How Much Energy Is Required To Melt 2 Kg Of Copper? Use The Table Below And The Equation: Q = M L Fusion Q = M L_{\text{fusion}} Q = M L Fusion ​ .$[ \begin{array}{|c|c|c|c|c|} \hline \text{Substance} & \text{Latent Heat Fusion (kJ/kg)} & \text{Melting Point} \

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Introduction

In this article, we will explore the concept of latent heat of fusion and its application in calculating the energy required to melt a given mass of a substance. We will use the equation Q=mLfusionQ = m L_{\text{fusion}} to determine the energy required to melt 2 kg of copper. We will also discuss the importance of latent heat of fusion in various fields, including chemistry and physics.

Latent Heat of Fusion

Latent heat of fusion is the amount of energy required to change the state of a substance from solid to liquid at its melting point. It is a measure of the energy required to break the bonds between the particles of a substance, allowing it to change its state. The latent heat of fusion is typically denoted by the symbol LfusionL_{\text{fusion}} and is usually expressed in units of joules per kilogram (J/kg) or kilojoules per kilogram (kJ/kg).

Table of Latent Heat of Fusion Values

The following table lists the latent heat of fusion values for various substances:

Substance Latent Heat Fusion (kJ/kg) Melting Point (°C)
Copper 205.4 1085
Water 334.7 0
Ice 334.7 0
Gold 63.1 1064
Silver 105.5 962
Lead 24.5 327

Calculating the Energy Required to Melt Copper

To calculate the energy required to melt 2 kg of copper, we can use the equation Q=mLfusionQ = m L_{\text{fusion}}. In this equation, QQ is the energy required to melt the substance, mm is the mass of the substance, and LfusionL_{\text{fusion}} is the latent heat of fusion of the substance.

Plugging in the values for copper, we get:

Q=2 kg×205.4 kJ/kg=410.8 kJQ = 2 \text{ kg} \times 205.4 \text{ kJ/kg} = 410.8 \text{ kJ}

Therefore, the energy required to melt 2 kg of copper is 410.8 kJ.

Importance of Latent Heat of Fusion

Latent heat of fusion is an important concept in various fields, including chemistry and physics. It is used to calculate the energy required to change the state of a substance, which is essential in many industrial processes, such as melting and solidification.

In chemistry, latent heat of fusion is used to calculate the energy required to melt a substance, which is essential in processes such as electrolysis and distillation. In physics, latent heat of fusion is used to calculate the energy required to change the state of a substance, which is essential in processes such as heat transfer and thermodynamics.

Conclusion

In conclusion, the energy required to melt 2 kg of copper is 410.8 kJ. This value can be calculated using the equation Q=mLfusionQ = m L_{\text{fusion}}, where QQ is the energy required to melt the substance, mm is the mass of the substance, and LfusionL_{\text{fusion}} is the latent heat of fusion of the substance.

Latent heat of fusion is an important concept in various fields, including chemistry and physics. It is used to calculate the energy required to change the state of a substance, which is essential in many industrial processes.

References

  • [1] CRC Handbook of Chemistry and Physics, 97th Edition, 2016.
  • [2] Latent Heat of Fusion, Encyclopedia Britannica, 2022.
  • [3] Thermodynamics, 2nd Edition, Cengage Learning, 2017.

Table of Latent Heat of Fusion Values (Expanded)

The following table lists the latent heat of fusion values for various substances:

Substance Latent Heat Fusion (kJ/kg) Melting Point (°C)
Copper 205.4 1085
Water 334.7 0
Ice 334.7 0
Gold 63.1 1064
Silver 105.5 962
Lead 24.5 327
Aluminum 334.7 660
Iron 270.6 1538
Zinc 113.8 419
Tin 59.7 231.9
Mercury 11.8 -38.8

Calculating the Energy Required to Melt Other Substances

Using the same equation Q=mLfusionQ = m L_{\text{fusion}}, we can calculate the energy required to melt other substances.

For example, to calculate the energy required to melt 1 kg of water, we can plug in the values for water:

Q=1 kg×334.7 kJ/kg=334.7 kJQ = 1 \text{ kg} \times 334.7 \text{ kJ/kg} = 334.7 \text{ kJ}

Therefore, the energy required to melt 1 kg of water is 334.7 kJ.

Similarly, to calculate the energy required to melt 2 kg of gold, we can plug in the values for gold:

Q=2 kg×63.1 kJ/kg=126.2 kJQ = 2 \text{ kg} \times 63.1 \text{ kJ/kg} = 126.2 \text{ kJ}

Therefore, the energy required to melt 2 kg of gold is 126.2 kJ.

Conclusion

In conclusion, the energy required to melt various substances can be calculated using the equation Q=mLfusionQ = m L_{\text{fusion}}. This equation is essential in various fields, including chemistry and physics, where it is used to calculate the energy required to change the state of a substance.

The latent heat of fusion values for various substances are listed in the table above. Using these values, we can calculate the energy required to melt other substances.

Future Work

In the future, we can explore other applications of latent heat of fusion, such as its use in thermodynamics and heat transfer. We can also investigate the effects of temperature and pressure on the latent heat of fusion of various substances.

References

  • [1] CRC Handbook of Chemistry and Physics, 97th Edition, 2016.
  • [2] Latent Heat of Fusion, Encyclopedia Britannica, 2022.
  • [3] Thermodynamics, 2nd Edition, Cengage Learning, 2017.
    Q&A: Latent Heat of Fusion =============================

Q: What is latent heat of fusion?

A: Latent heat of fusion is the amount of energy required to change the state of a substance from solid to liquid at its melting point. It is a measure of the energy required to break the bonds between the particles of a substance, allowing it to change its state.

Q: Why is latent heat of fusion important?

A: Latent heat of fusion is an important concept in various fields, including chemistry and physics. It is used to calculate the energy required to change the state of a substance, which is essential in many industrial processes, such as melting and solidification.

Q: How is latent heat of fusion calculated?

A: Latent heat of fusion is calculated using the equation Q=mLfusionQ = m L_{\text{fusion}}, where QQ is the energy required to melt the substance, mm is the mass of the substance, and LfusionL_{\text{fusion}} is the latent heat of fusion of the substance.

Q: What are some common applications of latent heat of fusion?

A: Some common applications of latent heat of fusion include:

  • Melting and solidification processes in industry
  • Thermodynamics and heat transfer
  • Energy storage and release
  • Phase transitions in materials science

Q: Can you give an example of how to calculate the energy required to melt a substance?

A: Yes, let's consider an example. Suppose we want to calculate the energy required to melt 2 kg of copper. We can use the equation Q=mLfusionQ = m L_{\text{fusion}}, where mm is the mass of the substance (2 kg) and LfusionL_{\text{fusion}} is the latent heat of fusion of copper (205.4 kJ/kg).

Plugging in the values, we get:

Q=2 kg×205.4 kJ/kg=410.8 kJQ = 2 \text{ kg} \times 205.4 \text{ kJ/kg} = 410.8 \text{ kJ}

Therefore, the energy required to melt 2 kg of copper is 410.8 kJ.

Q: What are some common substances that have high latent heat of fusion values?

A: Some common substances that have high latent heat of fusion values include:

  • Water: 334.7 kJ/kg
  • Ice: 334.7 kJ/kg
  • Copper: 205.4 kJ/kg
  • Gold: 63.1 kJ/kg

Q: What are some common substances that have low latent heat of fusion values?

A: Some common substances that have low latent heat of fusion values include:

  • Mercury: 11.8 kJ/kg
  • Tin: 59.7 kJ/kg
  • Lead: 24.5 kJ/kg

Q: Can you explain the difference between latent heat of fusion and specific heat capacity?

A: Yes, latent heat of fusion and specific heat capacity are two related but distinct concepts.

Latent heat of fusion is the energy required to change the state of a substance from solid to liquid at its melting point.

Specific heat capacity, on the other hand, is the energy required to change the temperature of a substance by a given amount.

For example, the specific heat capacity of water is 4.184 J/g°C, which means that it takes 4.184 J of energy to raise the temperature of 1 gram of water by 1°C.

Q: What are some common mistakes to avoid when working with latent heat of fusion?

A: Some common mistakes to avoid when working with latent heat of fusion include:

  • Confusing latent heat of fusion with specific heat capacity
  • Using the wrong units for latent heat of fusion (e.g. using J/kg instead of kJ/kg)
  • Failing to account for the mass of the substance when calculating the energy required to melt it

Q: Can you provide some resources for further learning on latent heat of fusion?

A: Yes, some resources for further learning on latent heat of fusion include:

  • CRC Handbook of Chemistry and Physics
  • Encyclopedia Britannica
  • Thermodynamics textbooks (e.g. Cengage Learning)
  • Online resources (e.g. Khan Academy, Physics Classroom)