1 part per million is the same as
<span>1 mcg/mL (mcg = 1 micro gram = 1 * 10^-6 grams). </span>
<span>125 ppm = 125 mcg/mL </span>
<span>125 mcg/ml * [1 gram / 1 * 10^6 mgrm] = 1.25 * 10^-4 grams </span>
<span>The density of hard water is 1.000 grams / mL </span>
<span>50 mL of water contains 1.25 * 10^-4 grams. </span>
<span>given mass = 1.25 * 10^-4 </span>
<span>Molar mass = 100.0 grams / mole </span>
<span>n = ????? </span>
<span>n = 1.25 * 10^-4/100 = 1.25 * 10^-6 moles.
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Answer:
.67 L
Explanation:
.030 mol x 22.4 L / 1 mol = .67 L
22.4 was used because that is what 1 mol equals for a gas at stp.
A O-18 has 2 more neutrons than O-16
<h3>Further explanation</h3>
Oxygen is located in group 16 in the p block which has the atomic number 8
In the atomic symbol (neutral), the atomic number indicates the number of electrons and protons. while the number of neutrons is obtained from the difference between the mass number and the atomic number.
The isotope will have the same number of protons (atomic number) but a different mass number
Isotopes of oxygen include: O-18 and O-16
Here we have to get the temperature and pressure at which helium gas mostly behaves as ideal gas.
Helium (He) behave most like an ideal gas upto 24K temperature and 0 atm pressure.
The deviation of a real gas to ideal gas occurs at high temperature and low pressure.
The deviation of ideal gas to real gas occurs on taking into account the van der waals' force of attraction between the gas molecules. Now, the van der waals' interaction depends upon the polarisibility of the gas molecule.
As helium (He) is non-polarisable and very small (atomic number 2) it mostly behaves as ideal gas upto 24K temperature and 0 atm pressure.
Although the deviation from the ideal gas behavior to real gas is not so prominent at little high temperature also. Upto 50K it mostly behaves like an ideal gas.
