Answer:
Explanation:
Hello,
In this case, for the given chemical reaction, we first identify the limiting reactant by noticing that due to the 1:1 mole ratio for magnesium to iodine the reacting moles must the same, nevertheless, there are only 2.68 moles of magnesium versus 3.56 moles of iodine, for that reason, magnesium is the limiting reactant, so the theoretical turns out:
Thus, we compute the percent yield as:
Best regards.
1.6726219 × 10-27 kilograms
(The -27 is a exponent)
<h2>The isotopes of an element all have the same __(atomic, mass) __number, but they have different __(atomic,mass)__numbers.</h2>
Explanation:
The isotopes of an element all have the same __atomic number __, but they have different __mass __numbers.
The isotopes have same atomic number that is :
- Same number of electrons
- Same number of protons
- same electronic configuration
- same valence electrons
- same valency
- same symbol
The isotopes have different mass number that is :
They differ in number of neutrons .
For example : Isotopes of hydrogen are : H₁¹ , H₁² , H₁³
isotopes of Oxygen is : O¹⁶ , O¹⁷, O¹⁸
Molar mass:
H₂O = 18.0 g/mol
O₂ = 32.0 g/mol
<span>C</span>₅<span>H</span>₁₂<span> + 8 O</span>₂<span> -> 5 CO</span>₂<span> + 6 H</span>₂<span>O
</span>
8 x (32 g ) ------------ 6 x (18 g )
mass O₂ ------------ 108 g H₂O
mass O₂ = 108 x 8 x 32 / 6 x 18
mass O₂ = 27648 / 108
mass O₂ = 256 g
hope this helps!
