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2 years ago

Identify the Lewis acids and Lewis bases in the following reactions:

Chemistry

1 answer:

postnew [5]2 years ago

8 0

Answer: 1. $H^++OH^-\rightarrow H_2O$ Lewis acid : $H^+$ , Lewis base : $OH^-$

2. $Cl^-+BCl_3\rightarrow BCl_4^-$ Lewis acid : $BCl_3$ , Lewis base : $Cl^-$

3. $K^++6H_2O\rightarrow K(H_2O)_6$ Lewis acid : $K^+$ , Lewis base : $H_2O$

Explanation:

According to the Lewis concept, an acid is defined as a substance that accepts electron pairs and base is defined as a substance which donates electron pairs.

1. $H^++OH^-\rightarrow H_2O$

As $H^+$ gained electrons to complete its octet. Thus it acts as lewis acid. $OH^-$ acts as lewis base as it donates lone pair of electrons to electron deficient specie $H^+$ .

2. $Cl^-+BCl_3\rightarrow BCl_4^-$

As $BCl_3$ is short of two electrons to complete its octet. Thus it acts as lewis acid. $Cl^-$ acts as lewis base as it donates lone pair of electrons to electron deficient specie $BCl_3$ .

3. $K^++6H_2O\rightarrow K(H_2O)_6$

As $K^+$ is short of electrons to complete its octet. Thus it acts as lewis acid. $H_2O$ acts as lewis base as it donates lone pair of electrons to electron deficient specie $K^+$ .

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Determine the total number of moles of ions in 40.0 ml of a 0.345 m solution of the strong electrolyte mgcl2

Sedbober [7]

A strong electrolyte like MgCl2 dissociates completely as per the following reaction:

$MgCl_2 ----\ \textgreater \ Mg^{2+} + 2Cl^-$

As you can see, from 1 molecule of MgCl2 produces 3 ions on dissociation.
So, 1 mole of MgCl2 produces 3 moles of ions.

Now, Moles of MgCl2 = Volume x Molarity

= 0.04 x 0.345 [Change volume to Litres]
= 0.0138 moles

Now, total moles of ions = 0.0138 x 3 = 0.0414

6 0

2 years ago

How many grams of NH3 can be prepared from the synthesis of 77.3 grams of nitrogen and 14.2 grams of hydrogen gas?

lbvjy [14]

Answer:

80.41 g

Explanation:

Data Given:

Mass of Nitrogen (N₂) = 77.3 g

Mass of Hydrogen (H₂) = 14.2 g

many grams of NH₃ = ?

Solution:

First we look at the balanced synthesis reaction

N₂ + 3 H₂ ------—> 2 NH₃

1 mol 3 mol

As 1 mole of Nitrogen react with 3 mole of hydrogen

Convert moles to mass

molar mass of N₂ = 2(14) = 28 g/mol

molar mass of H₂ = 2(1) + 2 g/mol

Now

N₂ + 3 H₂ ------—> 2 NH₃

1 mol (28 g/mol) 3 mol(2g/mol)

28 g 6 g

28 grams of N₂ react with 6 g of H₂

if 28 grams of N₂ produces 6 g of H₂ so how many grams of N₂ will react with 14.2 g of H₂.

Apply Unity Formula

28 g of N₂ ≅ 6 g of H₂

X g of N₂ ≅ 14.2 g of H₂

Do cross multiply

X g of N₂ = 28 g x 14.2 g / 6 g

X g of N₂ = 66.3 g

As we have given with 77. 3 g of N₂ but from this calculation we come to know that 66.3 g will react with 14.2 g of hydrogen and the remaining 10 g N₂ will be in excess

So, Hydrogen is limiting reactant in this reaction and the amount of NH₃ depends on the amount of hydrogen.

Now

To find mass of NH₃ we will do following calculation

Look at the reaction

As we Know

N₂ + 3 H₂ ------—> 2 NH₃

6 g 2 mol

So, 6 g of hydrogen gives 2 moles of NH₃, then how many moles of NH₃ will be produce by 14.2 g

Apply Unity Formula

6 g of H₂ ≅ 2 mol of NH₃

14.2 g of H₂ ≅ X mol of NH₃

Do cross multiply

X mol of NH₃= 14.2 g x 2 mol / 6 g

X mol of NH₃ = 4.73 mol

So, 14.2 g of hydrogen gives 4.73 moles of NH₃

Now

Convert moles of NH₃ to mass

Formula will be used

mass in grams = no. of moles x molar mass . . . . . . (2)

Molar mass of NH₃

Molar mass of NH₃ = 14 + 3(1)

Molar mass of NH₃ = 14 + 3 = 17 g/mol

Put values in equation 2

mass in grams = 4.73 mole x 17 g/mol

mass in grams = 80.41 g

mass of NH₃= 80.41 g

3 0

1 year ago

Assume the atomic mass of element X is 22.99 amu. A 17.15−g sample of X combines with 14.17 g of another element Y to form a com

Alenkasestr [34]

The formula of the compound is XY. This means that the relation between the moles is 1: 1. One mole of X per one mole of Y.

From the information about the element X you can determine the number of moles of X (which is the same that the number of moles of Y).

# of moles of X = weigth of X / atomic mass of X = 17.15 g / 22.9 g/mol = 0.74598

Now the atomic mass of Y = weight of Y / # of moles of Y = 14.17 g / 0.74598 mol = 19 amu

8 0

1 year ago

What is the density of 96 ml of a liquid that has a mass of 90.5 g?

Otrada [13]

Answer:

Density = Mass / Volume. so, x = 90.5 g / 96 mL ... The Density would be 0.942 g/mL

8 0

2 years ago

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O2 (g) →→ 2MgO (s) When 4.50 g of magnes

Klio2033 [76]

Answer:

7.46 g

Explanation:

From the balanced equation, 2 moles of Mg is required for 2 moles of MgO.

The mole ratio is 1:1

mole = mass/molar mass

mole of 4.50 g Mg = 4.50/24.3 = 0.185 mole

0.185 mole Mg will tiled 0.185 MgO

Hence, theoretical yield of MgO in g

mass = mole x molar mass

0.185 x 40.3 = 7.46 g

6 0

2 years ago

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