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You put a bottle of soft drink in a refrigerator and leave it until its temperature has dropped 10.0 K. What is its temperature change in (a) F\(^\circ\) and (b) C\(^\circ\)?

Short Answer

Expert verified
10.0 K equals 10.0 C° and 18.0 F° temperature change.

Step by step solution

01

Understand the Problem

The problem provides a temperature change in Kelvin (10.0 K) and asks us to convert this change to Fahrenheit and Celsius.
02

Convert Kelvin Change to Celsius Change

Since a change of 1 Kelvin is equivalent to a change of 1 degree Celsius, a temperature change of 10.0 K is equal to a change of 10.0 °C.
03

Convert Celsius Change to Fahrenheit Change

Use the conversion formula for temperature differences: \( \Delta T_{°F} = \Delta T_{°C} \times \frac{9}{5} \). Substitute \( \Delta T_{°C} = 10.0 \) to get \( \Delta T_{°F} = 10.0 \times \frac{9}{5} = 18.0 \).
04

Conclusion

The temperature change in Fahrenheit is 18.0 F° and in Celsius is 10.0 C°.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Kelvin to Celsius
The Kelvin and Celsius scales are two fundamental ways to measure temperature. A remarkable feature of these two scales is how closely they relate to each other.
To convert a temperature difference from Kelvin to Celsius, there is actually nothing complex about it. This is because both scales increase at the same rate.
  • 1 degree Celsius is exactly equal to 1 Kelvin when it comes to a temperature change.
This means that if an object experiences a temperature change of 10.0 Kelvin, its change in degrees Celsius would also be 10.0 C°.
This direct equivalence makes calculations between Kelvin and Celsius very straightforward. There's no need to add or subtract any constant—just a simple 1-to-1 conversion!
Celsius to Fahrenheit
Sometimes, you need to express Celsius in Fahrenheit, especially in places where Fahrenheit is commonly used.
When dealing with temperature changes, the scale conversion requires a little formulaic adjustment.To convert a temperature difference from Celsius to Fahrenheit, use the formula:\[ \Delta T_{°F} = \Delta T_{°C} \times \frac{9}{5} \]This equation scales the Celsius change into Fahrenheit.
For example, if a temperature change is 10.0 °C, then:
  • Plug into the formula: \(\Delta T_{°F} = 10.0 \times \frac{9}{5} = 18.0\)
  • The temperature change is 18.0 Fahrenheit degrees (F°).
This conversion is essential for countless scientific, engineering, and everyday practical applications, ensuring everyone can understand and communicate temperature changes efficiently.
Temperature Change
Temperature change refers to how much the temperature of an object or substance increases or decreases.
This is an essential concept in physics and everyday life because it affects how substances react or behave.Here are a few things to note about temperature changes:
  • Temperature change can occur in various scales such as Kelvin, Celsius, or Fahrenheit.
  • It is represented by the symbol \(\Delta T\), where \(\Delta\) signifies change.
  • It's crucial for understanding environmental shifts, chemical reactions, and physical transformations.
Whether you're chilling a beverage or studying thermodynamics, knowing how to properly calculate and express temperature changes helps you grasp the broader implications of heat transfer and energy conversion.

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Most popular questions from this chapter

You are given a sample of metal and asked to determine its specific heat. You weigh the sample and find that its weight is 28.4 N. You carefully add \(1.25 \times 10{^4}\) J of heat energy to the sample and find that its temperature rises 18.0 C\(^\circ\). What is the sample's specific heat?

In a container of negligible mass, 0.0400 kg of steam at 100\(^\circ\)C and atmospheric pressure is added to 0.200 kg of water at 50.0\(^\circ\)C. (a) If no heat is lost to the surroundings, what is the final temperature of the system? (b) At the final temperature, how many kilograms are there of steam and how many of liquid water?

A copper calorimeter can with mass 0.100 kg contains 0.160 kg of water and 0.0180 kg of ice in thermal equilibrium at atmospheric pressure. If 0.750 kg of lead at 255\(^\circ\)C is dropped into the calorimeter can, what is the final temperature? Assume that no heat is lost to the surroundings.

A 500.0-g chunk of an unknown metal, which has been in boiling water for several minutes, is quickly dropped into an insulating Styrofoam beaker containing 1.00 kg of water at room temperature (20.0\(^\circ\)C). After waiting and gently stirring for 5.00 minutes, you observe that the water’s temperature has reached a constant value of 22.0\(^\circ\)C. (a) Assuming that the Styrofoam absorbs a negligibly small amount of heat and that no heat was lost to the surroundings, what is the specific heat of the metal? (b) Which is more useful for storing thermal energy: this metal or an equal weight of water? Explain. (c) If the heat absorbed by the Styrofoam actually is not negligible, how would the specific heat you calculated in part (a) be in error? Would it be too large, too small, or still correct? Explain.

At a chemical plant where you are an engineer, a tank contains an unknown liquid. You must determine the liquid's specific heat capacity. You put 0.500 kg of the liquid into an insulated metal cup of mass 0.200 kg. Initially the liquid and cup are at 20.0\(^\circ\)C. You add 0.500 kg of water that has a temperature of 80.0\(^\circ\)C. After thermal equilibrium has been reached, the final temperature of the two liquids and the cup is 58.1\(^\circ\)C. You then empty the cup and repeat the experiment with the same initial temperatures, but this time with 1.00 kg of the unknown liquid. The final temperature is 49.3\(^\circ\)C. Assume that the specific heat capacities are constant over the temperature range of the experiment and that no heat is lost to the surroundings. Calculate the specific heat capacity of the liquid and of the metal from which the cup is made.

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