A strong acid, HA, is added to water. Which statement about the solution is true

How many li are in 2.5 moles of li

NARA [144]

Answer:

15.06 × 10²³ atoms of Li

Explanation:

Given data:

Number of moles of Li = 2.5 mol

Number of toms of Li = ?

Solution:

The given problem will solve by using Avogadro number.

It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance.

The number 6.022 × 10²³ is called Avogadro number.

For example,

18 g of water = 1 mole = 6.022 × 10²³ molecules of water

1.008 g of hydrogen = 1 mole = 6.022 × 10²³ atoms of hydrogen

For 2.5 mol of Li:

1 mole of lithium = 6.022 × 10²³ atoms of Li

2.5 mol × 6.022 × 10²³ atoms of Li / 1 mol

15.06 × 10²³ atoms of Li

8 0

3 years ago

What is the product of the oxidation reaction of isopropyl alcohol with sodium hypochlorite?

Archy [21]

<h3>OXIDATION REACTION</h3>

==============================

$\large \sf \underline{Question:}$

What is the product of the oxidation reaction of isopropyl alcohol with sodium hypochlorite?

==============================

$\large \sf \underline{Answer:}$

$\qquad \qquad \huge \bold{Ketone}$

==============================

$\large \sf \underline{Explanation:}$

The product of the oxidation reaction of isopropyl alcohol with sodium hypochlorite is called ketone.

==============================

3 0

2 years ago

I need a answer quick. PLEASE What is the volume of 2.43 x 1023 molecules of N2 gas at STP?

Readme [11.4K]

I think it is 2485.89.

6 0

3 years ago

The reaction of a quantity of sulfur trioxide with water gives an acid with a volume of 2 l, containing 1.8 mol of the dissolved

777dan777 [17]

Answer :]

A.)Calculate the mass of ammonium sulfate that would be obtained by reacting with ammonia acid.

Correct me if i'm wrong :]

8 0

2 years ago

Aspirin (C9H8O4) is synthesized by reacting salicylic acid (C7H6O3) with acetic anhydride (C4H6O3). The balanced equation isC7H6

prisoha [69]

Answer:

For a: The mass of acetic anhydride needed is 73.91 grams.

For b: The theoretical yield of aspirin is 130.43 grams.

Explanation:

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

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

For a:

Given mass of salicylic acid = $1.00\times 10^2g=100g$

Molar mass of salicylic acid = 138.121 g/mol

Putting values in equation 1, we get:

$\text{Moles of salicylic acid}=\frac{100g}{138.121g/mol}=0.724mol$

For the given chemical reaction:

$C_7H_6O_3+C_4H_6O_3\rightarrow C_9H_8O_4+CH_3COOH$

By stoichiometry of the reaction:

1 mole of salicylic acid reacts with 1 mole of acetic anhydride.

So, 0.724 moles of salicylic acid will react with = $\frac{1}{1}\times 0.724=0.724mol$ of acetic anhydride.

Now, to calculate the mass of acetic anhydride, we use equation 1:

Moles of acetic anhydride = 0.724 moles

Molar mass of acetic anhydride = 102.09 g/mol

Putting values in equation 1, we get:

$0.724mol=\frac{\text{Mass of acetic anhydride}}{102.09g/mol}\\\\\text{Mass of acetic anhydride}=73.91g$

Hence, the mass of acetic anhydride needed is 73.91 grams.

For b:

By stoichiometry of the reaction:

1 mole of salicylic acid is producing 1 mole of aspirin.

So, 0.724 moles of salicylic acid will produce = $\frac{1}{1}\times 0.724=0.724mol$ of aspirin.

Now, to calculate the mass of aspirin, we use equation 1:

Moles of aspirin = 0.724 moles

Molar mass of aspirin = 180.158 g/mol

Putting values in equation 1, we get:

$0.724mol=\frac{\text{Mass of aspirin}}{180.158g/mol}\\\\\text{Mass of aspirin}=130.43g$

Hence, the theoretical yield of aspirin is 130.43 grams.

4 0

3 years ago