Ammonium phosphate NH43PO4 is an important ingredient in many fertilizers. It can be made by reacting phosphoric acid H3PO4 with ammonia NH3. What mass of ammonium phosphate is produced by the reaction of 5.5g of phosphoric acid

Answer:

Milli, m.

Explanation:

Hey there!

In this case, according to the given information, it turns out possible for us to answer to this question by bearing to mind the attached file whereas the most common prefixes and their factors are shown both in standard and scientific notation.

In such a way, we will be able to infer that the prefix related to the numerical value of 0.001 is milli, m, for example 1 mm which is 0.001 m.

Regards!

Answer:

See explanation

Explanation:

The relationship between the activation energy and rate of reaction is best captured by the Arrhenius equation;

k= Ae^-Ea/RT

Where;

k= rate constant

A= pre-exponential factor

Ea=activation energy

R= gas constant

T= temperature

We can see from the foregoing that, as the activation energy increases, the rate of reaction decreases and vice versa. reactions that have a very high activation energy are markedly slow.

Since the activation energy for the malonic acid reaction is found to be greater than the activation energy for the tartaric acid reaction, then the rate of the malonic acid reaction(k) will be slower than that of the tartaric acid reaction.

The study of chemistry and bonds is called chemistry. There are two types of elements metal and nonmetals.

The correct answer is mentioned below.

The equation is as follows:-

[tex]k= Ae^{-Ea/RT[/tex] Where;

We can see from the foregoing that, as the activation energy increases, the rate of reaction decreases and vice versa. reactions that have very high activation energy are markedly slow. Since the activation energy for the malonic acid reaction is found to be greater than the activation energy for the tartaric acid reaction, then the rate of the malonic acid reaction(k) will be slower than that of the tartaric acid reaction.

Hence, the correct answer is mentioned above.

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Answer:

The heat absorbed in Trial 2 is about 1,240 J greater than the heat absorbed in Trial 1.

The heat absorbed in Trial 2 is about 1,674 J greater than the heat absorbed in Trial 1.

The amount of heat absorbed or released by a substance can be calculated using the formula Q = mcΔT, where Q represents heat, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

In this case, the mass (m) is the same in both trials, but the initial and final temperatures (ΔT) differ. By comparing the values of ΔT in both trials, we can determine the difference in the amount of heat absorbed.

In Trial 1, the initial temperature is 15.0 °C and the final temperature is 65.0 °C, resulting in a ΔT of 65.0 - 15.0 = 50.0 °C.

In Trial 2, the initial temperature is 10.0 °C and the final temperature is 65.0 °C, resulting in a ΔT of 65.0 - 10.0 = 55.0 °C.

Since the specific heat capacity of water is approximately 4.18 J/g°C, we can calculate the difference in heat absorbed:

ΔQ = mcΔT = (80.0 g)(4.18 J/g°C)(55.0 °C - 50.0 °C) = 1,674 J

Therefore, the heat absorbed in Trial 2 is approximately 1,674 J greater than the heat absorbed in Trial 1.

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Explanation:

the reaction is a decomposition reaction since potassium hypochlorite is decomposed into potassium chloride and oxygen

this is the difference between organic and inorganic if this doesn't help you can research more on it

Answer:

Increase

Decrease

Explanation:While in solution, ionic substances produce ions. The ions in solution determine the conductivity of the solution.

The ionic strength of a solution shows the concentration of ions in a given solution. The more the number of ions in the solution, the greater the ionic strength of the solution and vice versa.

When HNO3 is added to a solution of KOH, the number of ions in the solution increases and so does the ionic strength of the solution.

When KOH is added to a solution of CaCl2 then Ca(OH)2 is formed. The formation of a solid precipitate decreases the concentration of ions in solution as well as the ionic strength of the solution.

Answer:

1. Nitrate ions, NaNO3 - Sodium nitrate.

2. Sulphide ions, K2S - Potassium sulphide.

3. Sulphate ions, CaSO4 - Calcium sulphate.

4. Hydrogensulphite ions, NaHSO3 - Sodium hydrogensulphite.

5. Carbonate ions, CaCO3 - Calcium carbonate.

6. Hydrogencarbonate ions, KHCO3 - Potassium hydrogencarbonate.

7. Phosphite ions, PH3 - Hydrogen phosphite.

8. Nitride ions, NH3 - Hydrogen nitride ( ammonia ).

9. Ethanoate ions, CH3COONa - Sodium ethanoate.

10. Methanoate ions, HCOONa - Sodium methanoate.

11. Fluoride ions, HF - Hydrogen fluoride.

12. Chloride ions, KCl - Potassium chloride.

13. Bromide ions, HBr - Hydrogen bromide.

14. Iodide ions, NaI - Sodium iodide.

15. Phosphate ions, K3PO3 - potassium phosphate.

Answer:

P2>S2>Cl2 is the order of bond energy of the given molecules.

Explanation:

The bonding in each molecule is shown below:

Thus, between each P-atom, there exists a triple bond.

Between two S-atoms there exists a double bond.

Between two chlorine atoms, there exists a single bond.

As the number of bonds increases between the given atoms, then bond energy required to break the bonds also increases.

Thus, the bond order is shown below:

[tex]P_2>S_2>Cl_2[/tex].

Answer:

CO2 is a trigonal planar.

Answer:

0.696 m

Explanation:

We'll begin by calculating the number of mole in 16.7 g of C₆H₁₂O₆. This can be obtained as follow:

Mass of C₆H₁₂O₆ = 16.7 g

Molar mass of C₆H₁₂O₆ = (6×12) + (12×1) + (6×16)

= 72 + 12 + 96

= 180 g/mol

Mole of C₆H₁₂O₆ =?

Mole = mass / molar mass

Mole of C₆H₁₂O₆ = 16.7 / 180

Mole of C₆H₁₂O₆ = 0.093 mole

Next, we shall convert 133.6 g of water to Kg. This can be obtained as follow:

1000 g = 1 Kg

Therefore,

133.6 g = 133.6 g × 1 Kg / 1000 g

133.6 g = 0.1336 Kg

Thus, 133.6 g is equivalent to 0.1336 Kg.

Finally, we shall determine the molality of the solution. This can be obtained as illustrated below:

Mole of C₆H₁₂O₆ = 0.093 mole

Mass of water = 0.1336 Kg

Molality =?

Molality = mole / mass of water (in Kg)

Molality = 0.093 / 0.1336

Molality = 0.696 m

Therefore, the molality of the solution is 0.696 m

The volume of 1.5 moles of gas at STP  is 33.6 L.

The volume of the gas at STP is calculated as follows;

I mole of gas at STP = 22.4 L

1.5 moles of the gas at STP = ?

= 1.5 moles  x 22.4 L/mole

= 33.6 L

Thus, the volume of 1.5 moles of gas at STP  is 33.6 L.

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Answer:

Explanation:

Assume we have 100g of this substance. That means we would have 20.24g of Cl and 79.76g of Al. Now we can find how many moles of each we have:

[tex]\frac{79.76 \:g}{35.45 \: g/mol}[/tex] = 2.25 mol of chlorine

[tex]\frac{20.24 \: g}{26.98 \: g/mol}[/tex] = 0.750 mol of Al.

To form a integer ratio, do 2.25/0.75 = 2.99999 ~= 3.

So the ratio is essentially Al : Cl => 1 : 3. To the compound is possibly [tex]AlCl_3[/tex].

However, it says it has a molar mass of 266.64 g/mol, and since AlCl3 has a molar mass of 133.32, it must be [tex]Al_2Cl_6[/tex].

Actually this molecule isn't exactly AlCl3 (which is ionic). Al2Cl6 forms a banana bond where Cl acts as a hapto-2 ligand. But that's a bit advanced. All you need to know is X = Al2Cl6

The molecular formula of the compound is Al₂Cl₆

To solve the question given above, we'll begin by obtaining the empirical formula of the compound. This can be obtained as follow:

Aluminum (Al) = 20.24%

Chlorine (Cl) = 79.76%

Al = 20.24%

Cl = 79.76%

Divide by their molar mass

Al = 20.24 / 27 = 0.75

Cl = 79.76 / 35.5 = 2.25

Divide by the smallest

Al = 0.75 / 0.75 = 1

Cl = 2.25 / 0.75 = 3

Thus, the empirical formula of the compound is AlCl₃

Finally, we shall determine the the molecular formula of the compound.

Molar mass of compound = 266.64 g/mol

Empirical formula = AlCl₃

[AlCl₃]ₙ = 266.64

[27 + (3×35.5)]n = 266.64

[27 + 106.5]n = 266.64

133.5n = 266.64

Divide both side by 133.5

n = 266.64 / 133.5

Molecular formula = [AlCl₃]ₙ

Molecular formula = [AlCl₃]₂

Therefore, the molecular formula of the compound is Al₂Cl₆

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Answer:

B

Explanation:

Answer:

See explanation

Explanation:

Truly, the second law of thermodynamics requires that spontaneous processes generate entropy, either in the system or in the surroundings.

When a solid is dissolved in a liquid, the solid dissociates into ions. These ions increases the number of particles and hence the entropy of the system thereby making the process spontaneous.

Hence, the dissolution of a substance via an endothermic process is spontaneous because of increase in the number of particles which in turn increases the entropy of the system.

Answer:

A. 4+.

B. 4+

C. 2+.

Explanation:

Hey there!

In this case, according to the given substances, it turns out possible for us to find the oxidation number of each element by applying the concept of charge balance in all of them as shown below:

A. sulfur in S032- : overall charge is 2- and the oxidation number of oxygen is 2-, thus:

[tex]x-6=-2\\\\x=6-2\\\\x=4+[/tex]

B. nickel in NiO2 : overall charge is 0 and the oxidation number of oxygen is 2-, thus:

[tex]x-4=0\\\\x=4+[/tex]

C. iron in Fe(OH)2: overall charge is 0 and the oxidation state of the OH ion is 1-, thus:

[tex]x-2=0\\\\x=2+[/tex]

Regards!

Answer:

77%

Explanation:

First we convert 3.0 g of cyclohexanol (C₆H₁₂O) to moles, using its molar mass:

Then we convert 1.9 g of cyclohexene (C₆H₁₀) to moles, using its molar mass:

Finally we calculate the theoretical yield:

The properties of solids, liquids and gases regarding their shapes and volumes are:

                       Shape             Volume

Solids              Fixed                Fixed

Liquids           Variable            Fixed

Gases             Variable           Variable

Solids have strong attraction forces between their molecules. Thus, the molecules are closely packed with little movement. As a consequence, both shape and volume are fixed.

In liquids, attraction and repulsion forces are similar. They have a little more movement than the solid state. Then, they do have a fixed volume but they adopt the shape of the container.

Gases have very weak attraction forces between their molecules. They move very freely and expand trying to occupy as much volume as possible. So, they have a variable volume and shape (adopt the shape of the container).

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Answer:

c. C3H9N2O2

Explanation:

The empirical formula of a compound is defined as the simplest whole number ratio of atoms present in a molecule. To solve this question we need to convert the mass of each atom to moles. With the moles we can find the ratio as follows:

Moles N -Molar mass: 14.01g/mol-

0.420g N * (1mol/14.01g) = 0.0300 moles N

Moles O -Molar mass: 16g/mol-

0.480g O * (1mol/16g) = 0.0300 moles O

Moles C -Molar mass: 12.01g/mol-

0.540g C * (1mol/12.01g) = 0.0450 moles C

Moles H -Molar mass: 1.0g/mol-

0.135g H * (1mol/1g) = 0.135moles H

Dividing in the moles of N (Lower number of moles) the ratio of atoms is:

N = 0.0300 moles N / 0.0300 moles N = 1

O = 0.0300 moles O / 0.0300 moles N = 1

C = 0.0450 moles C / 0.0300 moles N = 1.5

H = 0.135 moles H / 0.0300 moles N = 4.5

As the empirical formula requires whole numbers, multiplying each ratio twice:

N = 2, O = 2, C = 3 and H = 9

And the empirical formula is:

Answer:

[tex]K=1.7x10^{-3}[/tex]

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to solve this problem by firstly setting up the equilibrium expression for the given reaction, in agreement to the law of mass action:

[tex]K=\frac{[NO]^2}{[N_2][O_2]}[/tex]

Next, we plug in the given concentrations on the data table to obtain:

[tex]K=\frac{(0.034)^2}{(0.69)(0.98)}\\\\K=1.7x10^{-3}[/tex]

Regards!

Explanation:

here's the answer to your question

Answer:

4.858 g

Explanation:

Start with the formula

density = [tex]\frac{mass}{volume}[/tex]

density = 1.98 g/mL

volume = 2.45 mL

mass = ??

rearrange the formula to solve for mass

(density) x (volume) = mass

Add in the substitutes and solve for mass

1.98 g/mL x 2.45 mL = 4.858 g

Answer:

Explanation:

maleic acid ⇒ fumaric acid

ΔHreaction = ΔHproduct - ΔHreactant

ΔHproduct = -1336.0 kJ mol⁻¹

ΔHreactant = - 1359.2 kJ mol⁻¹.

ΔHreaction = -1336.0 kJ mol⁻¹ - ( - 1359.2 kJ mol⁻¹.)

=   1359.2 kJ mol⁻¹   -1336.0 kJ mol⁻¹

= 23.2 kJ mol⁻¹ .

Enthalpy of isomerization from maleic to fumaric acid is 23.2 kJ per mol.

Answer:

a) [tex]K_{2} S[/tex] and [tex]NH_{4} Cl[/tex] :

There are no insoluble precipitate forms.

b) [tex]Ca Cl_{2}[/tex] and [tex](NH_{4} )_{2} Co_{3}[/tex] :

There are the insoluble precipitates of [tex]CaCo_{3}[/tex]  forms.

c) [tex]Li_{2}S[/tex] and [tex]MnBr_{2}[/tex] :

There are the insoluble precipitates of [tex]MnS[/tex]  forms.

d) [tex]Ba(No_{3} )_{2}[/tex] and [tex]Ag_{2} So_{4}[/tex] :                        

As [tex]Ag_{2} So_{4}[/tex] is insoluble, therefore no precipitate forms.

e) [tex]Rb_{2}Co_{3}[/tex] and [tex]NaCl[/tex]:

There are no insoluble precipitates forms.

Explanation:

a)

Solubility rule suggests:- [tex]K_{2} S[/tex] ⇒ soluble, [tex]NH_{4} Cl[/tex] ⇒ soluble.

                                          KCl ⇒ soluble, [tex](NH_{4})_{2} S[/tex]  ⇒ soluble.

There are no insoluble precipitate forms.

b)

Solubility rule suggests:- [tex]Ca Cl_{2}[/tex] ⇒ soluble, [tex](NH_{4} )_{2} Co_{3}[/tex] ⇒ soluble.

                                        [tex]CaCo_{3}[/tex] ⇒ insoluble, [tex]NH_{4} Cl[/tex]  ⇒ soluble.

There are the insoluble precipitates of [tex]CaCo_{3}[/tex]  forms.

c)

Solubility rule suggests:- [tex]Li_{2}S[/tex] ⇒ soluble, [tex]MnBr_{2}[/tex] ⇒ soluble.

                                        [tex]LiBr[/tex] ⇒ soluble, [tex]MnS[/tex]  ⇒ insoluble.

There are the insoluble precipitates of [tex]MnS[/tex]  forms.

d)

Solubility rule suggests:- [tex]Ba(No_{3} )_{2}[/tex] ⇒ soluble, [tex]Ag_{2} So_{4}[/tex] ⇒insoluble.

As [tex]Ag_{2} So_{4}[/tex] is insoluble, therefore no precipitate forms.

e)

Solubility rule suggests:- [tex]Rb_{2}Co_{3}[/tex] ⇒ soluble, [tex]NaCl[/tex] ⇒ soluble.

                                        [tex]RbCl[/tex] ⇒ soluble, [tex]Na_{2} Co_{3}[/tex]  ⇒ soluble.

There are no insoluble precipitates forms.

Answer:

The molar heat of fusion for a given substance basically tells you how much heat is required to melt one mole of that substance at its melting point from two angles.

Explanation:

:)

Answer:

If 13.50 mL of an aluminum chloride solution is needed to reach the equivalence point with 10.00 mL of 0.109 M silver nitrate solution, determine the molarity of the aluminum chloride solution.

Explanation:

The balanced chemical equation of the reaction is:

[tex]AlCl_3(aq)+3AgNO_3(aq)->3AgCl(s)+Al(NO_3)_3(aq)[/tex]

So, one mole of aluminum chloride reacts with three moles of silver nitrate.

At the equivalence point,

the number of moles of each reactant must be equal.

The number of moles = molarity x volume in L.

Number of moles of AlCl3 = volume x molarity

=0.0135Lx Molarity

The number of moles of AgNO3 = 3 x 0.010Lx 0.109M

Thus,

0.0135Lx Molarity = 3 x 0.010Lx 0.109M

Molarity of AlCl3 :

[tex]Molarity of Alcl_3=3 x 0.010Lx 0.109M/0.0135\\=0.242M[/tex]

Answer is : 0.242M.

For consumption of each gram of reactant released=37.9 kJ/g

Therefore, for consumption of 4kg of reactant heat released=37.9x4 kJ/g

This question is incomplete, the complete question is;

In recrystallization from boiling water of benzoic acid contaminated with acetanilide, you begin with an impure sample of 5 grams. If the % composition of the acetanilide impurity in the sample is 6.3 %, what is the minimum amount in mL of solvent (water) required for the recrystallization

Compound      Solubility in water at 25°C      Solubility in water at 100°C

Benzoic Acid      0.34 g/100mL                           5.6 g/100mL

Acetanilide         0.53 g/100mL                           5.5 g/100mL

Answer:

The minimum amount in mL of solvent (water) required for the recrystallization is 91 mL

Explanation:

Given the data in the question;

mass of sample = 5 g

percentage composition of the acetanilide impurity = 6.3%

mass of the acetanilide in impure sample will be;

⇒ 6.3% × 5 g = 0.315 g

Mass of benzoic acid in impure sample;

⇒ 5 g - 0.315 g = 4.685 g

now, solubility in water at 100°C for benzoic acid = 5.6 g/100mL

hence 4.685 g of benzoic acid is soluble in x mL

x = [ 100 mL × 4.685 g ] / 5.6 g

x = 83.66 ≈ 84 mL

Also, solubility in water at 100°C for acetanilide = 5.5 g/100mL

hence 0.315 g of benzoic acid is soluble in x mL

x = [ 100 mL × 0.315 g ] / 5.5 g

x = 5.727 ≈ 6 mL

So, the minimum amount in mL of solvent (water) required for the recrystallization will be;

⇒ 85 mL + 6 mL = 91 mL

The minimum amount in mL of solvent (water) required for the recrystallization is 91 mL

Answer:

[tex]C_9H_8O_4+C_2H_3O_2^-\rightarrow C_2H_4O_2+C_9H_7O_4^-[/tex]

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to figure out the required net ionic equation by firstly writing out the complete molecular equation between aspirin and sodium acetate:

[tex]C_9H_8O_4+NaC_2H_3O_2\rightarrow C_2H_4O_2+NaC_9H_7O_4[/tex]

Whereas acetic acid and sodium acetylsalicylate are formed. Now, we write the complete ionic equation whereby sodium acetate and sodium acetylsalicylate are ionized because they are salts yet neither aspirin nor acetic acid are ionized as they are weak acids:

[tex]C_9H_8O_4+Na^++C_2H_3O_2^-\rightarrow C_2H_4O_2+Na^++C_9H_7O_4^-[/tex]

Finally, for the net ionic equation we cancel out the sodium spectator ions to obtain:

[tex]C_9H_8O_4+C_2H_3O_2^-\rightarrow C_2H_4O_2+C_9H_7O_4^-[/tex]

Regards!

Answer:

Frequency and wavelength are inversely proportional. c=f⋅λ (The speed of light is directly proportional to f and λ)

If Gold's natural state has a definite shape and a definite volume, then its natural state is solid.