All categories

3 years ago

What occurs in combustion reaction? Explain

Chemistry

1 answer:

Shtirlitz [24]3 years ago

6 0

Answer:

In a combustion reaction, a substance reacts with oxygen from the air. Combustion reactions happen at high temperatures, and transfer energy to the surroundings as light and heat. This is why you see flames when things burn. ... The products of combustion reactions are compounds of oxygen, called oxides.

You might be interested in

Sediment spreads horizontality and it goes from youngest on top to oldest on bottom. When sediment deposits in water, it also sp

Ad libitum [116K]

My answer will be C. Law of Original lateral continuity. :)

7 0

3 years ago

Read 2 more answers

Explain how you would determine the volume of a powdered solid, a liquid, and a rock

siniylev [52]

To determine the volume you would need to find the density and mass of each.

3 0

3 years ago

Read 2 more answers

Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is comple

Kazeer [188]

Answer:

The ionic bond in NaCl are stronger than the stronger than the dispersion forces in HCl.

The hydrogen bonds in H2O are stronger than the dispersion forces in H2Se

Hydrogen bonds in NH3 are stronger than the dipole-dipole attractions in PH3.

Hydrogen bonds in HF are stronger than the dispersion forces in F2

Explanation:

Ionic bonds occur in molecules with high differences in their electronegative value where there are actual transfer of electrons. HCl has a bond which is involved in the sharing of electrons.

Hydrogen bonds are present in H2O which is stronger than the dispersion forces.

PH3 is a larger molecule with greater dispersion forces than ammonia, NH3 has very polar N-H bonds leading to strong hydrogen bonding. This dominant intermolecular force results in a greater attraction between NH3 molecules than there is between PH3 molecules.

F2 is a non-polar molecule, therefore they have London dispersion forces between molecules while HF has a hydrogen bond because F is highly electronegative.

7 0

3 years ago

etermine the molar concentration of magnesium ions in a solution formed by mixing 100.0 mL of 0.100 M MgCl, solution with 100.0

marysya [2.9K]

Answer:

Molar concentration of magnesium ions in the final solution is 0.2 M.

Explanation:

$c=\frac{n}{V}$

c = Concentration of the solution

n = moles of the compound

V = volume of the solution in L

1) Molarity of $MgCl_2$ solution = 0.100 M

Volume of $MgCl_2$ solution = 100.0 mL = 0.1 L

Moles of $MgCl_2$ in 100 mL solution= n

$0.100 M=\frac{n}{0.1L}$

$n=0.01 mol$

$MgCl_2(aq)\rightarrow Mg^{2+}(aq)+2Cl^-(aq)$

1 mole of magnesium chloride gives 1 mol of magnesium ions and 2 moles of chloride ions.

Then 0.01 moles of magnesium chloride will give:

$x=\frac{1}{1}\times 0.01 mol=0.01 mol$ magnesium ions.

2) Molarity of $Mg_3(PO_4)_2$ solution = 0.100 M

Volume of $Mg_3(PO_4)_2$ solution = 100.0 mL = 0.1 L

Moles of $Mg_3(PO_4)_2$ in 100 mL solution= n'

$0.100 M=\frac{n'}{0.1L}$

$n'=0.01 mol$

$Mg_3(PO_4)_2(aq)\rightarrow 3Mg^{2+}(aq)+2PO_{4}^-(aq)$

1 mole of magnesium phosphate gives 3 mol of magnesium ions and 2 moles of phosphate ions.

Then 0.01 moles of magnesium phosphate will give:

$y=\frac{3}{1}\times 0.01 mol=0.03 mol$ magnesium ions.

After mixing both solutions:

Moles of magnesium ions = x + y = 0.01 mol + 0.03 mol = 0.04 mol

Total volume after mixing = 0.1 L + 0.1 L = 0.2 L

Molar concentration of magnesium ions in the final solution: $[Mg^{2+}]$

$[Mg^{2+}]=\frac{0.04 mol}{0.2 L}=0.2 mol/L$

4 0

4 years ago

What is the boiling point of a solution of 76 g of water dissolved in 500 mL of acetic acid, CH3COOH?

tatuchka [14]

Answer:

127.3° C, (This is not a choice)

Explanation:

This is about the colligative property of boiling point.

ΔT = Kb . m . i

Where:

ΔT = T° boling of solution - T° boiling of pure solvent

Kb = Boiling constant

m = molal (mol/kg)

i = Van't Hoff factor (number of particles dissolved in solution)

Water is not a ionic compound, but we assume that i = 2

H₂O → H⁺ + OH⁻

T° boling of solution - 118.1°C = 0.52°C . m . 2

Mass of solvent = Solvent volume / Solvent density

Mass of solvent = 500 mL / 1.049g/mL → 476.6 g

Mol of water are mass / molar mass

76 g / 18g/m = 4.22 moles

These moles are in 476.6 g

Mol / kg = molal → 4.22 m / 0.4766 kg = 8.85 m

T° boling of solution = 0.52°C . 8.85 m . 2 + 118.1°C = 127.3°C

6 0

3 years ago

Read 2 more answers