Question

A beaker contains 115 g of ethanol at 18.2°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°c

Answer 1

To find the final temperature of the ethanol after absorbing 1125 J of heat, we use the formula for heat transfer.

Step-by-step explanation:

To find the final temperature of the ethanol, we can use the formula for heat transfer:

`q = m * c * ΔT`

Where q is the heat transferred, m is the mass of the ethanol, c is the specific heat of ethanol, and ΔT is the change in temperature. Rearranging the formula, we can solve for the final temperature:

`ΔT = q / (m * c)`

Substituting the given values, we have:

`ΔT = 1125 J / (115 g * 2.46 J/g·°C)`

Calculating, we find that ΔT is approximately 4.92°C. To find the final temperature, we add ΔT to the initial temperature:

Final temperature = 18.2°C + 4.92°C

Therefore, the final temperature of the ethanol is approximately 23.12°C.