The intermolecular forces, such as hydrogen bonds or van der Waals attractions, which draw one molecule to its neighbors, govern a substance's physical properties. Due to the relatively weak intermolecular forces of attraction, molecular substances typically take the form of gases, liquids, or low melting point solids.
<h3>How do the intermolecular forces affect physical properties?</h3>
The forces that bind two molecules together are known as intermolecular forces. Intermolecular forces have an impact on physical properties. Strong and weak forces both exist; the stronger the force, the more energy is needed to separate the molecules from one another. As intermolecular forces increase melting, boiling, and freezing points rise.
The following intermolecular forces are listed in order of strength:
- Van der Waals dispersion forces
- Van der Waals dipole-dipole interactions
- Hydrogen bonding
- Ionic bonds
It would take very little energy to separate two molecules if they are connected by van der Waals dispersion forces. On the other hand, it requires a lot more energy to separate two molecules that are joined together by ionic bonds.
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<u>Answer:</u> The amount of hydrogen sulfide needed is 6.2 moles and amount of sulfur dioxide gas produced is 6.2 moles
<u>Explanation:</u>
We are given:
Moles of oxygen gas = 9.3 moles
The chemical equation for the reaction of oxygen gas and hydrogen sulfide follows:
<u>For hydrogen sulfide:</u>
By Stoichiometry of the reaction:
3 moles of oxygen gas reacts with 2 moles of hydrogen sulfide
So, 9.3 moles of oxygen gas will react with = of hydrogen sulfide
<u>For sulfur dioxide:</u>
By Stoichiometry of the reaction:
3 moles of oxygen gas produces 2 moles of sulfur dioxide
So, 9.3 moles of oxygen gas will produce = of sulfur dioxide
Hence, the amount of hydrogen sulfide needed is 6.2 moles and amount of sulfur dioxide gas produced is 6.2 moles
1) Balance of mass
CxHyOz + O2 ---> CO2 + H20
0.880 g + X = 1.760g + 0.720 g
=> X = 1.760g + 0.720g - 0.880g = 1.6 g of O2
2) C in CO2:
molar mass of CO2 = 44 g/mol
=> 12 g C / 44 g CO2 * 1.760 g CO2 = 0.480 g C
3) H in H2O
molar mass of H2O = 18.0 g/mol
2 g H / 18.0 g H2O * 0.720 g H2O = 0.080 g H
4) O
4a) O in CO2: 32gO / 44 g CO2 * 1.760 g CO2 = 1.280 g O
4b) O in H2O: 16gO / 18 gH2O * 0.720 g H2O = 0.640 g O
4c) O in CxHyOz = 1.280 g + 0.64 g - 1.6 g = 0.320 g O
5) Convert grams into moles
C: 0.480 g / 12 g/mol = 0.04 mol
H: 0.08 g / 1 g/mol = 0.08 mol
O: 0.32 g / 16 g/mol = 0.02 mol
6) Divide by the smallest number
C: 0.04 / 0.02 = 2
H: 0.08 / 0.02 = 4
O: 0.02 / 0.02 = 1
7) Use those numbers as subscripts for the empirical formula:
C2 H4 O
Answer: C2H4O
Li2CO3 + Ca3(PO4)2 = Li3PO4 + CaCO3
Answer:
21.182 g
Explanation:
There are about (6.0)(10^23) atoms in one mole of a substance, so the given sample has about 0.333 mol of Cu.
The atomic mass of Cu is 63.546 g/mol, meaning that the answer is about <u>21.182</u><u> </u><u>g</u>