.2^$\circ$C. If the ethanol absorbs 1125 J of heat without losing heat to the surroundings, what will be the final temperature of the ethanol The specific heat of ethanol is 2.46 J/g*^$\circ$C. A) 4.08^$\circ$C B) 14.1^$\circ$C C) 18.4^$\circ$C D) 22.2^$\circ$C E) 36.4^$\circ$C

Question

Quizplus · Accepted Answer

The heat absorbed (Q) is given by Q = mcΔT, where m is mass, c is specific heat, and ΔT is the change in temperature. Solving for ΔT gives ΔT = Q/(mc). Substituting the given values: ΔT = 1125 J / (115 g * 2.46 J/g°C) = 4°C. The final temperature is the initial temperature plus ΔT: 18.2°C + 4°C = 22.2°C.

A Beaker Contains 115 G of Ethanol at 18 ∘\circ∘ C If the Ethanol Absorbs 1125 J of Heat Without

A Beaker Contains 115 G of Ethanol at 18 $\circ$ C If the Ethanol Absorbs 1125 J of Heat Without