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Chapter 13: Problem 48

For a particular reaction, the absorbed energy is \(800 \mathrm{~kJ}\) to break old bonds, and \(\Delta E_{\mathrm{rxn}}\) is equal to \(-800 \mathrm{~kJ}\). How much energy is released into the surroundings as the product bonds are formed?

Short Answer

Expert verified
The energy released into the surroundings as the product bonds are formed is 1600 kJ. We can find this value by using the conservation of energy principle. Given the energy absorbed to break old bonds, 800 kJ, and the overall energy change in the reaction, -800 kJ, we can write the equation: (Energy absorbed) + (Energy released) = \(\Delta E_{\mathrm{rxn}}\). Substituting the given values, we get (800 kJ) + (Energy released) = -800 kJ. Solving for the energy released, we find that Energy released = -1600 kJ. Since the energy released is negative, it means 1600 kJ of energy is released into the surroundings as the product bonds are formed.

Step by step solution

01

Write down the given values

In this exercise, we are given: - The energy absorbed to break old bonds: 800 kJ - The overall energy change in the reaction: -800 kJ
02

Use the conservation of energy principle

According to the conservation of energy principle, the energy absorbed plus the energy released must equal the total energy change of the reaction. In formula form, this can be written as: (Energy absorbed) + (Energy released) = \(\Delta E_{\mathrm{rxn}}\)
03

Substitute the given values into the equation

Now, we can substitute the given values into the equation: (800 kJ) + (Energy released) = -800 kJ
04

Solve for the energy released

To solve for the energy released, we can subtract the energy absorbed from both sides of the equation: Energy released = -800 kJ - 800 kJ Energy released = -1600 kJ
05

Interpret the result

Since the energy released is negative, it means that the energy is being released into the surroundings. In this reaction, 1600 kJ of energy is released into the surroundings as the product bonds are formed.

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Most popular questions from this chapter

\(\Delta E_{\mathrm{rxn}}\) for the reaction \(\mathrm{X} \rightarrow \mathrm{Y}\) is \(+30 \mathrm{~kJ}\). (a) Is the reaction endothermic or exothermic? (b) Rewrite the reaction showing heat as either a reactant or a product. (c) What is the value of \(\Delta E_{\mathrm{rxn}}\) for the reverse reaction \(\mathrm{Y} \rightarrow \mathrm{X} ?\) (d) Is the reverse reaction endothermic or exothermic? (e) Will the container in which the forward reaction \(\mathrm{X} \rightarrow\) Y occurs feel hot or cold to the touch? Why?

Why is it unlikely that the reaction \(\mathrm{A}+2 \mathrm{~B}+\mathrm{C} \rightarrow \mathrm{P}\) occurs in one step?

What is the rule of thumb for how reaction rate changes as the temperature changes?

The slowest step in a reaction mechanism is called the _______-_______ step.

In general, increasing the concentration of a reactant will usually increase the rate of a reaction. Why is this true?
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