/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 2 You are sick, and your temperatu... [FREE SOLUTION] | 91Ó°ÊÓ

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You are sick, and your temperature is 312.0 kelvins. Convert this temperature to the Fahrenheit scale.

Short Answer

Expert verified
The temperature is approximately 101.93°F.

Step by step solution

01

Understand the Conversion Formula

To convert Kelvin to Fahrenheit, you need to use the conversion formula: \( F = \frac{9}{5}(K - 273.15) + 32 \). Where \( K \) is the temperature in Kelvin and \( F \) is the temperature in Fahrenheit.
02

Substitute the Kelvin Temperature

Substitute the given temperature in Kelvin into the formula. Here, \( K = 312.0 \). The equation becomes: \( F = \frac{9}{5}(312.0 - 273.15) + 32 \).
03

Calculate the Conversion

First, perform the operation inside the parentheses: \( 312.0 - 273.15 = 38.85 \). Then, multiply by \( \frac{9}{5} \), which gives \( \frac{9}{5} \times 38.85 = 69.93 \).
04

Final Calculation

Add 32 to the result from Step 3 to complete the conversion: \( 69.93 + 32 = 101.93 \).
05

State the Result

The temperature in Fahrenheit is approximately 101.93°F.

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Key Concepts

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

Kelvin to Fahrenheit formula
To convert temperatures from Kelvin to Fahrenheit, you need to understand the conversion formula that directly relates these two different temperature scales. The key formula is:\[F = \frac{9}{5}(K - 273.15) + 32\]In this formula, \(K\) represents the temperature in Kelvin, and \(F\) stands for the temperature in Fahrenheit. The formula might look a bit tricky, but it simply includes a subtraction, a division, some multiplication, and an addition. These steps align the Kelvin scale, which starts at absolute zero, with the Fahrenheit scale. This formula is crucial as it helps you accurately convert temperatures from the international scientific and engineering standard (Kelvin) to a more commonly used household scale (Fahrenheit).
Keeping this formula handy can save you time when performing temperature conversions.
Step-by-step calculation
Converting temperatures step-by-step helps you understand each part of the formula while practicing essential math skills.
Let’s break down each step of our example problem where we convert 312.0 Kelvin to Fahrenheit.- **Step 1: Understand the Formula** First, familiarize yourself with all components of the conversion formula, which is \(F = \frac{9}{5}(K - 273.15) + 32\). Determine what each part does, for instance, \(K - 273.15\) converts Kelvin to Celsius before it's adjusted into Fahrenheit.- **Step 2: Substitute the Value** Next, insert the Kelvin temperature value within the equation. In our example, this is 312.0 Kelvin.
The substituted equation will be: \(F = \frac{9}{5}(312.0 - 273.15) + 32\).- **Step 3: Perform the Calculations** Begin with the operations inside the parentheses: \(312.0 - 273.15 = 38.85\).
Continue by multiplying the result by \(\frac{9}{5}\) to convert from Celsius to Fahrenheit: \(\frac{9}{5} \times 38.85 = 69.93\).- **Step 4: Finalize the Result** Finally, add 32 to the result to account for the offset between Celsius and Fahrenheit scales: \(69.93 + 32 = 101.93\).
Now we have our conversion complete with a final result of approximately 101.93°F.
Mathematical operations
Understanding mathematical operations is essential for correctly applying the Kelvin to Fahrenheit formula.
These operations include subtraction, multiplication, and addition.
Let's see how each operation plays a role in temperature conversion:- **Subtraction** This operation modifies the Kelvin temperature to align with Celsius by removing 273.15 from the given value. For our example, it was \(312.0 - 273.15\).- **Multiplication** The conversion from Celsius to Fahrenheit involves multiplying by the fraction \(\frac{9}{5}\), which scales the Celsius result appropriately for the Fahrenheit system.- **Addition** Finally, add 32 to complete the conversion to the Fahrenheit scale. This accounts for the difference in the starting point of the Celsius and Fahrenheit scales.
Each operation is straightforward but vital. By performing them accurately, step-by-step, you ensure the correctness of your temperature conversion. This stepwise approach, rooted in fundamental math, not only assists in conversion tasks but also sharpens your mathematical prowess.

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Most popular questions from this chapter

An unknown material has a normal melting/freezing point of \(-25.0^{\circ} \mathrm{C},\) and the liquid phase has a specific heat capacity of \(160 \mathrm{J} /\left(\mathrm{kg} \cdot \mathrm{C}^{\circ}\right)\) One-tenth of a kilogram of the solid at \(-25.0^{\circ} \mathrm{C}\) is put into a \(0.150-\mathrm{kg}\) aluminum calorimeter cup that contains \(0.100 \mathrm{kg}\) of glycerin. The temperature of the cup and the glycerin is initially \(27.0^{\circ} \mathrm{C}\). All the unknown material melts, and the final temperature at equilibrium is \(20.0^{\circ} \mathrm{C} .\) The calorimeter neither loses energy to nor gains energy from the external environment. What is the latent heat of fusion of the unknown material?

Ideally, when a thermometer is used to measure the temperature of an object, the temperature of the object itself should not change. However, if a significant amount of heat flows from the object to the thermometer, the temperature will change. A thermometer has a mass of\(31.0 \mathrm{g},\) a specific heat capacity of \(c=815 \mathrm{J} /\left(\mathrm{kg} \cdot \mathrm{C}^{\circ}\right),\) and a temperature of \(12.0^{\circ} \mathrm{C} .\) It is immersed in \(119 \mathrm{g}\) of water, and the final temperature of the water and thermometer is \(41.5^{\circ} \mathrm{C} .\) What was the temperature of the water before the insertion of the thermometer?

Two grams of liquid water are at \(0^{\circ} \mathrm{C},\) and another two grams are at \(100^{\circ} \mathrm{C} .\) Heat is removed from the water at \(0^{\circ} \mathrm{C},\) completely freezing it at \(0^{\circ} \mathrm{C} .\) This heat is then used to vaporize some of the water at \(100^{\circ} \mathrm{C} .\) What is the mass (in grams) of the liquid water that remains?

A steel bicycle wheel (without the rubber tire) is rotating freely with an angular speed of \(18.00 \mathrm{rad} / \mathrm{s}\). The temperature of the wheel changes from \(-100.0\) to \(+300.0^{\circ} \mathrm{C} .\) No net external torque acts on the wheel, and the mass of the spokes is negligible. (a) Does the angular speed increase or decrease as the wheel heats up? Why? (b) What is the angular speed at the higher temperature?

Occasionally, huge icebergs are found floating on the ocean's currents. Suppose one such iceberg is \(120 \mathrm{km}\) long, \(35 \mathrm{km}\) wide, and \(230 \mathrm{m}\) thick. (a) How much heat would be required to melt this iceberg (assumed to be at \(\left.0^{\circ} \mathrm{C}\right)\) into liquid water at \(0^{\circ} \mathrm{C}\) ? The density of ice is \(917 \mathrm{kg} / \mathrm{m}^{3} .\) (b) The annual energy consumption by the United States is about \(1.1 \times 10^{20} \mathrm{J}\). If this energy were delivered to the iceberg every year, how many years would it take before the ice melted?

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