All categories

3 years ago

Show your work including units in your answer. Calculate the molar mass of Li4OH

1 answer:

4 0

Empirical formula: Li4OH
Answer:
1 mole: 44.771 g
1 gram = 0.022 mole

Explanation:

Element: Li
Percentage by mass: 62.01%
Number of atoms: 4
Mass of atom;: 6.941

Element: O
Percentage by mass: 35.74%
Number of atoms: 1
Mass of atom: 15.9994

Element: H
Percentage by mass: 2.25%
Number of atoms: 1
Mass of atom: 1.00794

You might be interested in

ID = 801 720 6270 Pas = 1234 Jôîn frm zøôm app

icang [17]

Answer:

Explanation:

6 0

3 years ago

Drag the appropriate label under each illustration to identify the evolutionary mechanism at work. labels may be used more than

Alecsey [184]

Answer: Correct answers are- A. Gene flow B. Natural selection C. Natural selection D. Genetic drift E. Natural selection

6 0

4 years ago

Compare and contrast exothermic and endothermic

Vadim26 [7]

Exothermic is the release of heat. Exo as in exit to leave and thermos, the Greek word for heat. Endothermic is the absorption of heat. So if a chemical reaction is exothermic the reaction loses heat and it feels warm to you. If it is endothermic, it absorbs heat. If you are holding a beaker with an endothermic reaction, it will absorb the heat from you and therefore these re actions feel cool to touch!

3 0

4 years ago

Why do we need to balance chemical equations?

Mrrafil [7]

So we know the number of moles of each compound. If we need to know the concentration we must know the number of moles that the compounds react with...

8 0

4 years ago

Read 2 more answers

. Dimethyl nitrosamine is a known carcinogen. It can be formed in the intestinal tract when digestive juices react with the nitr

8090 [49]

Answer: The empirical formula for the given compound is $C_2H_6ON_2$

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

$C_xH_yN_z+O_2\rightarrow CO_2+H_2O$

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and nitrogen respectively.

We are given:

Mass of $CO_2=5.134g$

Mass of $H_2O=3.173g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 5.134 g of carbon dioxide, $\frac{12}{44}\times 5.134=1.4g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 3.173 g of water, $\frac{2}{18}\times 3.173=0.35g$ of hydrogen will be contained.

For calculating the mass of nitrogen:

As, 100 g of sample contains 37.87 % of nitrogen

So, 4.319 g of sample contains $\frac{37.87}{100}\times 4.319=1.635g$ of nitrogen

For calculating the mass of oxygen:

Mass of oxygen in the compound = (4.319) - (1.4 + 0.35 + 1.635) = 0.934 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{1.4g}{12g/mole}=0.116moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.35g}{1g/mole}=0.35moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{0.934g}{16g/mole}=0.058moles$

Moles of Nitrogen = $\frac{\text{Given mass of nitrogen}}{\text{Molar mass of nitrogen}}=\frac{1.635g}{14g/mole}=0.116moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.058 moles.

For Carbon = $\frac{0.116}{0.058}=2$

For Hydrogen = $\frac{0.35}{0.058}=6.03\approx 6$

For Oxygen = $\frac{0.058}{0.058}=1$

For Oxygen = $\frac{0.116}{0.058}=2$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O : N = 2 : 6 : 1 :2

Hence, the empirical formula for the given compound is $C_2H_6O_1N_2=C_2H_6ON_2$

8 0

4 years ago