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, we can use the formula q = m * c * ΔT, where q is the heat absorbed by the ethanol, m is the mass of the ethanol, c is the specific heat of ethanol, and ΔT is the change in temperature. By substituting the given values and rearranging the formula, we can find that the final temperature of the ethanol will be approximately 22.88 °C.

Step-by-step explanation:

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

q = m * c * ΔT

Where:

• q is the heat absorbed by the ethanol
• m is the mass of the ethanol
• c is the specific heat of ethanol
• ΔT is the change in temperature

Substituting the given values:

• q = 1125 J
• m = 115 g
• c = 2.46 J/g×°C

Now we can rearrange the formula to solve for ΔT:

ΔT = q / (m * c)

Plugging in the values:

• ΔT = 1125 J / (115 g * 2.46 J/g×°C)

Simplifying the equation gives us:

• ΔT ≈ 4.68 °C

Therefore, the final temperature of the ethanol will be approximately 18.2 °C + 4.68 °C = 22.88 °C.