Question

A 2.8 g sample of pure metal requires 10.1 J of energy to change its temperature from 21°C to 36°C. What is this metal? Substance Specific Heat Gold 0.129 J/g °C Silver 0.237 J/g °C Copper 0.385 J/g °C Water 4.18 J/g °C​

Answer 1

The specific heat of the metal can be determined by using the given specific heat values. By calculating the required energy for each metal, we find that the metal in question is most likely Copper.

Step-by-step explanation:

The specific heat of a substance is the amount of energy required to raise the temperature of 1 gram of the substance by 1°C. The metal in question requires 10.1 J of energy to change its temperature from 21°C to 36°C. By using the given specific heat values, we can calculate the specific heat of the metal. Let's calculate it for each metal given:

For Gold: 2.8g x 0.129 J/g °C x (36°C - 21°C) = 37.548 J

For Silver: 2.8g x 0.237 J/g °C x (36°C - 21°C) = 68.868 J

For Copper: 2.8g x 0.385 J/g °C x (36°C - 21°C) = 111.804 J

Based on our calculations, the metal with the closest value to the required energy is Copper with a specific heat of 0.385 J/g °C. Therefore, the metal in question is most likely Copper.

Answer 2

Silver 0.237 J/g °C

Step-by-step explanation:

We know that the heat required to raise the temperature of a given mass of a substance through a given temperature rise is given by;

H = mcθ

Where;

m = mass of the body

c = specific heat capacity of the body

θ = temperature rise

10.1 J = 2.8 g * c * (36°C - 21°C)

c = 10.1 J / 2.8 g * (36°C - 21°C)

c = 0.24 J/g °C