The junction where one neuron can transfer an impulse to the next structure is known as a

Determine the mass in grams of 3.75 x 10^21 atoms of zinc. (the mass of one mole of zinc is 65.39 g)

Nastasia [14]

Answer: The mass in $3.75 \times 10^{21}$ atoms of zinc is 0.405 g.

Explanation:

Given: Atoms of zinc = $3.75 \times 10^{21}$

It is known that 1 mole of every substance contains $6.022 \times 10^{23}$ atoms. So, the number of moles in given number of atoms is as follows.

$Moles = \frac{3.75 \times 10^{21}}{6.022 \times 10^{23}}\\= 0.622 \times 10^{-2}\\= 0.0062 mol$

As moles is the mass of a substance divided by its molar mass. So, mass of zinc (molar mass = 65.39 g/mol) is calculated as follows.

$Moles = \frac{mass}{molar mass}\\0.0062 mol = \frac{mass}{65.39 g}\\mass = 0.405 g$

Thus, we can conclude that the mass in $3.75 \times 10^{21}$ atoms of zinc is 0.405 g.

6 0

3 years ago

In a chemical formula the right side is called?

Ghella [55]

Answer:

Product

Explanation:

It is written at the right side of an arrow

8 0

4 years ago

4.00 dm of oxygen at a pressure of 2 atm and 1.00 dm3 nitrogen at a pressure of 1 atm are introduced into a 2.00 dm3 vessel.

podryga [215]

Answer:

A

Explanation:

5 0

3 years ago

According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6 with excess Cl2? The molar ma

bonufazy [111]

Answer:

1640 kJ are involved in the reaction

Explanation:

In the reaction:

B₂H₆(g) + 6Cl₂(g) → 2 BCl₃(g) + 6HCl(g)

1 mol of B₂H₆(g) with 6 moles of Cl₂(g) produce 1396 kJ of energy.

Now if 32.5g of B₂H₆(g) react with excess Cl₂(g), moles involved in reaction are:

$32.5g B_2H_6\frac{1mol}{27.67g} = 1.175 moles$

If 1 mol produce 1396kJ of energy, 1.175 moles produce:

$1.175mol\frac{1396kJ}{1mol} = 1640kJ\\$

Thus, 1640 kJ are involved in the reaction

5 0

4 years ago

Read 2 more answers

The sulfur content of an ore is determined gravimetrically by reacting the ore with concentrated nitric acid and potassium chlor

katen-ka-za [31]

Answer:

13.92 %

Explanation:

Mass of $BaSO_4$ = 12.5221 g

Molar mass of $BaSO_4$ = 233.43 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{12.5221\ g}{233.43\ g/mol}$

Moles of $BaSO_4$ = 0.0536 moles

According to the given reaction,

$Ba^{2+}_{(aq)}+SO_4^{2-}_{(aq)}\rightarrow BaSO_4_{(s)}$

1 mole of $BaSO_4$ is formed from 1 mole of $SO_4^{2-}$

Thus,

0.0536 moles of $BaSO_4$ is formed from 0.0536 moles of $SO_4^{2-}$

Moles of $SO_4^{2-}$ = 0.0536 moles

Moles of sulfur in 1 mole $SO_4^{2-}$ = 1 mole

Moles of sulfur in 0.0536 mole $SO_4^{2-}$ = 0.0536 mole

Molar mass of sulfur = 32.065 g/mol

Mass = Moles * Molar mass = 0.0536 * 32.065 g = 1.7187 g

Mass of ore = 12.3430 g

Mass % = $\frac{Mass\ of\ Sulfur}{Mass_{ore}}\times 100$ = $\frac{1.7187}{12.3430}\times 100$ = 13.92 %

3 0

4 years ago