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11Alexandr11 [23.1K]

3 years ago

6

If you take energy away from oxygen, will it turn into water? If not, then what will turn into water if you take away energy fro

m it?

1 answer:

myrzilka [38]3 years ago

3 0

Take heat away from oxygen and it becomes liquid oxygen. Take heat away from steam and it becomes liquid water.

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PLEASE HELP NEED THIS TO PASS!!!

nadya68 [22]

(1)

At phase A, the water is fully solid, At phase C the water is fully liquid and at phase E the water is fully gas. At this ponts all the substance is in one state other than the fact that its molecules are getting more excited as they gain more energy. This is why there is an increase in temperatures. At the transition points water is changing phase and therefore at any point in between the transition not all water will be in the same phase.

(2)

Point F

This is because the solid water stops rising in temperatures and begins changing phase into liquid water. This is the highest temperatures that the solid water can attain without turning into liquid. You can see from the graph that the temperatures rise at this point levels off between point F and G

(3)

Point H

This is because the liquid water stops rising in temperatures and begins changing phase into gaseous form. This is the highest temperatures that the liquid water can attain without turning into gas/water vapor. You can see from the graph that the temperatures rise at this point levels off between point H and I.

(4)

The energy is increasing

You can see from the graph that energy is being absorbed by the water (due to increases in energy on the x-axis on the graph) but there is no corresponding rise in temperatures in y-axis. This means the energy begin absorbed is being used to change the phase of the water.

(5)

The water is changing phases

Because the energy absorbed is being used to change the phase of the liquid. The energy is being used to break the bonds between the molecules so the molecules become farther apart and causing a change in phase on the water. Therefore the vibrational moments of the molecules (responsible for rising in temperatures) remain the same over this latent phase. This energy absorbed to change phase is called latent energy/heat.

Learn More:

For more on change of phase of water check out;

brainly.com/question/2128466

brainly.com/question/13251064

#LearnWithBrainly

3 0

3 years ago

Doing it again please answer for me appreciate it thank you

Mandarinka [93]

Answer:

1. A

Explanation:

i guessed on this answer

4 0

2 years ago

Read 2 more answers

A student has 70.5 mL of a 0.463 M aqueous solution of sodium bromide. The density of the solution is 1.22 g/mL. Find the follow

AleksandrR [38]

Answer:

a.) 86.01 g.

b.) 3.36 g.

c.) 0.394 m ≅ 0.40 m.

d.) 4.77%.

e.) 3.9%.

Explanation:

<em>a.) mass of the solution:</em>

The density of the solution is the mass per unit volume.

<em>∵ Density of solution = (mass of solution)/(volume of the solution).</em>

∴ Mass of the solution = (density of solution)*(volume of the solution) = (1.22 g/mL)*(70.5 mL) = 86.01 g.

<em>b.) grams of sodium bromide :</em>

Molarity (M) is defined as the no. of moles of solute dissolved per 1.0 L of the solution.

∵ M = (no. of moles of NaBr)/(Volume of the solution (L))

∴ no. of moles of NaBr = M*(Volume of the solution (L)) = (0.463 M )*(0.0705 L) = 0.0326 mol.

<em>∵ no. of moles of NaBr = (mass of NaBr)/(molar mass of NaBr)</em>

∴ mass of NaBr = (no. of moles of NaBr)*(molar mass of NaBr) = (0.0326 mol)*(102.894 g/mol) = 3.36 g.

<em>c.) molality of the solution:</em>

Molality (m) is defined as the no. of moles of solute dissolved per 1.0 kg of the solvent.

∵ m = (no. of moles of NaBr)/(mass of the soluvent (kg))

no. of moles of NaBr = 0.0326 mol,

mass of solvent = mass of the solution - mass of NaBr = 86.01 g - 3.36 g = 82.65 g = 0.08265 kg.

∴ m = (no. of moles of NaBr)/(mass of the soluvent (kg)) = (0.0326 mol)/(0.08265 kg) = 0.394 m ≅ 0.40 m.

<em>d.) % (m/v) of the solution:</em>

∵ (m/v)% = [(mass of solute) /(volume of the solution)]* 100

∴ (m/v)% = [(3.36 g)/(70.5 mL)]* 100 = 4.77%.

<em>e.) % (m/m) of the solution:</em>

∵ (m/m)% = [(mass of solute) /(mass of the solution)]* 100

∴ (m/m)% = [(3.36 g)/(86.01 g)] * 100 = 3.9 %.

4 0

2 years ago

3. Would polar or non-polar gases be more likely to be considered an ideal gas? Explain

zubka84 [21]

Answer:

it is an ideal gas because all of the substances that it has are good for us and won't affect us in any way

6 0

3 years ago

What is the vapor pressure at 20 °c of an ideal solution prepared by the addition of 7.38 g of the nonvolatile solute urea, co(n

Romashka [77]

Answer:

83.24 mmHg.

Explanation:

<em>The vapor pressure of the solution (Psolution) = (Xmethanol)(P°methanol).</em>

where, Psolution is the vapor pressure of the solution,

Xmethanol is the mole fraction of methanol,

P°methanol is the pure vapor pressure of methanol.

We need to calculate the mole fraction of methanol (Xmethanol).

<em>Xmethanol = (n)methanol/(n) total.</em>

where, n methanol is the no. of moles of methanol.

n total is the total no. of moles of methanol and urea.

We can calculate the no. of moles of both methanol and urea using the relation: n = mass/molar mass.

n of methanol = mass/molar mass = (56.9 g)/(32.04 g/mol) = 1.776 mol.

n of urea = mass/molar mass = (7.38 g )/(60.06 g/mol) = 0.123 mol.

∴ Xmethanol = (n)methanol/(n) total = (1.776 mol)/(1.776 mol + 0.123 mol) = 0.935.

<em>∴ Psolution = (Xmethanol)(P°methanol)</em> = (0.935)(89.0 mmHg) =<em> 83.24 mmHg.</em>

7 0

2 years ago