Technically, the answer should be 3.30 * 10^23 grams. But I think you mean either molecules, atoms, moles or grams of Ni2I6 with that number of molecules .
1 mole of Ni2 I6 = 6.02 * 10^23 molecules
x [mole] = 3.30 * 10^23 molecules
1/x = 6.02 * 10^23 / 3.30 * 10^23 Cancel the 10^23 on the right side
1/x = 6.02 / 3.30 Cross multiply
3.30 = 6.02 x Divide by 6.02
3.30 / 6.02 = x
x = 0.548 moles
what to do from here?
1 mole of Ni2I6 is
2 * Ni = 2 * 59 = 118 grams
6 * I = 6 * 131 = <u>786 grams</u>
Total = 904 grams
Set up a proportion.
<u>1 mole Ni2I6 </u> = <u>904 grams</u>
0.548 moles = x
1/0.548 = 904/x Cross multiply
x = 0.548 * 904
x = 495.4 grams of Ni2I6 <<<<<< Answer.
Answer:
Metals tend to lose electrons in chemical reactions, as indicated by their low ionization energies. Within a compound, metal atoms have relatively low attraction for electrons, as indicated by their low electronegativities.
Answer:
2.25 M is the final concentration of hydroxide ions ions in the solution after the reaction has gone to completion.
Explanation:
Moles of NaOH = 
Molarity of the nitric acid solution = 0.250 M
Volume of the nitric solution = 0.150 L
Moles of nitric acid = n



According to reaction, 1 mole of nitric acid recats with 1 mole of NaOH, then 0.0375 moles of nitric acid will react with :
of NaOH
Moles of NaOH left unreacted in the solution =
= 0.375 mol - 0.0375 mol = 0.3375 mol

1 mole of sodium hydroxide gives 1 mol of sodium ions and 1 mole of hydroxide ions.
Then 0.3375 moles of NaOH will give :
of hydroxide ion
The molarity of hydroxide ion in solution ;

2.25 M is the final concentration of hydroxide ions ions in the solution after the reaction has gone to completion.






Answer:
Explanation:
From the correct question above:
The reaction can be represented as:

From the above reaction; the ICE table can be represented as:

I (mol/L) 0.086 0.28 0 0
C -4x -3x +2x +6x
E 0.086 - 4x 0.28 - 3x +2x +6x
At equilibrium;
The water vapor = 


![\text{equilibrium constant} ({k_c}) = \dfrac{ [N_2]^2 [H_2O]^6 }{ [[NH_3]^4] [O_2]^3 }](https://tex.z-dn.net/?f=%5Ctext%7Bequilibrium%20constant%7D%20%20%28%7Bk_c%7D%29%20%3D%20%20%5Cdfrac%7B%20%5BN_2%5D%5E2%20%5BH_2O%5D%5E6%20%7D%7B%20%5B%5BNH_3%5D%5E4%5D%20%5BO_2%5D%5E3%20%7D)

Replacing the value of x, we have:


Answer:
I believe this is a K-12 test question. If the answers below are what you have on your test . . .
- Precise
- Accurate
- Identical
- None of the above
Then the answer is <u>precise</u>.