The system international (SI) unit for energy is:

Is Pb(NO3)2 molecular?

o-na [289]

Answer:

no

Explanation:

its ionic

4 0

2 years ago

Can we use water as a solvent to obtain ethyl butyrate?

klio [65]

Answer:

yes but it depends

Explanation:

7 0

3 years ago

A chemist needs 1.25 moles of sugar to dissolve in 1 liter of water how many grams of sugar needed

sdas [7]

Answer:

The mass of sugar used is 427.5 grams.

Explanation:

The formula of common sugar is $\mathrm{C_{12}H_{22}O_{11}}$ .

Its molar mass of molecule is 342 grams per mole.

The number of moles of sugar used is equal to '1.25'

$\mathbf{Mole=\frac{Mass \ given \ in \ grams}{Molar \ mass \ of \ molecule \ in \ grams}}$

$\textrm{Mass in grams}=\textrm{Mole} \times \textrm{Molar mass of molecule in grams}$

$\textrm{Mass in grams}= 1.25\times342$

$\mathbf{Mass \ in \ grams=427.5 g}$

(NOTE : You can calculate molar mass by adding the mass of all the atoms present in the atom.

Mass of Oxygen (O) = 16 ; Total number of Oxygen atoms present = 11

Mass of Hydrogen (H) =1 ; Total number of Hydrogen Atoms present = 22

Mass of Carbon (C) = 12 ; Total number of Carbon atoms present = 12

Total mass of molecule = 12 × 12 + 1 × 22 + 16 × 11 = 342)

4 0

3 years ago

Hydrogen bonds:__________

Elina [12.6K]

Answer:

Option e.

Explanation:

The option 'e' fact about Hydrogen bonds are correct, that is; ''form weak interactions but can provide structural stability when many are found in a single molecule''.

So, what is this Hydrogen bond?

Hydrogen bonds is a kind of strong dipole- dipole attractions. Hydrogen bonding occurs as a result of the bonding between hydrogen and strongly electronegative atoms for example oxygen, Fluorine and so on.

Since we now know what Hydrogen bond is, let us take a look at the options.

(a) for the first option, we can see from above meaning of Hydrogen bonds that Hydrogen bonds occur between Hydrogen and a strong Electronegative atom. So, this option is wrong.

(b). Option 'b' is also wrong Because Hydrogen bonds does not occur between hydrogen and oxygen atoms ONLY but also with other strong Electronegative atoms such as oxygen.

(c). Option 'c' is wrong because between a strong and not only between a weak electronegative atom and hydrogen.

(d). Option 'd' is also not correct.

(e). Option 'e' is correct. Hydrogen bonds contribute to the effect of boiling and melting point of substance, solubilty, dimerization, strength of bonds, shape of molecules and so on

5 0

4 years ago

Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s)+3Cl2(g)→2AlCl3(s) What is the max

jolli1 [7]

Answer: The mass of aluminium chloride that can be formed are 46.3 g

Explanation:

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

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ....(1)

For Aluminium:

Given mass of aluminium = 32 g

Molar mass of aluminium = 26.98 g/mol

Putting values in above equation, we get:

$\text{Moles of aluminium}=\frac{32g}{26.98g/mol}=1.186mol$

For Chlorine:

Given mass of chlorine = 37 g

Molar mass of chlorine = 71 g/mol

Putting values in above equation, we get:

$\text{Moles of chlorine gas}=\frac{37g}{71g/mol}=0.521mol$

For the given chemical equation:

$2Al(s)+3Cl_2(g)\rightarrow 2AlCl_3(s)$

By Stoichiometry of the reaction:

3 moles of chlorine gas is reacting with 2 moles of aluminium.

So, 0.521 moles of chlorine gas will react with = $\frac{2}{3}\times 0.521=0.347moles$ of aluminium.

As, given amount of aluminium is more than the required amount. Thus, it is considered as an excess reagent.

So, chlorine gas is considered as a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

3 moles of chlorine gas is producing 2 moles of aluminium chloride

So, 0.521 moles of chlorine gas will react with = $\frac{2}{3}\times 0.521=0.347moles$ of aluminium chloride.

Now, calculating the mass of aluminium chloride by using equation 1, we get:

Moles of aluminium chloride = 0.347 moles

Molar mass of aluminium chloride = 133.34 g/mol

Putting all the values in equation 1, we get:

$0.347mol=\frac{\text{Mass of aluminium chloride}}{133.34g/mol}\\\\\text{Mass of aluminium chloride}=46.3g$

Hence, the mass of aluminium chloride that can be formed are 46.3 g

7 0

4 years ago