solution:
First we calculate the number of mole of gas as follows:
PV = n RT
Here temperature; T= 100°C or 373 K
n = PV/ RT
= 4.78 atm * 3.82 L / 0.0821 L ∙ atm / mol ∙ K * 373 K
= 0.596 Moles
Now determine the molar mass of gas as follows:
Number of moles = amount in g/ molar mass
Molar mass = 19.08 grams / 0.596 Moles
= 32.013 g/ mole
This the molar mass of O2 hence the gas is oxygen
Answer:
150.000 g
Explanation:
The law of conservation of mass states that the mass of reactants and products of a reaction must be equal to one another.
In other words, for this case:
- Mass of KOH + Mass of HCl = Mass of Products
We are given all required data to<u> calculate the mass of the KOH solution</u>:
- Mass of KOH + 250.000 g = 400.000 g
Pounds of gold ore : 11,02311
<h3>Further explanation</h3>
Given
5 g of gold
0.1% gold by mass
Required
Pounds of gold ore
Solution
![\tt \%mass~gold=\dfrac{mass~gold}{mass~ore}\times 100\%](https://tex.z-dn.net/?f=%5Ctt%20%5C%25mass~gold%3D%5Cdfrac%7Bmass~gold%7D%7Bmass~ore%7D%5Ctimes%20100%5C%25)
For percent mass = 0.1%, than mass of gold ore :
![\tt 0.1\%=\dfrac{5~g}{mass~ore}\times 100\%\\\\mass~ore=\dfrac{5\times 100}{0.1}\\\\mass~ore=5000~g](https://tex.z-dn.net/?f=%5Ctt%200.1%5C%25%3D%5Cdfrac%7B5~g%7D%7Bmass~ore%7D%5Ctimes%20100%5C%25%5C%5C%5C%5Cmass~ore%3D%5Cdfrac%7B5%5Ctimes%20100%7D%7B0.1%7D%5C%5C%5C%5Cmass~ore%3D5000~g)
Conversion factor :
1 g = 0,00220462 pound, than for 5000 g = 11,02311 pounds
Somewhat of the same element, have same amount of protons but different number of neutrons. <span />