Answer:
ΔG° = 2.57 × 10² kJ
The reaction is spontaneous.
Explanation:
<em>The standard cell potential, E°cell, for a reaction in which two electrons are transferred between the reactants is +1.33 V. Calculate the standard free energy change, ΔG°, in kJ for this reaction and determine if it is spontaneous or nonspontaneous at 25°C.</em>
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We can calculate the standard Gibbs free energy (ΔG°) using the following expression.
ΔG° = -n × F × E°cell
where,
n: moles of electrons transferred
F: Faraday's constant
E°cell: standard cell potential
ΔG° = - (2 mol) × (96468 J/V . mol) × 1.33 V
ΔG° = -2.57 × 10⁵ J = 2.57 × 10² kJ
ΔG° < 0 means that the reaction is spontaneous.
Answer:
B. six protons, six neutrons, and six electrons
Explanation:
Carbon-14 and Carbon-12 are the isotopes of carbon.
Isotope:
An atom of an element that contain same atomic number but different atomic mass.
The difference in atomic mass is due to the different number of neutrons present, but the number protons and electrons are remain same.
In C-14 there are six protons and six electrons while number of neutrons are,
Mass number - number of protons = number of neutrons
14- 6 = 8
In C-12 there are six protons and six electrons while number of neutrons are,
Mass number - number of protons = number of neutrons
12- 6 = 6
Thus in C-12, there are six protons, six neutrons and six electrons present.
Chemists use reactions to generate a desired product. For the most part, a reaction is only useful if it occurs at a reasonable rate. For example, a reaction that took 8,000 years to complete would not be a desirable way to produce brake fluid. However, a reaction that proceeded so quickly that it caused an explosion would also not be useful (unless the explosion was the desired result). For these reasons, chemists wish to be able to control reaction rates. In order to gain this control, we must first know what factors affect the rate of a reaction. We will discuss some of these factors in this section.
