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charle [14.2K]
3 years ago
12

Determine which decay process is being described in each case. the atomic number deceases by one, and the atomic mass is unchang

ed. the atomic number decreases by two, and the atomic mass decreases by four. the atomic number increases by one, and the atomic mass remains unchanged.
Chemistry
2 answers:
Sav [38]3 years ago
8 0
1. The atomic number deceases by one and the atomic mass is unchanged - β⁺/positron emission. In this a proton is converted to a neutron, hence no net change in mass. Since a proton is converted to neutron, the daughter nuclide's proton number /atomic number decreases by 1. Then atomic number decreases by 1 and no change in mass.

2.the atomic number decreases by two, and the atomic mass decreases by four - alpha decay / ⁴₂α. alpha particles have 2 neutrons and 2 protons. Since 2 protons and 2 neutrons are emitted, the mass of the nuclide decreases by 4. Since 2 protons have been emitted, this results in atomic number decreasing  by 2.

3.<span>the atomic number increases by one, and the atomic mass remains unchanged. - </span>β⁻ beta decay. In this type of decay - beta decay , a neutron is converted to a proton, therefore no net change in mass. Since a proton is formed, atomic number increases by 1. Therefore atomic number increases by 1 and no change in mass.
swat323 years ago
8 0

Determine which decay process is being described in each case.

The atomic number deceases by one, and the atomic mass is unchanged.      

beta-plus decay

The atomic number decreases by two, and the atomic mass decreases by four.      

alpha-decay

The atomic number increases by one, and the atomic mass remains unchanged.      

beta-minus decay

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The molecular formula of the unknown compound is determined as  C₉H₁₁NO₂.

<h3>Molecular formula of the compound</h3>

The molecular formula is calculated as follows;

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Mass of carbon, C:  = (6.64 x 12)/44 = 1.81 g in 2.77 g sample

Mass of hydrogen, H: = (1.67 x 2)/18 = 0.186 g in 2.77 g sample

Mass of Nitrogen, N: = (2.77 x 0.143)/1.69 = 0.234 g

Mass of oxygen, O:  = 2.77 g - 1.81 g - 0.186 g - 0.234 g = 0.54 g

<h3>molar ratio of the elements: </h3>

C = 1.81 g = 0.15 mol

H = 0.186 g = 0.186 mol

N = 0.234 g = 0.017 mol

O = 0.54 g = 0.0337 mol

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Check the molar mass of the compound = (9 x 12) + (11 x 1) + (14) + (2 x 16) = 165 g/mol

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⇒with m(water) = the mass of the water = 250.0 grams

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