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4 years ago

The water that penetrates into the ground is stored in

Chemistry

2 answers:

miss Akunina [59]4 years ago

6 0

geysers,
here you go
I hope this helps and you pass you ? or test

Studentka2010 [4]4 years ago

4 0

Answer:

Aquifers and groundwater

Explanation:

Also known as "Groundwater", these are underground layers of water-bearing permeable rocks, unconsolidated materials or rock fractures.

Grandwater can also be extracted using a water well.

Hydrogeology is the study of water flow in aquifers and the characterization of aquifers.

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What are some physical properties of a candle

Troyanec [42]

The wick and the wax

Sorry if that was useless, I'm not sure how generalized you were being

6 0

3 years ago

Read 2 more answers

Need this ASAP PLEASE

ss7ja [257]

SOLVENT- A substance (usually a liquid) capable of dissolving one or more pure substances. SOLUTE- Solid, liquid or gas that is dissolved in a solvent. SOLUTION- A homogeneous (looks the same throughout) mixture of a solvent and one or more solutes. AQUEOUS SOLUTION- Solution in which water is the solvent.
Answer

it raises the boiling point substance is dissolved in water

7 0

3 years ago

How many grams of Fe can be produced when 5.50 g of Fe2O3 reacts?

vichka [17]

Answer:

3,85 g of Fe

Explanation:

1- The first thing to do is calculate the molar mass of the Fe2O3 compound. With the help of a periodic table, the weights of the atoms are searched, and the sum is made:

Molar mass of Fe2O3 = (2 x mass of Fe) + (3 x mass of O) = 2 x 55.88 g + 3 x 15.99 g = 159.65 g / mol

Then, one mole of Fe2O3 has a mass of 159.65 grams.

2- Then, the relationship between the Fe2O3 that will react and the iron to be produced. With the previous calculation, we can say that with one mole of Fe2O3, two moles of Fe can be produced. Passing this relationship to the molar masses, it would be as follows:

1 mole of Fe2O3_____ 2 moles of Fe

159.65 g of Fe2O3_____ 111.76 g of Fe

3- Finally, the calculation of the mass that can be produced of Fe is made, starting from 5.50 g of Fe2O3

159.65 g of Fe2O3 _____ 111.76 g of Fe

5.50 g of Fe2O3 ______ X = 3.85 g of Fe

Calculation: 5.50 g x 111.76 g / 159.65 g = 3.85 g

The answer is that 3.85 g of Fe can be produced when 5.50 g of Fe2O3 react

7 0

3 years ago

Given that cao(s) + h2o(l) → ca(oh)2(s), δh°rxn = –64.8 kj/mol, how many grams of cao must react in order to liberate 525 kj of

USPshnik [31]

Answer:

454.3 g.

Explanation:

From the given data:

1.0 mol of CaO liberates → – 64.8 kJ.

??? mol of CaO liberates → - 525 kJ.

∴ The no. of moles needed = (1.0 mol)(- 525 kJ)/(- 64.8 kJ) = 8.1 mol.

∴ The no. of grams of CaO needed = no. of moles x molar mass = (8.1 mol)(56.077 g/mol) = 454.3 g.

8 0

3 years ago

Using the thermodynamic information in the ALEKS Data tab, calculate the boiling point of titanium tetrachloride . Round your an

ddd [48]

Answer:

The boiling point is 308.27 K (35.27°C)

Explanation:

The chemical reaction for the boiling of titanium tetrachloride is shown below:

Ti $Cl_{4(l)}$ ⇒ Ti $Cl_{4(g)}$

ΔH° $_{f}$ (Ti $Cl_{4(l)}$ ) = -804.2 kJ/mol

ΔH° $_{f}$ (Ti $Cl_{4(g)}$ ) = -763.2 kJ/mol

Therefore,

ΔH° $_{f}$ = ΔH° $_{f}$ (Ti $Cl_{4(g)}$ ) - ΔH° $_{f}$ (Ti $Cl_{4(l)}$ ) = -763.2 - (-804.2) = 41 kJ/mol = 41000 J/mol

Similarly,

s°(Ti $Cl_{4(l)}$ ) = 221.9 J/(mol*K)

s°(Ti $Cl_{4(g)}$ ) = 354.9 J/(mol*K)

Therefore,

s° = s° (Ti $Cl_{4(g)}$ ) - s°(Ti $Cl_{4(l)}$ ) = 354.9 - 221.9 = 133 J/(mol*K)

Thus, T = ΔH° $_{f}$ /s° = [41000 J/mol]/[133 J/(mol*K)] = 308. 27 K or 35.27°C

Therefore, the boiling point of titanium tetrachloride is 308.27 K or 35.27°C.

5 0

3 years ago