B, I would believe. There are 58, but B is the closest we can get.
Answer:
awnser is true took the test
Explanation:
i took the test
Answer : It takes time to produce 3 g of aluminium is, 165 seconds.
Explanation :
As we are given that the mass of aluminium is, 3 grams. Now we have to calculate the total mass of aluminum.
Total mass of aluminum = 3g × 24 = 72 g
Now we have to calculate the moles of aluminum.

Molar mass of Al = 27 g/mol

As, 1 mole of Al has 3 Faradays
So, 2.67 mole of Al has =
Faradays
and,
Charge = 
Current = 
Now we have to calculate the time.

Hence, it takes time to produce 3 g of aluminium is, 165 seconds.
Answer:
Therefore the required function is

Therefore 25°C=57°F
Explanation:
F denotes temperature of Fahrenheit and C denotes temperature of Celsius.



Therefore the required function is

Putting C=25°C in above equation


⇒45 =F-32
⇒F=32+45
⇒F=57
Therefore 25°C=57°F
<u>Answer:</u> The
for the reaction is 54.6 kJ/mol
<u>Explanation:</u>
For the given balanced chemical equation:

We are given:

- To calculate
for the reaction, we use the equation:
![\Delta G^o_{rxn}=\sum [n\times \Delta G_f(product)]-\sum [n\times \Delta G_f(reactant)]](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo_%7Brxn%7D%3D%5Csum%20%5Bn%5Ctimes%20%5CDelta%20G_f%28product%29%5D-%5Csum%20%5Bn%5Ctimes%20%5CDelta%20G_f%28reactant%29%5D)
For the given equation:
![\Delta G^o_{rxn}=[(2\times \Delta G^o_f_{(COCl_2)})]-[(1\times \Delta G^o_f_{(CO_2)})+(1\times \Delta G^o_f_{(CCl_4)})]](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo_%7Brxn%7D%3D%5B%282%5Ctimes%20%5CDelta%20G%5Eo_f_%7B%28COCl_2%29%7D%29%5D-%5B%281%5Ctimes%20%5CDelta%20G%5Eo_f_%7B%28CO_2%29%7D%29%2B%281%5Ctimes%20%5CDelta%20G%5Eo_f_%7B%28CCl_4%29%7D%29%5D)
Putting values in above equation, we get:
![\Delta G^o_{rxn}=[(2\times (-204.9))-((1\times (-394.4))+(1\times (-62.3)))]\\\Delta G^o_{rxn}=46.9kJ=46900J](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo_%7Brxn%7D%3D%5B%282%5Ctimes%20%28-204.9%29%29-%28%281%5Ctimes%20%28-394.4%29%29%2B%281%5Ctimes%20%28-62.3%29%29%29%5D%5C%5C%5CDelta%20G%5Eo_%7Brxn%7D%3D46.9kJ%3D46900J)
Conversion factor used = 1 kJ = 1000 J
- The expression of
for the given reaction:

We are given:

Putting values in above equation, we get:

- To calculate the Gibbs free energy of the reaction, we use the equation:

where,
= Gibbs' free energy of the reaction = ?
= Standard gibbs' free energy change of the reaction = 46900 J
R = Gas constant = 
T = Temperature = ![25^oC=[25+273]K=298K](https://tex.z-dn.net/?f=25%5EoC%3D%5B25%2B273%5DK%3D298K)
= equilibrium constant in terms of partial pressure = 22.92
Putting values in above equation, we get:

Hence, the
for the reaction is 54.6 kJ/mol