The specific heat of ethanol, C 2 H 5 OH(l), is 2.44 J•g/K. b. Which will require more heat, increasing the temperature of 1 mol of C 2 H 5 OH(𝑙) by a certain amount or increasing the temperature of 1 mol of H 2 O(𝑙) by the same amount?

Hi everyone here we have a question asking us to identify which between one mole of water or one mole of acetic acid will cries more heat to increase the temperature by one degree. At the specific heat of acetic acid is 2.043 jules. Programs kelvin. So first we're going to convert to moles Using the more mass, the more mass of acetic acid is 60 0.6 grams Permal. The molar mass of water is 18 .02 g per mole. And now we can convert to moles. So for acetic acid, we're going to take our heat capacity to point 043 jules, her grams times kelvin. We're going to multiply by the molar mass. So 60.6 grams per mole And that equals 0.7 jules Permal times kelvin. Next we're going to do the same for water. So its specific heat is for .184 jules per grams times killed in Are going to multiply by its molar mass, which is 18.02 grams per mole. And that equals 0.40 jules Permal times kelvin. So acetic acid Is going to require more heat to increase the temperature by 1° because it is our larger number. So our answer is acetic acid. Thank you for watching. Bye.

Ch.5 - Thermochemistry

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Brown 15th Edition

Ch.5 - Thermochemistry

Problem 53b

Chapter 5, Problem 53b

The specific heat of ethanol, C₂H₅OH(l), is 2.44 J•g/K. b. Which will require more heat, increasing the temperature of 1 mol of C₂H₅OH(𝑙) by a certain amount or increasing the temperature of 1 mol of H₂O(𝑙) by the same amount?

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Identify the specific heat capacity of both substances: Ethanol (C_2H_5OH) has a specific heat capacity of 2.44 J/g·K, and water (H_2O) has a specific heat capacity of 4.18 J/g·K.

Calculate the molar mass of ethanol (C_2H_5OH) by adding the atomic masses of its constituent atoms: 2 carbon atoms, 6 hydrogen atoms, and 1 oxygen atom.

Calculate the molar mass of water (H_2O) by adding the atomic masses of its constituent atoms: 2 hydrogen atoms and 1 oxygen atom.

Determine the mass of 1 mole of each substance using their respective molar masses.

Use the formula q = m × c × ΔT to compare the heat required for each substance, where q is the heat absorbed, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

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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 one Kelvin). It is a crucial property that varies between different substances, influencing how much heat is needed to change their temperature. In this question, the specific heat of ethanol is given, which allows for comparison with water's specific heat to determine which substance requires more heat for the same temperature change.

Molar Mass and Moles

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. Understanding moles is essential in chemistry as it allows for the conversion between mass and the number of particles. In this question, both ethanol and water are considered in terms of moles, which helps in calculating the total heat required to raise their temperatures based on their specific heat capacities.

Heat Transfer Equation

The heat transfer equation, often expressed as q = mcΔT, relates the heat absorbed or released (q) to the mass (m), specific heat capacity (c), and the change in temperature (ΔT). This equation is fundamental for solving problems involving temperature changes in substances. In this context, it will be used to compare the heat required for both ethanol and water when their temperatures are increased by the same amount.

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Heat Capacity

Related Practice

Textbook Question

(d) How many kJ of heat are needed to raise the temperature of 10.00 kg of liquid water from 24.6 to 46.2 °C?

Textbook Question

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

Textbook Question

The specific heat of ethanol, C₂H₅OH(l), is 2.44 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?

Textbook Question

Consider the data about gold metal in Exercise 5.24(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 the other is iron metal. Which block will have the greater rise in temperature after addition of the heat?

Textbook Question

Consider the data about gold metal in Exercise 5.24(b). c. What is the molar heat capacity of Au(s)?

Textbook Question

When a 5.10-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 20.5 to 33.2 °C. a. Calculate the quantity of heat (in kJ) released in the reaction.

The specific heat of ethanol, C2H5OH(l), is 2.44 J•g/K. b. Which will require more heat, increasing the temperature of 1 mol of C2H5OH(𝑙) by a certain amount or increasing the temperature of 1 mol of H2O(𝑙) by the same amount?

Verified video answer for a similar problem:

Key Concepts

Specific Heat Capacity

Molar Mass and Moles

Heat Transfer Equation

The specific heat of ethanol, C₂H₅OH(l), is 2.44 J•g/K. b. Which will require more heat, increasing the temperature of 1 mol of C₂H₅OH(𝑙) by a certain amount or increasing the temperature of 1 mol of H₂O(𝑙) by the same amount?