Chemistry College

For the following equation, assume you started with 15.6g potassium (K). How many moles of potassium oxide would be produced assuming you had unlimited oxygen? ____ K + ____ O2 → _____ K2O

Answers

Answer 1

According to the stoichiometry of the given chemical equation, 0.2 moles of potassium oxide would be produced assuming you had unlimited oxygen.

What is stoichiometry?

Stoichiometry is defined as   the determination of proportions of elements or compounds in a chemical reaction. The  relations are based on law of conservation of mass and law of combining weights and volumes.

Stoichiometry is used in quantitative analysis for measuring concentrations of substances present in the sample.

In the given equation,156 g potassium gives 188.4 g potassium oxide, thus, 15.6 g will give 15.6×188.4/156=18.84 g potassium oxide which is 18.84/94.2= 0.2 moles.

Thus, 0.2 moles of potassium oxide would be produced assuming you had unlimited oxygen.

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Related Questions

Which characteristic is not a periodic trend?


A. Atomic radius


B. Electron affinity


C. Ionization energies


D. Number of elements in a group

Answers

Answer:

Explanation:

D

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Given the following equation: 2N₂+502 → 2N₂O5
How many moles of N₂O5 are produced by reacting 10 moles of O₂?

Answers

Mole Ratios and Stoichiometry

We can form mole ratios by using a balanced chemical equation.

Solving the Question

[tex]2N_2+5O_2\rightarrow 2N_2O_5[/tex]

2 moles of [tex]N_2O_5[/tex] can be formed with 5 moles of [tex]O_2[/tex]:

[tex]\dfrac{n_{N_2O_5}}{2}=\dfrac{n_{O_2}}{5}[/tex]

We're given that we have 10 moles of [tex]O_2[/tex]:

[tex]\dfrac{n_{N_2O_5}}{2}=\dfrac{10}{5}[/tex]

[tex]n_{N_2O_5}=4[/tex]

Answer

4 moles of N2O4 are produced by reacting 10 moles of O2.

As per the balanced equation of the reaction, 5 moles of oxygen molecule gives 2 moles of the product N₂O₅ . Hence, 10 moles of oxygen will give 4 moles of nitrogen pentoxide.

What is mole ratio ?

The balanced chemical equation of a reaction represents the perfect stoichiometry of the reactants and products. Hence, the number of atoms of each element in the reactant side must be equal to their number of atoms in the product side.

The stochiometric ratio of number of moles of one reactant to the other or the product is called its mole ratio.

From the given reaction, it is clear that 5 moles of oxygen molecules reacts with nitrogen gas to give 2 moles of dinitrogen pentoxide.

Hence, the number of moles of dinitrogen pentoxide produced by 10 moles of oxygen gas is calculated as follows:

(10× 2)/5 = 4

Therefore, the number of moles of the product formed from 10 moles of oxygen gas is 4 moles.

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Determine the empirical formula of a compound containing 47. 37 grams of carbon, 10. 59 grams of hydrogen, and 42. 04 grams of oxygen.

Answers

the empirical formula of a compound containing 47. 37 grams of carbon, 10. 59 grams of hydrogen, and 42. 04 grams of oxygen is C3H8O2.

To determine the empirical formula of the compound, we need to find the ratios of the different elements present in the compound.

The first step is to convert the masses of each element to moles using their respective molar masses:

Carbon: 47.37 g / 12.01 g/mol = 3.94 mol

Hydrogen: 10.59 g / 1.01 g/mol = 10.48 mol

Oxygen: 42.04 g / 16.00 g/mol = 2.63 mol

Next, we divide each of the mole values by the smallest of the three, which is 2.63 mol:

Carbon: 3.94 mol / 2.63 mol = 1.50

Hydrogen: 10.48 mol / 2.63 mol = 3.98

Oxygen: 2.63 mol / 2.63 mol = 1.00

Now we need to convert these ratios to whole numbers by multiplying each by a common factor. The smallest ratio is 1.00, so we will multiply all the ratios by 2 to get:

Carbon: 1.50 x 2 = 3

Hydrogen: 3.98 x 2 = 8

Oxygen: 1.00 x 2 = 2

Therefore, the empirical formula of the compound is C3H8O2.

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