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Ch.5 - Thermochemistry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.5 - ThermochemistryProblem 53a
Chapter 5, Problem 53a

The specific heat of octane, C8H18(l), is 2.22 J•g/K. (a) How many J of heat are needed to raise the temperature of 80.0 g of octane from 10.0 to 25.0 °C?

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Identify the given values: specific heat (c) = 2.22 J/g/K, mass (m) = 80.0 g, initial temperature (T1) = 10.0 °C, and final temperature (T2) = 25.0 °C.
Calculate the change in temperature (ΔT) by subtracting the initial temperature from the final temperature: ΔT = T2 - T1.
Use the formula for heat transfer, Q = mcΔT, where Q is the heat energy transferred, m is the mass, c is the specific heat, and ΔT is the change in temperature.
Substitute the values into the formula: Q = (80.0 g) * (2.22 J/g/K) * (ΔT from step 2).
Calculate the product to find the total heat energy (Q) required in joules.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Specific Heat Capacity

Specific heat capacity is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius (or Kelvin). It is a material-specific property that indicates how much energy is needed to change the temperature of a given mass of the substance. In this case, octane has a specific heat of 2.22 J/g·K, meaning it requires 2.22 joules of energy to increase the temperature of one gram of octane by one degree.
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Heat Transfer Calculation

The heat transfer (q) required to change the temperature of a substance can be calculated using the formula q = m × c × ΔT, where m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature. This formula allows us to quantify the energy needed for temperature changes in various materials, making it essential for solving problems related to thermal energy.
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Temperature Change

Temperature change (ΔT) is the difference between the final and initial temperatures of a substance. It is calculated as ΔT = T_final - T_initial. In the context of the question, the temperature change for octane is from 10.0 °C to 25.0 °C, which is a critical component in determining the total heat required for the temperature increase, as it directly influences the amount of energy needed.
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Related Practice
Textbook Question

The specific heat of octane, C8H18(l), is 2.22 J•g/K. (b) Which will require more heat, increasing the temperature of 1 mol of C8H18(l), by a certain amount or increasing the temperature of 1 mol of H2O(l) by the same amount?

Textbook Question

Consider the data about gold metal in Exercise 5.26(b). (a) Based on the data, calculate the specific heat of Au(s).

Textbook Question

Consider the data about gold metal in Exercise 5.26(b). (b) Suppose that the same amount of heat is added to two 10.0-g blocks of metal, both initially at the same temperature. One block is gold metal, and one is iron metal. Which block will have the greater rise in temperature after the addition of the heat?

Textbook Question

(d) How many kJ of heat are needed to raise the temperature of 5.00 kg of liquid water from 24.6 to 46.2 °C?

Textbook Question

(b) Calculate the energy needed for this temperature change.

Textbook Question

(c) What is the heat capacity of 185 g of liquid water?

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