A hot lump of 31.9 g of copper at an initial temperature of 50.0 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to

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Question:

A hot lump of 31.9 g of copper at an initial temperature of 50.0 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(g·°C)? Assume no heat is lost to surroundings.

Answers

the earth would become to overheated and everything alive on it will eventually die from overheating. plants will eventually die as well, water will evaporate, and it will be nothing but a hot planet without anything living on it.

High-energy and unstable.

Answer(false);

As long as you're breathing, you'll be fine : /p. s. if you aren't breathing, you'll pass out. mark as brainliest.

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