Answer:
C
Explanation:
For electromagnetic waves frequency X wavelength = speed of light
f * 2.2 x 10^-11 = 3 x 10^8 m/s
f = 3 x 10^8 / 2.2 x 10^-11
= 1.36 x 10 ^19
= 1.4 x 10^19 with two significant digits
Answer:
330 mL of (NH₄)₂SO₄ are needed
Explanation:
First of all, we determine the reaction:
(NH₄)₂SO₄ + 2NaOH → 2NH₃ + 2H₂O + Na₂SO₄
We determine the moles of base:
(First, we convert the volume from mL to L) → 62.6 mL . 1L/1000 mL = 0.0626L
Molarity . volume (L) = 2.31 mol/L . 0.0626 L = 0.144 moles
Ratio is 2:1. Therefore we make a rule of three:
2 moles of hydroxide react with 1 mol of sulfate
Then, 0.144 moles of NaOH must react with (0.144 .1) /2 = 0.072 moles
If we want to determine the volume → Moles / Molarity
0.072 mol / 0.218 mol/L = 0.330 L
We convert from L to mL → 0.330L . 1000 mL/1L = 330 mL
Answer:
![\boxed {\boxed {\sf 0.80 \ mol\ F}}](https://tex.z-dn.net/?f=%5Cboxed%20%7B%5Cboxed%20%7B%5Csf%200.80%20%5C%20mol%5C%20F%7D%7D)
Explanation:
We are asked to find how many moles are in 4.8 × 10²³ fluorine atoms. We convert atoms to moles using Avogadro's Number or 6.022 × 10²³. This is the number of particles (atoms, molecules, formula units, etc.) in 1 mole of a substance. In this case, the particles are atoms of fluorine.
We will convert using dimensional analysis and set up a ratio using Avogadro's Number.
![\frac {6.022 \times 10^{23} \ atoms \ F}{ 1 \ mol \ F}](https://tex.z-dn.net/?f=%5Cfrac%20%7B6.022%20%5Ctimes%2010%5E%7B23%7D%20%5C%20atoms%20%5C%20F%7D%7B%201%20%5C%20mol%20%5C%20F%7D)
We are converting 4.8 × 10²³ fluorine atoms to moles, so we multiply the ratio by this number.
![4.8 \times 10^{23} \ atoms \ F *\frac {6.022 \times 10^{23} \ atoms \ F}{ 1 \ mol \ F}](https://tex.z-dn.net/?f=4.8%20%5Ctimes%2010%5E%7B23%7D%20%5C%20atoms%20%5C%20F%20%2A%5Cfrac%20%7B6.022%20%5Ctimes%2010%5E%7B23%7D%20%5C%20atoms%20%5C%20F%7D%7B%201%20%5C%20mol%20%5C%20F%7D)
Flip the ratio so the units of atoms of fluorine cancel each other out.
![4.8 \times 10^{23} \ atoms \ F *\frac { 1 \ mol \ F}{6.022 \times 10^{23} \ atoms \ F}](https://tex.z-dn.net/?f=4.8%20%5Ctimes%2010%5E%7B23%7D%20%5C%20atoms%20%5C%20F%20%2A%5Cfrac%20%7B%201%20%5C%20mol%20%5C%20F%7D%7B6.022%20%5Ctimes%2010%5E%7B23%7D%20%5C%20atoms%20%5C%20F%7D)
![4.8 \times 10^{23} *\frac { 1 \ mol \ F}{6.022 \times 10^{23} }](https://tex.z-dn.net/?f=4.8%20%5Ctimes%2010%5E%7B23%7D%20%20%2A%5Cfrac%20%7B%201%20%5C%20mol%20%5C%20F%7D%7B6.022%20%5Ctimes%2010%5E%7B23%7D%20%7D)
Condense into 1 fraction.
![\frac { 4.8 \times 10^{23} }{6.022 \times 10^{23} } \ mol \ F](https://tex.z-dn.net/?f=%5Cfrac%20%7B%204.8%20%5Ctimes%2010%5E%7B23%7D%20%7D%7B6.022%20%5Ctimes%2010%5E%7B23%7D%20%7D%20%5C%20mol%20%5C%20F)
Divide.
![0.7970773829 \ mol \ F](https://tex.z-dn.net/?f=0.7970773829%20%5C%20mol%20%5C%20F)
The original measurement of atoms has 2 significant figures, so our answer must have the same. For the number we found, that is the hundredths place. The 7 in the thousandths tells us to round the 9 in the hundredths place up to a 0. Then, we also have to round the 7 in the tenths place up to an 8.
![0.80 \ mol \ F](https://tex.z-dn.net/?f=0.80%20%5C%20mol%20%5C%20F)
4.8 × 10²³ fluorine atoms are equal to <u>0.80 moles of fluorine.</u>