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3 years ago

Starting with 195 g Li2O and 106 g H2O, decide which reactant is present in limiting quantities. Given: Li2O+H2O→2LiOH

1 answer:

4 0

Taking into account the stoicionetry reaction and the definition of limiting reagent, Li₂O is present in limiting quantities.

The balanced reaction is:

Li₂O + H₂O → 2 LiOH

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

Li₂O: 1 mole
H₂O: 1 mole
LiOH: 2 moles

The molar mass of each compound is:

Li₂O: 29.88 g/mole
H₂O: 18 g/mole
LiOH: 23.95 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

Li₂O: 1 mole× 29.88 g/mole= 29.88 g
H₂O: 1 mole× 18 g/mole= 18 g
LiOH: 2 moles× 23.95 g/mole= 47.9 g

On the other side, the limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

To determine the limiting reagent, it is possible to use a simple rule of three as follows: if by stoichiometry 18 grams of H₂O reacts with 29.88 grams of Li₂O, 106 grams of H₂O react with how much mass of Li₂O?

$mass of Li_{2} O=\frac{29.88 grams of Li_{2} Ox106 grams of H_{2} O}{18 grams of H_{2} O}$

mass of Li₂O= 175.96 grams

But 175.96 grams of Li₂O are not available, 195 grams are available. Since you have less moles than you need to react with 106 grams of H₂O, Li₂O will be the limiting reagent.

Finally, Li₂O is present in limiting quantities.

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3 years ago

What mass of oxygen reacts when 84.9 g of iron is consumed in the following reaction: Fe+O2= Fe2O3

konstantin123 [22]

First we will calculate the number of moles of Iron:
$n = \frac{m}{M}
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$n= \frac{84.9}{55.845} = 1,52$ moles of Iron.
The same number of moles of Oxygen will take part in the reaction.
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The electron configuration can be also be represented by writing the symbol for the occupied subshell and adding a superscript t

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Answer: The electron configuration of carbon atom is written as 1s²,2s², 2p².

Explanation:

The electronic configuration of an atom is defined as the arrangement of electrons into the shells or orbit of an atom. The constituents of an atom are proton, neutron and electron. the nucleus of an atom, where most of its mass are concentrated, consists of neutrons and protons fused together. Electrons occupy the shells surrounding the nucleus. The shells are lettered K, L, M, N and so on. Numerically, K shell is numbered 1, L is 2 and so on. These numbers also correspond with the increase in the energy level. All the electrons in K shell for instance belong to the first energy level and they have equal energy.

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These shells are further subdivided into subshells. There are 4 subshells, s, p, d, and f. Each subshell can hold a different number of electrons.

This electron configuration of carbon can be written as 1s² 2s² 2p² where 1s, 2s, and 2p are the occupied subshells, and the superscript "2" is the number of electrons in each of these subshells.

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