/*! 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 52 The specific heat of ethylene gl... [FREE SOLUTION] | 91影视

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Chapter 5: Problem 52

The specific heat of ethylene glycol is \(2.42 \mathrm{~J} / \mathrm{g}-\mathrm{K} .\) How many J of heat are needed to raise the temperature of \(62.0 \mathrm{~g}\) of ethylene glycol from \(13.1^{\circ} \mathrm{C}\) to \(40.5^{\circ} \mathrm{C}\) ?

Short Answer

Expert verified
Approximately \(4188.5 \mathrm{~J}\) of heat are needed to raise the temperature of \(62.0 \mathrm{~g}\) of ethylene glycol from \(13.1^{\circ} \mathrm{C}\) to \(40.5^{\circ} \mathrm{C}\).

Step by step solution

01

Identify the given values

We have been given the following values: - Specific Heat (c) = 2.42 J/g-K - Mass (m) = 62.0 g - Initial Temperature (T1) = 13.1掳C - Final Temperature (T2) = 40.5掳C
02

Calculate the temperature change

We need to find the temperature change (鈭員), so we subtract the initial temperature (T1) from the final temperature (T2): 鈭員 = T2 - T1 鈭員 = 40.5掳C - 13.1掳C 鈭員 = 27.4 K
03

Use the formula to calculate the heat required

Now that we have all the values, we can use the formula: Heat (Q) = Mass (m) x Specific Heat (c) x Temperature Change (鈭員) Q = (62.0 g) x (2.42 J/g-K) x (27.4 K)
04

Calculate the heat required

Multiply the values to get the result: Q = 62.0 x 2.42 x 27.4 Q 鈮� 4188.5 J So, approximately 4188.5 J of heat are needed to raise the temperature of 62.0 g of ethylene glycol from 13.1掳C to 40.5掳C.

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Most popular questions from this chapter

It is estimated that the net amount of carbon dioxide fixed by photosynthesis on the landmass of Earth is \(5.5 \times\) \(10^{16} \mathrm{~g} / \mathrm{yr}\) of \(\mathrm{CO}_{2}\). Assume that all this carbon is converted into glucose. (a) Calculate the energy stored by photosynthesis on land per year in \(\mathrm{kJ}\). (b) Calculate the average rate of conversion of solar energy into plant energy in MW \((1 \mathrm{~W}=1 \mathrm{~J} / \mathrm{s})\). A large nuclear power plant produces about \(10^{3} \mathrm{MW}\). The energy of how many such nuclear power plants is equivalent to the solar energy conversion?

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