Determine the identity of the daughter nuclide from the electron capture by 3517cl. determine the identity of the daughter nucli
1 answer:
Answer:
Explanation:
When the nucleus of an <em>atom captures and electron</em>, such electron combines with a proton and forms a neutron. Thus, the mass number remains the same (just a proton has been converted into a neutron) but the atomic number (the number of protons) decrease in one.
Then, the daughter nuclide will have the same mass number and the atomic number reduced in one.
The given parent isotope is , which means that it has these features:
- Chemical symbol: Cl
- Name of the element: chlorine
- Mass number (the superscript to the left): 35
- Atomic number (the subscript to the left): 17
And the daughter nuclide after the electron capture will be:
- Mass number: 35 (the same of the parent nuclide)
- Atomic number: 17 - 1 = 16
- Identity: sulfur (search the element with atomic number 16 in a periodic table).
- Chemical symbol: S
- Idenity of the daughter nuclide using the isotope notation:
Hence, the answer is the third choice.
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Answer:
The amount of heat to absorb is 6,261 J
Explanation:
Calorimetry is in charge of measuring the amount of heat generated or lost in certain physical or chemical processes.
The total energy required is the sum of the energy to heat the ice from -20 ° C to ice of 0 ° C, melting the ice of 0 ° C in 0 ° C water and finally heating the water to 60 ° C.
So:
- Heat required to raise the temperature of ice from -20 °C to 0 °C
Being the sensible heat of a body the amount of heat received or transferred by a body when it undergoes a temperature variation (Δt) without there being a change of physical state (solid, liquid or gaseous), the expression is used:
Q = c * m * ΔT
Where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation (ΔT=Tfinal - Tinitial).
In this case, m= 10 g, specific heat of the ice= 2.1 and ΔT=0 C - (-20 C)= 20 C
Replacing: Q= 10 g*2.1 *20 C and solving: Q=420 J
- Heat required to convert 0 °C ice to 0 °C water
The heat Q necessary to melt a substance depends on its mass m and on the called latent heat of fusion of each substance:
Q= m* ΔHfusion
In this case, being 1 mol of water= 18 grams: Q= 10 g*= 3.333 kJ= 3,333 J (being kJ=1,000 J)
- Heat required to raise the temperature of water from 0 °C to 60 °C
In this case the expression used in the first step is used, but being: m= 10 g, specific heat of the water= 4.18 and ΔT=60 C - (0 C)= 60 C
Replacing: Q= 10 g*4.18 *60 C and solving: Q=2,508 J
Finally, Qtotal= 420 J + 3,333 J + 2,508 J
Qtotal= 6,261 J
<u><em> The amount of heat to absorb is 6,261 J</em></u>
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