How many water molecules are in a block of ice containing 1.50 mol of water (H2O)?

Answers

Answer 1
Answer: 1.50 moles H20(6.02*10^23 molecules/1 mole)
9.03*10^23 molecules
Answer 2
Answer:

Final answer:

The number of water molecules in a 1.50 mol block of ice is calculated by multiplying the number of moles of water by Avogadro's number. The result is approximately 9.033 x 10^23 water molecules.

Explanation:

In chemistry, the amount of substance in moles is related to the number of particles (atoms, molecules) through Avogadro's number. Avogadro's number, which is 6.022 x 1023 particles/mol, tells us the number of molecules in one mole of a substance.

To calculate the number of water molecules in 1.50 mol of water, you would multiply the number of moles of water by Avogadro's number:

1.50 mol of water x 6.022 x 1023 water molecules/mol of water = 9.033 x 1023 water molecules

Therefore, there are approximately 9.033 x 1023 water molecules in a 1.50 mol block of ice.

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What type of hybridization is needed to explain why ethyne, C2H2, is linear?

Answers

When C-C is having a triple bond the hybridization is sp. But I am not sure how to relate that to the linear shape.

In what way(s) is(are) the structure of water similar to that of CHCl3? In what way is the structure of water different from that of CHCl3?

Answers

Answer:

See explanation below

Explanation:

In both cases the central atoms, C in CHCl₃ and O in H₂O, are sp³ hybridized .

Since they are sp³ hybridized we predict an angle  between the  H-C-Cl and H-O-H of 109.5 º ( tetrahedral ), but two of the sp³ orbitals in water are occupied by lone pairs.

These lone pairs do excercise more repulsion ( need more room ) than the bonds oxygen is making with hydrogen.

As a consequence of this repulsion the angles H-O-H are less than the predicted 109.5º in tetrahedra. ( Actually is 104.5 º)

What effect does salt have on most metals?

Answers

the combination of moisture, oxygen and salt ,especially sodium chloride, damages metal worse than rust does. This combination corrodes, or eats away at, the metal, weakening it and causing it to fall apart.

Saved Propane burns in air according to the equation C3Ha(g 502lg)3CO2) + 4H20(g) What volume of O2 in liters would be required if 15.0 L of propane burns, assuming that all of the gases are under the same conditions? Short Answer Toolbar navigation E I E B IUS EA This question will be sent to your Instructor for grading. 20 of 25 l Next > Prev nere to search

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Answer: 75 liters of O_2 in liters would be required if 15.0 L of propane burns, assuming that all of the gases are under the same conditions.

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 Lat STP and contains avogadro's number 6.023* 10^(23) of particles.

To calculate the number of moles, we use the equation:

\text{Number of moles of propane}=\frac{\text{Given volume}}{\text{Molar volume}}=(15.0L)/(22.4L)=0.67moles

C_3H_8+5O_2\rightarrow 3CO_2+4H_2O

According to stoichiometry:

1 mole of propane combines with = 5 moles of oxygen

Thus 0.67 moles of propane combine with  = (5)/(1)* 0.67=3.35moles

Volume of O_2=moles* {\text {Molar Volume}}=3.35* 22.4L=75L

Thus 75 liters of O_2 in liters would be required if 15.0 L of propane burns, assuming that all of the gases are under the same conditions.

2. Which test for iron(II) ions is conclusive ​

Answers

The conclusive test for iron(II) ions is the test by the use of potassium hexacyanoferrate III solution.

In qualitative analysis certain reagents are used to test for the presence of certain cations or anions. Those reagents react in a certain way with those reagents. Usually, a positive test may involve a color change, formation of a precipitate or evolution of a gas.

In the case of iron(II) ions, potassium hexacyanoferrate III solution is used in the conclusive qualitative test for the ion. A positive test involves the appearance of a deep blue precipitate.

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Answer:

please brainlist answer

Explanation:

The addition of K 3 Fe(CN) 6 to a solution causes the formation of a deep blue precipitate which indicates that iron(II) ions are present.