The theoretical yield for CuCO3.Cu(OH)2+2h2SO4 ®2CuSO4+2H2O+3CO2

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Answer 1

Answer:

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A food is initially at a moisture content of 90% dry basis. Calculate the moisture content in wet basis

Answers

Answer:

Moisture content in wet basis = 47.4 %

Explanation:

Moisture content expresses the amount of water present in a moist sample.Dry basis and wet basis are widely used to express moisture content.

The next equation express the moisture content in wet basis:

$MC_(wb)=(MC_(db))/(1+MC_(db))$

where, $MC_(wb)$ : moisture content in wet basis and

$MC_(db)$ : moisture content in dry basis

We now calculate the moisture content in wet basis:

$MC_(wb)=(MC_(db))/(1+MC_(db))$

$MC_(wb)=(0.90)/(1+0.90)$

$MC_(wb)$ = 0.474 = 47.4 % wet basis

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How many moles of Al are necessary to form 23.6 g of AlBr₃ from this reaction: 2 Al(s) + 3 Br₂(l) → 2 AlBr₃(s) ?

Answers

0.085 moles of Al are required to form 23.6 g of AlBr₃.

Let's consider the following balanced equation for the synthesis reaction of AlBr₃.

2 Al(s) + 3 Br₂(l) → 2 AlBr₃(s)

First, we will convert 23.6 g to moles using the molar mass of AlBr₃ (266.69 g/mol).

$23.6 g * (1mol)/(266.69g) = 0.0885 mol$

The molar ratio of Al to AlBr₃ is 2:2. The moles of Al required to form 0.0885 moles of AlBr₃ are:

$0.0885molAlBr_3 * (2molAl)/(2molAlBr_3) = 0.0885molAl$

0.085 moles of Al are required to form 23.6 g of AlBr₃.

You can learn more about stoichiometry here: brainly.com/question/22288091

Answer:

0.088 mole of Al.

Explanation:

First, we shall determine the number of mole in 23.6 g of AlBr₃.

This is illustrated below:

Mass of AlBr₃ = 23.6 g

Molar Mass of AlBr₃ = 27 + 3(80) = 267 g/mol

Mole of AlBr₃ =.?

Mole = mass/Molar mass

Mole of AlBr₃ = 23.6 / 267

Mole of AlBr₃ = 0.088 mol

Next, we shall writing the balanced equation for the reaction.

This is given below:

2Al(s) + 3Br₂(l) → 2AlBr₃(s)

From the balanced equation above,

2 moles of Al reacted with 3 mole of Br₂ to 2 moles AlBr₃.

Finally, we shall determine the number of mole of Al needed for the reaction as follow:

From the balanced equation above,

2 moles of Al reacted to 2 moles AlBr₃.

Therefore, 0.088 mole of Al will also react to produce 0.088 mole of AlBr₃.

What is the bond character of this molecule? A.) strongly covalent
B.) Positively charged
C.) Strongly ionic
D.) Negatively charged

Answers

There are two types of atomic bonds - ionic bonds and covalent bonds. They differ in their structure and properties. Covalent bonds consist of pairs of electrons shared by two atoms, and bind the atoms in a fixed orientation. ... This results in a positively charged ion (cation) and negatively charged ion (anion)

Barium chloride + sodium phosphate 
Answer with double replacement

Answers

Answer:

Barium chloride + Sodium phosphate → barium phosphate + sodium chloride

Explanation:

Double replacement:

It is the reaction in which two compound exchange their ions and form new compounds.

AB + CD → AC +BD

Chemical equation:

BaCl₂ + Na₃PO₄ → Ba₃(PO₄)₂ + NaCl

Balanced chemical equation:

3BaCl₂ + 2Na₃PO₄ → Ba₃(PO₄)₂ + 6NaCl

The cation and anion of both reactants are exchanged with each other.

Ba²⁺ react with PO₄³⁻ and form Ba₃(PO₄)₂ while Cl⁻ react with Na⁺ and form sodium chloride.

Molecular equation:

Barium chloride + Sodium phosphate → barium phosphate + sodium chloride

Final answer:

A double replacement reaction between barium chloride and sodium phosphate results in the formation of barium phosphate and sodium chloride.

Explanation:

The given chemical equation represents a double replacement reaction. The chemical reactants are barium chloride (BaCl2) and sodium phosphate (Na3PO4). In a double replacement reaction, the cations and anions of the two reactants switch places to form two new compounds.

So here is how the reaction would proceed: BaCl2 + Na3PO4 -> Ba3(PO4)2 + NaCl.

This translates to: Barium chloride reacts with sodium phosphate to form barium phosphate and sodium chloride.

Learn more about double replacement reaction here:

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Consider the following unbalanced equation for the combustion of hexane: αC6H14(g)+βO2(g)→γCO2(g)+δH2O(g) Part A Balance the equation. Give your answer as an ordered set of numbers α, β, γ, ... Use the least possible integers for the coefficients. α α , β, γ, δ = nothing Request Answer Part B Determine how many moles of O2 are required to react completely with 5.6 moles C6H14. Express your answer using two significant figures. n n = nothing mol Request Answer Provide Feedback

Answers

Answer:

2C₆H₁₄ + 19O₂ → 12CO₂ + 14H₂O

α =2

β = 19

γ = 12

δ = 14

53.2moles of O₂

Explanation:

Proper equation of the reaction:

αC₆H₁₄ + βO₂ → γCO₂ + δH₂O

This is a combustion reaction for a hydrocarbon. For the combustion of a hydrocarbon, the combustion equation is given below:

CₓHₙ + (x + $(n)/(4)$ )O₂ → xCO₂ + $(n)/(2)$ H₂O

From the given combustion equation, x = 6 and n = 14

Therefore:

β = x + $(n)/(4)$ = 6 + $(14)/(4)$ = 6 + 3.5 = 9 $(1)/(2)$

γ = 6

δ = $(n)/(2)$ = $(14)/(2)$ = 7

The complete reaction equation is therefore given as:

C₆H₁₄ + 9 $(1)/(2)$ O₂ → 6CO₂ + 7H₂O

To express as whole number integers, we multiply the coefficients through by 2:

2C₆H₁₄ + 19O₂ → 12CO₂ + 14H₂O

Problem 2

From the reaction:

2 moles of hexane are required to completely react with 19 moles of O₂

∴ 5.6 moles of hexane would react with k moles of O₂

This gives: 5.6 x 19 = 2k

k = $(5.6 x 19)/(2)$

k = 53.2moles of O₂

A sample of solid calcium hdroxide, Ca(OH)2 is allowed to stand in water until a saturated solution is formed. A titration of 75.00mL of this solution with 5.00 x 10-2 M HCl 36.6 mL of the acid to reach the end pointCa(OH)2 + 2HCl ? CaCl + 2H2O
What is the molarity?