The answer to 4 is A.
The answer to 5 is C.
Answer:
0.54g of Cr
Explanation:
Current (I) = 10A
Time (t) = 100s
Molecular mass of Cr = 51.996 amu
Faraday's first law of electrolysis states that
The mass of the substance (m) of a given substance deposited at an electrode is directly proportional to the quantity of electricity or charge (Q) passed
m = nQ
M = mass of the substance
n = electrochemical constant
Q = charge passed through it
Q = IT
Q = (10 * 100) = 1000C
1 moles = molarmass = Faraday's constant (96500C)
Molar mass = Faraday's constant (96500C)
51.996 g = 96500C
How many grams will be liberated with 1000C
51.996g = 96500C
Xg = 1000C
X = (1000 * 51.996) / 96500
X = 51996 / 96500
X = 0.5388g = 0.54 g of Cr will be deposited
If iron (Fe) gained a proton it would become cobalt (CO).
Answer:

Explanation:
<u>1. Convert Grams to Moles</u>
Use the molar mass (found on the Periodic Table) to convert from grams to moles.
Use this value as a ratio.

Multiply by the given number of grams.

Flip the ratio so the grams of boron cancel out.



<u>2. Convert Moles to Atoms</u>
We use Avogadro's Number, 6.02*10²³: the number of particles (atoms, molecules, etc.) in 1 mole of a substance. In this case, the particles are atoms of boron.

Multiply by the number of moles we calculated.

The moles of boron cancel.


The original value of grams has 4 significant figures, so our answer should have the same. For the number we calculated, that is the thousandth place.

The 6 tells us to round the 2 to a 3.

25.00 grams of boron is equal to 1.393*10²⁴ atoms.
8.509 kilocalories I think