For the reaction 2Co^3+ (aq) + 2Cl^- (aq) ----> 2Co^2+ + Cl2 (g)
E^o = 0.46 V (STANDARD cell potential)
what is the cell potential at (25 deg C) if the concentrations are [Co^3+] = 0.651M , [Co^2+]= 0.846 M, and [Cl^-] = 0.636 M and the pressure of Cl2 is PCl2= 9.30 atm ?
For the reaction
2Co^{3+}(aq)+2Cl^-(aq) ----> 2Co^{2+}(aq)+Cl2(g).E= 0.71V
what is the cell potential at 25 C if the concentrations are [Co^{3+}]= 0.437M, [Co^{2+}]= 0.109 M, and [Cl^-]= 0.856 M and the pressure of Cl2 is 7.20 atm?
Nernst equation is E=E-({0.0591/{n})*log Q
here E^\circ is the standard reduction potential for the reaction in volts and Q is the reaction quotient. The reaction quotient has the usual form
Q ={ products}]^x / [ reactants}]^y}
i think your answer is
E = Eo - 0.0591/n x log ([Co2+]^2 x PCl2) / ([Co3+]^2 x [Cl-])^2
E = 0.71 - 0.0591 / 2 x log (0.109)^2(7.20)/(0.437)^2(0.856)^2
E = 0.71 + 0.006 = 0.72 V (to 2 sig figs
Well, to calculate the cell potential at 25 degrees Celsius, we can use the Nernst equation, which is like the mood ring of electrochemistry. It tells us how the cell potential changes with concentration and pressure. Let's dive in and make some calculations while keeping our sense of humor intact.
The Nernst equation is given as follows:
E = E^o - (0.0592/n) * log(Q)
First, we need to find the reaction quotient, Q. For this, we'll use the concentrations of the species involved. Since the stoichiometric coefficients are both 2, we don't need to worry about balancing them. So, we'll have:
Q = ([Co^2+]^2 * [Cl2]) / ([Co^3+]^2 * [Cl^-]^2)
Plugging in the given concentrations, we get:
Q = (0.846^2 * 9.30) / (0.651^2 * 0.636^2)
Now, let's use the Nernst equation, keeping in mind that n (the number of electrons transferred) is 2 for this reaction:
E = 0.46 V - (0.0592/2) * log(Q)
Calculating this expression will give us the actual cell potential at 25 degrees Celsius. Math time!
E = 0.46 V - (0.0296) * log[(0.846^2 * 9.30) / (0.651^2 * 0.636^2)]
And... voila! There you have it. Plug in the numbers and solve away. Just remember, even though electrochemistry can be electrifying, it's always good to keep your humor charged.
To calculate the cell potential at 25 °C, we can use the Nernst equation:
E = E^o - (0.0592 V / n) log(Q)
where:
E is the cell potential
E^o is the standard cell potential
n is the number of electrons transferred in the balanced equation
Q is the reaction quotient
Let's start by determining the value of Q:
Q = [Co^2+]^2 * [Cl2] / [Co^3+]^2 * [Cl^-]^2
Plugging in the given values:
[Co^2+] = 0.846 M
[Cl2] = PCl2 / RT (R = 0.0821 L·atm/(K·mol), T = 25 + 273.15 K)
[Co^3+] = 0.651 M
[Cl^-] = 0.636 M
Using the ideal gas law, we can calculate the pressure of Cl2 in terms of concentration:
PV = nRT
n/V = P/RT, where n/V is the molar concentration, P is the pressure, and R is the ideal gas constant.
n/V (Cl2) = PCl2 / RT
Now let's calculate n/V for Cl2:
n/V (Cl2) = (9.30 atm) / (0.0821 L·atm/(K·mol) * (25 + 273.15) K)
Next, we calculate the reaction quotient Q:
Q = (0.846 M)^2 * PCl2 / (0.651 M)^2 * (0.636 M)^2
Now we can substitute the values into the Nernst equation:
E = E^o - (0.0592 V / n) log(Q)
where:
E^o = 0.46 V
n = number of electrons transferred (from balanced equation)
You'll need to provide the balanced equation to determine the value of n - how many electrons are transferred in the reaction.
To calculate the cell potential at 25°C with the given concentrations and pressure, we need to use the Nernst equation:
E = E^o - (0.0592/n) * log(Q)
Where:
- E is the cell potential at non-standard conditions
- E^o is the standard cell potential
- n is the number of electrons transferred in the balanced equation
- Q is the reaction quotient, which is calculated using the concentrations of the species involved in the reaction
Step 1: Calculate the reaction quotient (Q)
In this case, the reaction quotient (Q) is calculated by taking the ratios of the products and reactants raised to their stoichiometric coefficients:
Q = ([Co^2+]^2 * [Cl2]) / ([Co^3+]^2 * [Cl^-]^2)
Substituting the given concentrations:
Q = (0.846^2 * 9.30) / (0.651^2 * 0.636^2)
Step 2: Calculate the cell potential (E)
Using the Nernst equation, with n = 2 (since 2 electrons are transferred in the balanced equation):
E = E^o - (0.0592/2) * log(Q)
Substituting the given standard cell potential (E^o = 0.46 V) and the calculated reaction quotient (Q), we can now calculate E.