The number of protons found in the nucleus equals the number of electrons that surround it, giving the atom a neutral charge (neutrons have zero charge). Most of an atom's mass is in its nucleus; the mass of an electron is only 1/1836 the mass of the lightest nucleus, that of hydrogen.Hoped this helped
You have to use Dalton's law of partial pressure for this question. Dalton's law of partial pressure basically states that the total pressure of the system is all of the partial pressures of the components added together. Therefore to answer the question you just need to add all the patial pressures together meaning that the total pressure would be 700+500+500=1700.
The answer would be 1700 torr.
I hope this helps. Let me know if anything is unclear or if you have any further questions.
Answer: There is a single covalent bond in a chlorine molecule.
Explanation: The chlorine molecule is represented as Cl−Cl, i.e. C
l2. Between the chlorine atoms, 2 electrons overlap to form a region of high electron density to which the positively charged chlorine nuclei are attracted, such that internuclear repulsion is negated and a net attractive force results. Because the bonding electrons are shared between the nuclei, we conceive that each atom has 8 valence electrons.
Of course, on reaction with sodium, the sodium reduces the chlorine molecule to give 2×Cl−. The resultant bond between Na+ and Cl−is ionic and a non-molecular substance results.
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I think it is True because the SI unit is <span>J/°C</span>
Answer:
The partial pressure of Ar is 356.04 mm Hg (= 0.4685 atm)
Explanation:
<u>Step 1:</u> Data given
A mixture of three gases has a total pressure of 1380 mm Hg (=1.81579 atm) at 298 K
Moles of CO2 = 1.27 moles
Moles of CO = 3.04 moles
Moles of Ar = 1.50 moles
<u>Step 2:</u> Calculate total number of moles
Total number of moles = n(CO2)+ n(CO)+ n(Ar) = 1.27 mol+ 3.04 mol+ 1.50 mol = 5.81 moles
<u>Step 3:</u> Calculate mol fraction Ar
Mol fraction Ar = 1.50 mol/5.81 mol = 0.258
<u>Step 4</u>: Calculate partial pressure
1380 mm Hg * 0.258 moles Ar = 356.04 mm Hg = 0.4685 atm
The partial pressure of Ar is 356.04 mm Hg (= 0.4685 atm)
