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A heterogeneous equilibrium reaction is when there are different phases in the reaction. An equilibrium reaction is a reaction that can go in both the forward and reverse directions, and the concentrations of the reactants and products remain the same.
So therefore, your answer is A. Heterogeneous!
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-Philaeagles14
Answer:
0.30 M
Explanation:
Using integrated rate law for first order kinetics as:
Where,
is the concentration at time t = ?
is the initial concentration = 1.36 M
k is the rate constant = 0.208 s⁻¹
t = 7.30 seconds
So,
<u>Answer:</u> The
for the reaction is -1052.8 kJ.
<u>Explanation:</u>
Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.
According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.
The given chemical reaction follows:
![\Delta H^o_{rxn}=?](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo_%7Brxn%7D%3D%3F)
The intermediate balanced chemical reaction are:
(1)
![\Delta H_1=-668.5kJ](https://tex.z-dn.net/?f=%5CDelta%20H_1%3D-668.5kJ)
(2)
![\Delta H_2=+384.3kJ](https://tex.z-dn.net/?f=%5CDelta%20H_2%3D%2B384.3kJ)
The expression for enthalpy of the reaction follows:
![\Delta H^o_{rxn}=[1\times \Delta H_1]+[1\times (-\Delta H_2)]](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo_%7Brxn%7D%3D%5B1%5Ctimes%20%5CDelta%20H_1%5D%2B%5B1%5Ctimes%20%28-%5CDelta%20H_2%29%5D)
Putting values in above equation, we get:
![\Delta H^o_{rxn}=[(1\times (-668.5))+(1\times (-384.3))=-1052.8kJ](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo_%7Brxn%7D%3D%5B%281%5Ctimes%20%28-668.5%29%29%2B%281%5Ctimes%20%28-384.3%29%29%3D-1052.8kJ)
Hence, the
for the reaction is -1052.8 kJ.
Because the older cells will not be able to function properly without the new cells taking over them. :)