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3 years ago

Given 2.14g of B2H6

Chemistry

1 answer:

Shkiper50 [21]3 years ago

5 0

Answer:

(A) is 0.0773 mol B2H6

Explanation:

Questions (A) and (B) are the same.

2.14 g B2H6 x (1 mol B2H6/27.668g B2H6) = 0.0773 mol B2H6 (A)

<u>27.668 is the molar mass of B2H6 calculated from the period table: </u>

(2 x 10.81) + (6 x 1.008) = 27.668

1.008 is the mass of H and 10.81 is the mass of B

(C)

0.0773 mol B2H6 x (6 mol H/ 1 mol B2H6) x (6.022 x 10^23 H atoms/1 mol H)

= 2.79 x 10^23 hydrogen atoms

Further Explanation:

For every 1 mol of B2H6, there are 6 moles of H (indicated by the subscript)

6.022 x 10^23 is Avogrado's number and it equals to 1 mol of anything

Avogrado's number can be in units of atoms, molecules, or particles

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Answer : The balanced complete and net ionic equations are written below.

Explanation :

Complete ionic equation : In complete ionic equation, all the substance that are strong electrolyte and present in an aqueous are represented in the form of ions.

Net ionic equation : In the net ionic equations, we are not include the spectator ions in the equations.

Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides.

(a) The balanced molecular equation will be,

$FeCl_3(aq)+Cs_3PO_4(aq)\rightarrow 3CsCl(aq)+FePO_4(s)$

The complete ionic equation in separated aqueous solution will be,

$Fe^{3+}(aq)+3Cl^{-}(aq)+3Cs^{+}(aq)+PO_4^{3-}(aq)\rightarrow 3Cs^{+}(aq)+3Cl^{-}(aq)+FePO_4(s)$

In this equation the species present are, $3Cl^{-}\text{ and }Cs^{+}$ are the spectator ions.

By removing the spectator ions from the balanced ionic equation, we get the net ionic equation.

The net ionic equation will be,

$Fe^{3+}(aq)+PO_4^{3-}(aq)\rightarrow FePO_4(s)$

(b) The balanced molecular equation will be,

$2NaOH(aq)+Cd(NO_3)_2(aq)\rightarrow 2NaNO_3(aq)+Cd(OH)_2(s)$

The complete ionic equation in separated aqueous solution will be,

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In this equation the species present are, $Na^{+}\text{ and }NO_3^{-}$ are the spectator ions.

By removing the spectator ions from the balanced ionic equation, we get the net ionic equation.

The net ionic equation will be,

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The complete ionic equation in separated aqueous solution will be,

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In this equation all the species are the spectator ions.

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The complete ionic equation in separated aqueous solution will be,

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In this equation no species are the spectator ions.

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The complete ionic equation in separated aqueous solution will be,

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The net ionic equation will be,

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