A simple, albeit slightly less useful example perhaps, is when a foundry, or individual metalworker, liquefies metal such as iron, aluminum, or steel so that it can be mixed in with specific forging agents or transferred around a workplace.
In general solids are easier to transport than liquids, but the above metal example is a valid one and the only other one that comes to mind is that of concrete. It is mixed as a liquid and transported as such, but then sprayed or laid down to dry and form a solid surface or filler. <span />
Answer : The mass of carbon required is, 309.4 grams.
Explanation : Given,
Mass of oxygen = 1100 g
Molar mass of oxygen = 16 g/mol
Molar mass of carbon = 12 g/mol
First we have to calculate the moles of oxygen.
![\text{Moles of oxygen}=\frac{\text{Mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{1100g}{16g/mol}=68.75mol](https://tex.z-dn.net/?f=%5Ctext%7BMoles%20of%20oxygen%7D%3D%5Cfrac%7B%5Ctext%7BMass%20of%20oxygen%7D%7D%7B%5Ctext%7BMolar%20mass%20of%20oxygen%7D%7D%3D%5Cfrac%7B1100g%7D%7B16g%2Fmol%7D%3D68.75mol)
Now we have to calculate the moles of carbon.
Moles of carbon = ![\frac{3.0}{8.0}\times \text{Moles of oxygen}](https://tex.z-dn.net/?f=%5Cfrac%7B3.0%7D%7B8.0%7D%5Ctimes%20%5Ctext%7BMoles%20of%20oxygen%7D)
Moles of carbon = ![\frac{3.0}{8.0}\times 68.75mol=25.78mol](https://tex.z-dn.net/?f=%5Cfrac%7B3.0%7D%7B8.0%7D%5Ctimes%2068.75mol%3D25.78mol)
Now we have to calculate the mass of carbon.
![\text{Mass of carbon}=\text{Moles of carbon}\times \text{Molar mass of carbon}](https://tex.z-dn.net/?f=%5Ctext%7BMass%20of%20carbon%7D%3D%5Ctext%7BMoles%20of%20carbon%7D%5Ctimes%20%5Ctext%7BMolar%20mass%20of%20carbon%7D)
![\text{Mass of carbon}=25.78mol\times 12g/mol=309.4g](https://tex.z-dn.net/?f=%5Ctext%7BMass%20of%20carbon%7D%3D25.78mol%5Ctimes%2012g%2Fmol%3D309.4g)
Thus, the mass of carbon required is, 309.4 grams.
<span> because gasoline changes volume as a function of temperature or because there are different grades of gasoline or because the values are given in different units of measure .</span>
<h2>
Answer: 1.22 × 10⁻¹ m</h2>
<h3>Explanation:</h3>
Wavelength = Speed of Light ÷ Frequency
= (2.99 × 10⁸ m/s) ÷ ( 2.45 × 10⁹ /s)
= 1.22 × 10⁻¹ m
The wavelength of a light of frequency 2.45 × 10⁹ /s is 1.22 × 10⁻¹ m.
<u>Notes:</u>
Hz ≡ /s