Write the symbolic notation of an isotope of an element having 8 protons, 8 electrons, and 11 neutrons. Click on the “Templates”
button template button and make use of the "stacked super/subscript" button button for entering stackes super/subscripts for entering the mass number and atomic number of the isotope. Express your answer as an isotope.
1 answer:
Attached to this answer is the format of Isotope Notation that you can use for future reference. <em>(Please open)</em>
There are 8 Protons. The Atomic Number is the same number of an element's proton.
If you can see in the format, the mass number is calculated by adding the atomic number/protons and neutrons.
Mass number = 8 + 11
Mass number = 19
The image of the final answer is attached as well.
There are 8 Protons. The Atomic Number is the same number of an element's proton.
If you can see in the format, the mass number is calculated by adding the atomic number/protons and neutrons.
Mass number = 8 + 11
Mass number = 19
The image of the final answer is attached as well.
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Explanation:
The given reaction is as follows.
a). Molar mass of is [(mass of Sn) + (2 × mass of O)].
Therefore, molar mass of = (118.7 + 2 × 16) g/mol = 150.7 g/mol
Since, it is known that number of moles equal mass divided by molar mass. So, moles of Sn will be calculated as follows.
No. of moles =
=
= 2.53 mol
As it is given that 1 mole of produces 1 moles of Sn and 1 moles of
. Hence, 2.53 moles of
will also produce 2.53 moles of Sn and 2.53 moles of
.
Volume of 1 mole of at STP is 22.4 L. Therefore, volume of 2.53 moles of
will be calculated as follows.
2.53 × 22.5 L = 56.67 L
Hence, 56.67 L of are produced if 300.0 grams of tin are produced at STP.
b). Mass of tin is given as 1800.0 g. So, number of moles will be calculated as follows.
No. of moles =
=
= 15.2 moles
As 15.2 moles of produces 15.2 moles of Sn. Therefore, weight of
will be calculated as follows.
Mass = no. of moles × molar mass of
= 15.2 moles × 150.7 g/mol
= 2290.64 g
Hence, 2290.64 grams of are required to produce 1800.0 grams of tin.
c). Mass of carbon given is 100.0 grams.
No. of moles =
=
= 8.33 moles
As, 1 mole of carbon is produced by 1 mole of tin. So, 8.33 mole of carbon will be produced by 8.33 moles of tin.
Therefore, calculate mass of tin produced as follows.
Mass = no. of moles × molar mass of Sn
= 8.33 moles × 118.7 g/mol
= 988.8 g
Hence, 988.8 grams of tin will be produced per 100 grams of carbon used.