<span>These are the rules of the quantum numbers that you have to use to dilucidate the validity of a set of quantum numbers:
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<span>1) Main quantum number, n: 1, 2, 3, 4, 5, 6, 7
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2) Second quantum number, ℓ: 0, 1, 2, ... n-1
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<span>3) Third quantum number (magnetic quantum number), mℓ: -l,...0,,,,+l
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<span>4) Fourth quantum number (spin): ms: +1/2 or -1/2
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Answers:
<span>i) 3,2,0,1/2: valid, because 0<= l < n; - l <= ml <= +l; and ms = +1/2 or -1/2
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</span><span>ii) 2,2,-1, 1/2 invalid because l = n (violates second rule)</span><span /><span>
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</span><span>iii) 4,3,-4,1/2 invalid because ml is less than - l (violates third rule)</span><span /><span>
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</span><span>iv) 1,0,0,1/2 valid: meet the four rules</span><span /><span>
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</span><span>v) 2,2,1,-1/2 invalid because l = n (violate the second rule)</span><span /><span>
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</span><span>vi) 3,2,1,1 invalid because ms can be only +1/2 or -1/2 (fourth rule)
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<span /><span /><span>vii) 0,1,1,-1/2 invalid because l > n (violates rule 2)
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<span /><span /><span>viii) 3,3,1,1/2 invalid because l = n (violate rule 2)
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<span /><span /><span>ix) 2,-2,-2,-1/2 invalid because l is negative (violates rule 2)
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x)<span> 3,2,2,1/2 valid: meet the four rules</span>
xi)<span> 4,2,1,1/2 valid: meet the four rules</span>
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</span><span>xii) 2,1,-1,-1/2 valid meet the four rules</span>
The molar mass of the gas with the given mass and volume at the given temperature and pressure is 16.00g/mol.
<h3>What is the molar mass of the gas?</h3>
From the Ideal gas law or general gas equation;
PV = nRT
Where P is pressure, V is volume, n is the amount of substance, T is temperature and R is the ideal gas constant ( 0.08206 Latm/molK )
Given that;
- Temperature T = 21°C = (21 + 273.15)K = 294.15K
- Pressure P = 745 mmHg = (745/760)atm = 0.98026atm
- Volume of the gas V = 3.97L
- Mass of gas m = 2.58g
First, we determine the amount of gas;
PV = nRT
n = PV / RT
n = ( 0.98026atm × 3.97L ) / ( 0.08206 Latm/molK × 294.15K )
n = 3.8916Latm / (24.137949Latm/mol)
n = 0.1612mol
Molar Mass = Mass of the gas / Amount of the gas
Molar Mass = m / n
Molar Mass = 2.58g / 0.1612mol
Molar Mass = 16.00g/mol
Therefore, the molar mass of the gas with the given mass and volume at the given temperature and pressure is 16.00g/mol.
Learn more about ideal gases here: brainly.com/question/15634266
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Answer:
1.209g of MgO participates
Explanation:
In this problem, we have 0.030 moles of MgO that participates in a particular reaction.
And we are asked to solve for the mass of MgO that participates, that means, we need to convert moles to grams.
To convert moles to grams we need to use molar mass of the compound:
<em>1 atom of Mg has a molar mass of 24.3g/mol</em>
<em>1 atom of O has a molar mass of 16g/mol</em>
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That means molar mass of MgO is 24.3g/mol + 16g/mol = 40.3g/mol
And mass of 0.030 moles of MgO is:
0.030 moles MgO * (40.3g/mol) =
<h3>1.209g of MgO participates</h3>