How many moles is 592.1 grams of LiCO3

8.84 mols LiCO3

Explanation:

We will have to find the molar mass of LiCO3, which we can use a periodic table.

Li: 6.97 g/mol

C: 12.01 g/mol

O: 48 g/mol (molar mass of O is 16, but we multiply it by 3)

Adding these values together will get our molar mass of LiCO3, which 66.98 g/mol.

Now we can use the molar mass of LiCO3 to convert the number of grams shown to the amount of mols we are trying to find.

Total moles of gas = 0.1225

Volume of gas produced : 6.7375 L

mass of Nitrogen : 0.588 g

Given

2 ml of Nitroglycerin(ρ=1.592 g/ml)

Required

Total moles of gas

Solution

Nitroglycerin detonated ⇒ decomposition reaction

4C₃H₅N₃O₉(s)⇒ 6N₂(g)+12CO(g)+10H₂O(g)+7O₂(g)

mass of Nitroglycerin :

moles of Nitroglycerin :

Total moles of gas:

Volume of gas produced :

moles of Nitrogen :

mass of Nitrogen :

Total moles of gas = 0.1225

Volume of gas produced : 6.7375 L

mass of Nitrogen : 0.588 g

Given

2 ml of Nitroglycerin(ρ=1.592 g/ml)

Required

Total moles of gas

Solution

Nitroglycerin detonated ⇒ decomposition reaction

4C₃H₅N₃O₉(s)⇒ 6N₂(g)+12CO(g)+10H₂O(g)+7O₂(g)

mass of Nitroglycerin :

moles of Nitroglycerin :

Total moles of gas:

Volume of gas produced :

moles of Nitrogen :

mass of Nitrogen :

Calcium (Ca)(On the periodic table, ionization energy increases as you go up and to the right of the periodic table)

glycoproteins

Explanation:

A positive reaction for Molisch's test is given by almost all carbohydrates (exceptions include tetroses & trioses). It can be noted that even some glycoproteins and nucleic acids give positive results for this test (since they tend to undergo hydrolysis when exposed to strong mineral acids and form monosaccharides).

Answer:

Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L.

An ideal gas is a theoretical gas that is considered to be composed of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:  

P×V = n×R×T

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas. The universal constant of ideal gases R has the same value for all gaseous substances.

Explanation:

In this case, you know:

P= 0.884 atm

V= ?

n= 0.857 moles (where 28 g/mole is the molar mass of N₂, that is, the amount of mass that the substance contains in one mole.)

R=0.082

T= 328 K

Replacing in the ideal gas law:

0.884 atm×V= 0.857 moles× 0.082 ×328 K

Solving:

V= 26.07 L

The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L.