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1 year ago

How many hydrogen bonds can CH2O make to water

1 answer:

5 0

Hydrogen bonds are not like covalent bonds. They are nowhere near as strong and you can't think of them in terms of a definite number like a valence. Polar molecules interact with each other and hydrogen bonds are an example of this where the interaction is especially strong. In your example you could represent it like this:

H2C=O---------H-OH 

But you should remember that the H2O molecule will be exchanging constantly with others in the solvation shell of the formaldehyde molecule and these in turn will be exchanging with other H2O molecules in the bulk solution. 

Formaldehyde in aqueous solution is in equilibrium with its hydrate. 

H2C=O + H2O <-----------------> H2C(OH)2

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What is the mass (in grams) of 8.45 x 1023 molecules of dextrose: C6H12O6 (Mw. 180.16 g/mol)?

Goryan [66]

The mass (in grams) of 8.45 x 10^23 molecules of dextrose is 252.798g Working: Mw. dextrose is 180.16 g/mol therefore 180.16 grams dextrose = 1 mole therefore 180.16 grams dextrose= 6.022x10^23 molecules (Avogadro's number) We have 8.45 x 10^23 molecules of dextrose. Therefore, (180.16 divided by 6.022x10^23) times 8.45x10^23 gives the mass (in grams) of 8.45 x 10^23 molecules of dextrose; 252.798.

4 0

1 year ago

Aluminum metal and bromine liquid (red) react violently to make aluminum bromide (white powder). One way to represent this equil

Illusion [34]

Answer:

Part A

K = (K₂)²

K = (K₃)⁻²

Part B

K = √(Ka/Kb)

Explanation:

Part A

The parent reaction is

2Al(s) + 3Br₂(l) ⇌ 2AlBr₃(s)

The equilibrium constant is given as

K = [AlBr₃]²/[Al]²[Br₂]³

2) Al(s) + (3/2) Br₂(l) ⇌ AlBr₃(s)

K₂ = [AlBr₃]/[Al][Br₂]¹•⁵

It is evident that

K = (K₂)²

3) AlBr₃(s) ⇌ Al(s) + 3/2 Br₂(l)

K₃ = [Al][Br₂]¹•⁵/[AlBr₃]

K = (K₃)⁻²

Part B

Parent reaction

S(s) + O₂(g) ⇌ SO₂(g)

K = [SO₂]/[S][O₂]

a) 2S(s) + 3O₂(g) ⇌ 2SO₃(g)

Ka = [SO₃]²/[S]²[O₂]³

[SO₃]² = Ka × [S]²[O₂]³

b) 2SO₂(g) + O₂(g) ⇌ 2 SO₃(g)

Kb = [SO₃]²/[SO₂]²[O₂]

[SO₃]² = Kb × [SO₂]²[O₂]

[SO₃]² = [SO₃]²

Hence,

Ka × [S]²[O₂]³ = Kb × [SO₂]²[O₂]

(Ka/Kb) = [SO₂]²[O₂]/[S]²[O₂]³

(Ka/Kb) = [SO₂]²/[S]²[O₂]²

(Ka/Kb) = {[SO₂]/[S][O₂]}²

Recall

K = [SO₂]/[S][O₂]

Hence,

(Ka/Kb) = K²

K = √(Ka/Kb)

Hope this Helps!!!

6 0

1 year ago

identify the element in period 3 that requires the least amount of energy to remove the most loosely held electrons from a mole

OLga [1]

Answer:

The element is Na

Explanation:

Ionization energy is the energy needed to release the last electron from an atom in its ground state to the gaseous state. It is a periodic property that increases as we go through the periods of the periodic table, but decreases if we move in groups. Sodium has thr ionic radius (another periodic property) that is too large, making it easier to release the electron away, since it is too far from the nucleus.

3 0

1 year ago

Small quantities of h2 gas can be collected by adding hcl to zn. a sample of 195 ml of h2 gas was collected over water at 25 c a

Umnica [9.8K]

15.4 milligrams The ideal gas law is PV = nRT where P = pressure of the gas V = volume of the gas n = number of moles of gas R = Ideal gas constant (8.3144598 L*kPa/(K*mol) ) T = absolute temperature. So let's determine how many moles of gas has been collected. Converting temperature from C to K 273.15 + 25 = 298.15 K Converting pressure from mmHg to kPa 753 mmHg * 0.133322387415 kPa/mmHg = 100.3917577 kPa Taking idea gas equation and solving for n PV = nRT PV/RT = n n = PV/RT Substituting known values n = PV/RT n = (100.3917577 kPa 0.195 L) / (8.3144598 L*kPa/(K*mol) 298.15 K) n = (19.57639275 L*kPa) / (2478.956189 L*kPa/(mol) ) n = 0.007897031 mol So we have a total of 0.007897031 moles of gas particles. Now let's get rid of that percentage that's water vapor. The percentage of water vapor is the vapor pressure of water divided by the total pressure. So 24/753 = 0.03187251 The portion of hydrogen is 1 minus the portion of water vapor. So 1 - 0.03187251 = 0.96812749 So the number of moles of hydrogen is 0.96812749 * 0.007897031 mol = 0.007645332 mol Now just multiple the number of moles by the molar mass of hydrogen gas. Start with the atomic weight. Atomic weight hydrogen = 1.00794 Molar mass H2 = 1.00794 * 2 = 2.01588 g/mol Mass H2 = 2.01588 g/mol * 0.007645332 mol = 0.015412073 g Rounding to 3 significant figures gives 0.0154 g = 15.4 mg

7 0

2 years ago

Read 2 more answers

An ecosystem now receives far less rain than it used to. The weather also became drier and hotter. Over time, plants with struct

Vadim26 [7]

The plants of this ecosystem were influenced by the change of abiotic factors (climate).
The plants who had these specialized structures that have helped them conserve water and adapt to these new environmental conditions were more successful, and left more offspring.After several generations, the specialized plants became more prevalent.
Since there was a selection of successful individuals trough generations, we can conclude that this was due to the working of the evolutionary mechanism called the natural selection.

5 0

1 year ago