Find the weighted average for the three following isotopes:

How many liters of hydrogen gas will be produced at STP from the reaction of 7.179×10^23 atoms of magnesium with 54.219g of phos

Alexeev081 [22]

Answer: The volume of hydrogen gas produced will be, 12.4 L

Explanation : Given,

Mass of $H_3PO_4$ = 54.219 g

Number of atoms of $Mg$ = $7.179\times 10^{23}$

Molar mass of $H_3PO_4$ = 98 g/mol

First we have to calculate the moles of $H_3PO_4$ and $Mg$ .

$\text{Moles of }H_3PO_4=\frac{\text{Given mass }H_3PO_4}{\text{Molar mass }H_3PO_4}$

$\text{Moles of }H_3PO_4=\frac{54.219g}{98g/mol}=0.553mol$

and,

$\text{Moles of }Mg=\frac{7.179\times 10^{23}}{6.022\times 10^{23}}=1.19mol$

Now we have to calculate the limiting and excess reagent.

The balanced chemical equation is:

$3Mg+2H_3PO_4\rightarrow Mg(PO_4)_2+3H_2$

From the balanced reaction we conclude that

As, 3 mole of $Mg$ react with 2 mole of $H_3PO_4$

So, 0.553 moles of $Mg$ react with $\frac{2}{3}\times 0.553=0.369$ moles of $H_3PO_4$

From this we conclude that, $H_3PO_4$ is an excess reagent because the given moles are greater than the required moles and $Mg$ is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of $H_2$

From the reaction, we conclude that

As, 3 mole of $Mg$ react to give 3 mole of $H_2$

So, 0.553 mole of $Mg$ react to give 0.553 mole of $H_2$

Now we have to calculate the volume of $H_2$ gas at STP.

As we know that, 1 mole of substance occupies 22.4 L volume of gas.

As, 1 mole of hydrogen gas occupies 22.4 L volume of hydrogen gas

So, 0.553 mole of hydrogen gas occupies $0.553\times 22.4=12.4L$ volume of hydrogen gas

Therefore, the volume of hydrogen gas produced will be, 12.4 L

4 0

3 years ago

The number of molecules in 1.0 mole of H2O is the same as in one mole of O2.

zaharov [31]

True. A mole of anything has the same amount of molecules. 1 mole = 6.022 x 1023 molecules

8 0

3 years ago

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Name some of the chemical substances in a tea mixture

faltersainse [42]

Answer:

caffience

Explanation:

6 0

3 years ago

Part a choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force. Choose the mole

mart [117]

Answer : $SO_{2}$ is the molecule that exhibit dipole-dipole forces as its strongest intermolecular force.

Explanation : The shape or geometry of given molecules of $N_{2}$ , $H_{2}$ , $CBr_{4}$ , $BCl_{3}$ and $SO_{2}$ are linear, linear, tetrahedral, trigonal planar and angular respectively.

The given molecules $N_{2}$ , $H_{2}$ , $CBr_{4}$ , $BCl_{3}$ are symmetrical molecules. These symmetric molecules cannot exists as dipole even they contain polar bonds. Thus, these molecules will not exhibit dipole-dipole forces.

$SO_{2}$ molecule has polar bonds and unsymmetrical bonds as shown in attached image. This molecule cannot exhibit H-bonding. It exhibit only dipole-dipole forces.

Therefore, $SO_{2}$ molecule exhibit dipole-dipole forces as strongest intermolecular force.

7 0

3 years ago

Which statement is most consistent with the plum pudding model of the atom?

lianna [129]

The answer to this question would be: <span>1) Electrons occupy regions of space
</span><span>
In plum pudding model, the atoms are drawn as pudding and the negative particle is spread around the pudding. In this model, the electron is spread but not moving in orbit. Rutherford model that comes afterward is the one that says most of the atoms is empty space.</span>

3 0

3 years ago

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