That because that element has received electrons from another element
hope that helps
Answer:
The mole fraction of NaOH in an aqueous solution that contain 22.9% NaOH by mass=0.882
Explanation:
We are given that
Aqueous solution that contains 22.9% NaOH by mass means
22.9 g NaOH in 100 g solution.
Mass of NaOH(WB)=22.9 g
Mass of water =100-22.9=77.1
Na=23
O=16
H=1.01
Molar mass of NaOH(MB)=23+16+1.01=40.01
Number of moles =![\frac{Given\;mass}{Molar\;mass}](https://tex.z-dn.net/?f=%5Cfrac%7BGiven%5C%3Bmass%7D%7BMolar%5C%3Bmass%7D)
Using the formula
Number of moles of NaOH![(n_B)=\frac{W_B}{M_B}=\frac{22.9}{40.01}](https://tex.z-dn.net/?f=%28n_B%29%3D%5Cfrac%7BW_B%7D%7BM_B%7D%3D%5Cfrac%7B22.9%7D%7B40.01%7D)
![n_B=0.572moles](https://tex.z-dn.net/?f=n_B%3D0.572moles)
Molar mass of water=16+2(1.01)=18.02g
Number of moles of water![(n_A)=\frac{77.1}{18.02}](https://tex.z-dn.net/?f=%28n_A%29%3D%5Cfrac%7B77.1%7D%7B18.02%7D)
![n_A=4.279 moles](https://tex.z-dn.net/?f=n_A%3D4.279%20moles)
Now, mole fraction of NaOH
=![\frac{n_B}{n_B+n_A}](https://tex.z-dn.net/?f=%5Cfrac%7Bn_B%7D%7Bn_B%2Bn_A%7D)
![=\frac{4.279}{0.572+4.279}](https://tex.z-dn.net/?f=%3D%5Cfrac%7B4.279%7D%7B0.572%2B4.279%7D)
=0.882
Hence, the mole fraction of NaOH in an aqueous solution that contain 22.9% NaOH by mass=0.882
2 C5H12O + 15 O2 = 10 CO2 + 12 H2O
Hope this helped :)
Avogadro’s constant tells us the number of atoms in a mole of any substance: 6.022x10^23. A mole of water, oxygen, sodium - they all have this many atoms in a 1 mole sample.
A 0.5 mole sample of helium gas would contain 0.5 x (6.022 x 10^23) atoms, or 3.011 x 10^23 atoms. Still a big amount.