The bombardier beetle uses an explosive discharge as a defensive measure. The chemical reaction involved is the oxidation of hydroquinone by hydrogen peroxide to produce quinone and water: C 6 H 4 (OH) 2 ( aq ) + H 2 O 2 ( aq ) → C 6 H 4 O 2 ( aq ) + 2H 2 O( l ) Calculate Δ H for this reaction from the following data: C 6 H 4 (OH) 2 ( aq ) → C 6 H 4 O 2 ( aq ) + H 2 ( g ) Δ H = 177.4 kJ H 2 ( g ) + O 2 ( g ) → H 2 O 2 ( aq ) Δ H = −191.2 kJ H 2 ( g ) + 1 2 O 2 ( g ) → H 2 O( g ) Δ H = −241.8 kJ H 2 O( g ) → H 2 O( l ) Δ H = −43.8 kJ
The bombardier beetle uses an explosive discharge as a defensive measure. The chemical reaction involved is the oxidation of hydroquinone by hydrogen peroxide to produce quinone and water: C 6 H 4 (OH) 2 ( aq ) + H 2 O 2 ( aq ) → C 6 H 4 O 2 ( aq ) + 2H 2 O( l ) Calculate Δ H for this reaction from the following data: C 6 H 4 (OH) 2 ( aq ) → C 6 H 4 O 2 ( aq ) + H 2 ( g ) Δ H = 177.4 kJ H 2 ( g ) + O 2 ( g ) → H 2 O 2 ( aq ) Δ H = −191.2 kJ H 2 ( g ) + 1 2 O 2 ( g ) → H 2 O( g ) Δ H = −241.8 kJ H 2 O( g ) → H 2 O( l ) Δ H = −43.8 kJ
The bombardier beetle uses an explosive discharge as a defensive measure. The chemical reaction involved is the oxidation of hydroquinone by hydrogen peroxide to produce quinone and water:
C6H4(OH)2(aq) + H2O2(aq) → C6H4O2(aq) + 2H2O(l)
Calculate ΔH for this reaction from the following data:
C6H4(OH)2(aq) → C6H4O2(aq) + H2(g) ΔH = 177.4 kJ
H2(g) + O2(g) → H2O2(aq) ΔH = −191.2 kJ
H2(g) +
1
2
O2(g) → H2O(g) ΔH = −241.8 kJ
H2O(g) → H2O(l) ΔH = −43.8 kJ
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
Expert Solution & Answer
Interpretation Introduction
Interpretation:
The
ΔH value for the given reaction should be calculated.
Concept Introduction:
Enthalpy change: It is defined as the amount of heat released or absorbed by the chemical reaction at constant pressure conditions.
Specific heat capacity: It is the amount of heat required by the substance to increase temperature of the 1 kilogram of the substance by 1 kelvin.
Calorimeter: It is the device used to measure the heat involved in the chemical reaction.
The heat released by the reaction is measured in calorimetry by using the following formula.
Coffee cup calorimeter: It is used to measure the heat in the reaction where the atmospheric pressure remains constant. It is also regarded as constant pressure calorimeter.
Bomb calorimeter: It is used to measure the heat which the volume kept constant. Hence it enables us to find the energy changes in the reaction. It is also regarded as constant volume calorimeter.
Answer to Problem 79E
The
ΔH value for the given reaction is
-202.6kJ.
To calculate: The
ΔH value for the given reaction.
Explanation of Solution
Examining the given process the enthalpy change value that is
ΔH for the given reaction calculated as follows,
The final given reaction is obtained by equating all the four given reactions where second reaction is written in reverse order hence its
ΔH value will be then positive value.
Then third and fourth reactions are multiplied by 2 which their
ΔH values should also be multiplied by 2.
Hence, the final reaction
C6H4(OH)2(aq)+H2O2(aq)→C6H4O2(aq)+2H2O(l) is obtained by rearranging the given set of equations as follows,
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