Chemistry, 22.07.2019 18:50 haileysmile2006

The specific heat of copper is 0.385 j/(g · °c). if 34.2 g of copper, initially at 24.0°c, absorbs 4.689 kj, what will be the final temperature of the copper?

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We know the relation between heat and temperature follows the formula: Q = Ce * m * (Tf-Ti) , where Q is heat transfer, Ce is specific heat, m is mass, Tf is final temperature and Ti is initial temperature. Note that heat value is given in kj so we need to change to joules, then as heat is absorbed the final temperature will increase. 4,689 = 0.385 * 34.2 * (Tf-24) Tf = 4,689 / (0.385 * 34.2) + 24 =380.12ÂşC

Answer from: quantraviousdavid

The final temperature of copper is $\boxed{{\text{380}}{\text{.117}}\;{{^\circ C}}}$

Further explanation:

The property is a unique feature of the substance that differentiates it from the other substances. It is classified into two types:

1. Intensive properties:

These are the properties that depend on the nature of the substance. These don't depend on the size of the system. Their values remain unaltered even if the system is further divided into a number of subsystems. Temperature, refractive index, concentration, pressure, and density are some of the examples of intensive properties.

2. Extensive properties:

These are the properties that depend on the amount of the substance. These are additive in nature when a single system is divided into many subsystems. Mass, enthalpy, volume, energy, size, weight, and length are some of the examples of extensive properties.

Specific heat is the amount of heat required to increase the temperature of any substance per unit mass. Specific heat capacity is also known as mass specific heat. Its SI unit is Joule (J).

The formula to calculate the heat energy of copper is as follows:

${\text{Q}}={mc\Delta T}}$ …… (1)

Here,

Q is the amount of heat transferred.

m is the mass of copper.

c is the specific heat of copper.

${\Delta T}}$ is the change in temperature of copper.

Rearrange equation (1) to calculate the temperature change.

${\Delta T}}=\frac{{\text{Q}}}{{{\text{mc}}}}$ …… (2)

The value of Q needs to be converted into J. The conversion factor for this is,

$1\;{\text{kJ}}={10^3}\;{\text{J}}$

So the value of Q can b calculated as follows:

$\begin{gathered}{\text{Q}}=\left({{\text{4}}{\text{.689 kJ}}}\right)\left({\frac{{{\text{1}}{{\text{0}}^3}{\text{ J}}}}{{{\text{1 kJ}}}}}\right)\\=4689\;{\text{J}}\\\end{gathered}$

The value of Q is 4689 J.

The value of m is 34.2 g.

The value of c is $0.385\;{\text{J/g}}\;{\text{^\circ C}}$ .

Substitute these values in equation (2).

$\begin{gathered}{\Delta T}}=\frac{{{\text{4689 J}}}}{{\left({{\text{34}}{\text{.2 g}}}\right)\left({0.385\;{\text{J/g}}\;{^\circ C}}}\right)}}\\=356.117\;^\circ{\text{C}}\\\end{gathered}$

The temperature change $\left({\Delta{\text{T}}}\right)$ can be calculated as follows:

${\Delta T}}={{\text{T}}_{\text{f}}}-{{\text{T}}_{\text{i}}}$ …… (3)

Here,

${\Delta T}}$ is the change in temperature.

${{\text{T}}_{\text{f}}}$ is the final temperature.

${{\text{T}}_{\text{i}}}$ is the initial temperature.

Rearrange equation (3) to calculate the final temperature.

${{\text{T}}_{\text{f}}}={\Delta T}}+{{\text{T}}_{\text{i}}}$ …… (4)

The value of ${{\text{T}}_{\text{i}}}$ is $24\;^\circ{\text{C}}$ .

The value of $\Delta {\text{T}}$ is $356.117\;^\circ{\text{C}}$

Substitute these values in equation (4).

$\begin{gathered}{{\text{T}}_{\text{f}}}=356.117\;^\circ{\text{C}}+24\;^\circ{\text{C}}\\=380.117\;^\circ{\text{C}}\\\end{gathered}$

So the final temperature of copper is ${380}}{\mathbf{.117}}\;{\mathbf{^\circ C}}$ .

Learn more:

1. What is the equilibrium constant of pure water at ?

2. Calculate the wavelength of the electron:

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Thermodynamics

Keywords: intensive, extensive, enthalpy, specific heat of copper, copper, m, Q, initial temperature, final temperature, change in temperature, mass of copper, amount of heat transferred and 380.117 degree celsius.

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The specific heat of copper is 0.385 j/(g · °c). if 34.2 g of copper, initially at 24.0°c, absorbs 4...

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