A 0.380 kg sample of aluminum (with a specific heat of 910.0 J/(kg x K)) is heated to 378 K and then placed in 2.40 kg of water that is at 293 K. If the system is left to reach its equilibrium state, what will the equilibrium temperature be? Assume that no thermal energy is lost to the external environment. Use 4.186 J/(g x K) as the specific heat of water.

The equilibrium temperature of the system is 276.494 Kelvin.

Explanation:

Let consider the system formed by the sample of aluminium and water as a control mass, in which the sample is cooled and water is heated until thermal equilibrium is reached. The energy process is represented by First Law of Thermodynamics:

Where:

- Heat received by water, measured in joules.

- Heat released by the sample of aluminium, measured in joules.

Given that no mass is evaporated, the previous expression is expanded to:

Where:

, - Mass of water and the sample of aluminium, measured in kilograms.

, - Specific heats of the sample of aluminium and water, measured in joules per kilogram-Kelvin.

, - Initial temperatures of the sample of aluminium and water, measured in Kelvin.

- Temperature which system reaches thermal equilibrium, measured in Kelvin.

The final temperature is now cleared:

Given that , , , , and , the final temperature of the system is:

The equilibrium temperature of the system is 276.494 Kelvin.

sorry idk the answer well to you i have a explaination

explanation: a formula which shows the arrangement of atoms in the molecule of a compound

the ratio of the conjugate base to the acid required to attain the desired ph.