What is the net ionic equation for Fe(NO3)3+3NaOH=Fe(OH)3+3NaNO3

The molecule described below is known as :

2-pentene.

In the diagram below:

As a result, the compound is 2 pentene.

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The number of moles of NO₂ formed when 10.2 moles of NO₃ reacts is 20.4moles.

According to this question, nitrogen IV oxide (NO₂) reacts with nitrogen II oxide (NO) to form nitrogen VI oxide (NO₃) as follows:

NO₃ + NO → 2NO₂

The number of moles of either the reactants or the products can be calculated stoichiometrically as follows:

Based on the above chemical equation, 1 moles of NO₃ reacts to form 2 moles of NO₂.

This means that if 10.2 moles of NO₃ reacts, 10.2 × 2 = 20.4 moles of NO2 will be produced.

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Answer:

1.06

Explanation:

One mole of nitrogen is 14.009, or the mass number and you divide 14.9 by 14.009 and get 1.06 for the amount of moles

Answer:

1.063753837 mol

Explanation:

14.9 * (1/14.007) = 1.063753837

Original grams * (1 mol/atomic weight of nitrogen) = 1.063753837

Answer:yes

Explanation: Because i can help u

Answer:

I believe it is the last choice

Explanation:

Isotopes of a certain element must have the same atomic number(the # of protons). This is what differentiates the different elements. However, isotopes could have varying amounts of neutrons, therefore the atomic mass could vary as well.

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Si3P4 this is the answer i beleive!

The number of nickel atoms that would be laid side by side to span a distance of 2.65 mm is 1.06 x 10⁷ atoms of nickel.

The diameter of the nickel atom is the line that divides the nickel atom into two equal halves. The diameter of an object is always double of the radius when the radius of the atom is known.

The diameter of the nickel atom is calculated as follows;

d = 2r

where;

d = 2 x 125 pm

d = 250 pm

d = 2.5 x 10⁻¹⁰ m

The number of nickel atoms that would be laid side by side to span a distance of 2.65 mm is calculated as follows;

n(2.5 x 10⁻¹⁰ m) = 2.65 mm

n(2.5 x 10⁻¹⁰ m) = 2.65 x 10⁻³ m

n = (2.65 x 10⁻³) / (2.5 x 10⁻¹⁰)

n = 1.06 x 10⁷ atoms of nickel

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The concentration of the 27.7 mL H₃PO₄ solution is 0.323 M

We'll begin by writing the balanced equation for the reaction. This is given below:

H₃PO₄ + 3NaOH —> Na₃PO₄ + 3H₂O

From the balanced equation above, we obatined:

CaVa / CbVb = nA / nB

(Ca × 27.7) / (0.609 × 44.1) = 1 / 3

(Ca × 27.7) / 26.8569 = 1 / 3

Cross multiply

Ca × 27.7 × 3 = 26.8569

Ca × 83.1 = 26.8569

Divide both side by 83.1

Ca = 26.8569 / 83.1

Ca = 0.323 M

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Answer:

yess Petroleum—or crude oil—is a fossil fuel that is found in large quantities beneath the Earth's surface and is often used as a fuel or raw material in the chemical industry.

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The gram molecular masses of the following species are

H₂O is a compound.

molecular mass H₂O :

mass of hydrogen = 1 g/mol

mass of oxygen = 16 g/mol

molecular mass of H₂O = 2 × 1 + 16

                                       = 18 g/mol

C₁₂H₂₂O₁₁ is a compound.

mass of carbon = 12 g/mol

mass of hydrogen = 1 g/mol

mass of oxygen = 16 g/mol

molecular mass of C₁₂H₂₂O₁₁ = 12 × 12 + 22 × 1 + 11 × 16

                                                = 144 + 22 + 176

                                                = 342 g/mol

-----(C₃H₆)₁₀₀----- Polypropylene is a compound.

mass of carbon = 12 g/mol

mass of hydrogen = 1 g/mol

molecular mass of -----(C₃H₆)₁₀₀₀----- = (3 × 12 + 6 × 1 ) × 1000

                                                            = 42000 g/mol

Al₂O₃ ( aluminum oxide ) is chemical compound.

mass of aluminum = 27 g/mol

mass of oxygen = 16 g/mol

molecular mass = 2 × 27 + 3 × 16

                          = 102 g/mol

S₆ (sulfur powder)

mass of sulfur = 32 g/mol

molar mass of = 6 × 32

                        = 192 g/mol

CHCl₃ ( chloroform) is a compound

mass of carbon = 12 g/mol

mass of hydrogen = 1 g/mol

mass of chlorine = 35 g/mol

molar mass of CHCl₃ = 12 + 1 + 3 × 35

                                   = 119 g/mol

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Mole measure the number of elementary entities of a given substance that are present in a given sample. Therefore, 0.02moles of NH₃ are there in 500cm³ of the gas.

The SI unit of amount of substance in chemistry is mole. The mole is used to measure the quantity or amount of substance. We know one mole of any element contains 6.022×10²³ atoms which is also called Avogadro number.

Mathematically,

number of moles of any ideal gas =given volume ÷Volume occupied by one mole of a ideal gas at STP

Volume occupied by one mole of a ideal gas at STP=22400cm³

given volume of NH₃=500cm³

substituting all the given values in the above equation we get,

number of moles of NH₃ =500 ÷22400

number of moles of NH₃ =0.02moles

Therefore, 0.02moles of NH₃ are there in 500cm³ of the gas.

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First, we need to figure the reaction out.

Both reactants are ionic compounds, so their reaction is probably a double displacemente reaction.

The Cl has a charge of 1-, so Fe has a charge of 2+. Na has a charge of +1 and PO₄ has a charge of 3-.

To combine Fe²⁺ with PO₄³⁻, we will need 3 Fe²⁺ and 2 PO₄³⁻, so the compound becomes neutral.

Both Na and Cl have single charge, so their combination is simply 1 Na and 1 Cl.

So, the products are Fe₃(PO₄)₂ and NaCl, so the unbalanced reaction is:

To balance it, We can start by putting a coefficient of 2 on Na₃PO₄, so we have two PO₄³⁻ anions on both sides:

Now, we put a coefficient of 3 on FeCl₂ and 6 on NaCl to get the balanced equation:

Now, we first need to calculate the number of moles of each reactant, using their molar masses:

So:

Now, if the coefficient of FeCl₂ is 3, for each 3 FeCl₂ that reacts, one reaction occurs, so the number of reactions that will need to occur to consume all its number of moles is that amount over 3:

Similarly, we get the number of reactions that would occur if all Na₃PO₄ reacts by dividing its number of moles by its coefficient, that is 2:

This means that the amount we have of FeCl₂ is enough for only about 0.0605 mol of reactions while the amount we have of Na₃PO₄ is enought for about 0.1250 mol of reactions, which is more than the other reactant.

This means that the reactant that limits the amount of reaction that can occur is FeCl₂, so the limiting reactant is FeCl₂.

By the definition of molarity, 1000ml of HCl solution contains 0.0858 moles of HCl.

The moles of HCl in 21ml of solutions can be obtained as follows-

Moles of HCl = 21ml *0.0858moles/1000ml

                     = 0.0081moles

Hence, moles of ethylamine =0.0081moles

Now,

the molarity of ethylamine solutions can be obtained as follows-

Since,

35ml of ethylamine solution contains 0.0018moles

the moles of ethylamine in 1000ml of the solution(molarity) can be obtained as-

Molarity = 1000ml/L * 0.0018mol/35ml

            = 0.0514 M

Hence,

the molarity of ethylamine solution is 0.0514 M

This is because, to find molarity of a solution considering a titration curve  which is a plot of pH v/s volume of titrant. The equivalence point in the titration curve is the point at which there is a significant change in pH with small addition of titrant. At the equivalence point, the moles of titrant equal the moles of analyte.

The volume of the HCl solution added to reach the equivalence point is 21ml.

At this point, the moles of HCl = moles of ethylamine

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Answer: The correct option is ○ O₂

Explanation:

All the other options denote that they are not a single element theyare  

in compound form. Only the oxygen is in element form.

40.4417g of PbS is formed from 55.11g of Pb(C2H3O2)2 and excess amount of H2S .

Given,

balanced chemical equation is ,

Pb(C2H3O2)2 (s) + H2S (g) ⇒ PbS (s) + HC2H3O2 (g)

to making the chemical equation balanced , we have to make sure that all the molecules on the left hand side and in the right hand side should be equal .

thus to making it equal 1st see that the number of carbon , oxygen and hydrogen is doubled in the left side than that of right side .

so we have to multiply HC2H302 by 2 .

Pb(C2H3O2)2 (s) +H2S(g) ⇒ PbS(s) + 2 HC2H3O2 (g)

so now the given chemical equation is balanced that we can say , 1 mol of       Pb(C2H3O2)2 produces 1 mol of PbS .

It is given that , we can take H2S is in excess means the Pb(C2H3O2 )2 acts as limiting agent .

We know , molecular mass of Pb(C2H3O2)2 is 325.29g

325.29g contains 1mole

55.11g contains 55.11/325.29 = 0.169 moles

thus ,the mole of PbS formed from 55.11g of Pb(C2H3O2)2 is 0.169moles.

We know ,

molecular mass of PbS is 239.3g

1mole of PbS is 239.3g

0.169moles pf PbS is 239.3×0.169 = 40.4417 g

Hence , 40.4417g of PbS is formed from 55.11g of Pb(C2H3O2)2 and excess amount of H2S .

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The limiting reactant is lead(II) acetate the theoretical yield is 1.1909 g and the percent yield is 83.71 %.

The amount of the sample in a specific solution volume is known as its molarity (M). The molarity of a solute per liter of the a solution is known as molar ratio. The molar concentration in a solution is another name for molarity.

Molarity

= moles of solute/volume of the solution

or Moles

= Molarity * volume of solution

For potassium sulfate :

Molarity = 0.116 M

Volume = 56.0 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume = 56.0×10⁻³ L

Thus, moles of potassium sulfate:

Moles = 0.116 M * 56.0 * 10-3 moles

Moles of potassium sulfate  = 0.006496 moles

For lead(II) acetate :

Molarity = 0.102 M

Volume = 38.5 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume = 38.5×10⁻³ L

Thus, moles of lead(II) acetate :

Moles = 0.102 * 38.5 *10-3 moles

Moles of lead(II) acetate  = 0.003927 moles

According to the given reaction:

[tex]$\mathrm{K}_2 \mathrm{SO}_{4(a q)}+\mathrm{Pb}\left(\mathrm{C}_2 \mathrm{H}_3 \mathrm{O}_2\right)_{2(a q)} \rightarrow 2 \mathrm{KC}_2 \mathrm{H}_3 \mathrm{O}_{2(s)}+\mathrm{PbSO}_{4(a q)}$[/tex]

1 mole of potassium sulfate react with 1 mole of lead(II) acetate

0.006496 moles potassium sulfate react with 0.006496 mole of lead(II) acetate

Moles of lead(II) acetate = 0.003927 moles

Lead(II) acetate is limiting reagent. ( 0.003927 < 0.006496)

0.003927 mole of lead(II) acetate gives 0.003927 mole of lead(II) sulfate

Molar mass of lead(II) sulfate = 303.26 g/mol

Mass of lead(II) sulfate = Moles × Molar mass = 0.003927 × 303.26 g = 1.1909 g

Theoretical yield = 1.1909 g

Given experimental yield = 0.997 g

% yield = (Experimental yield / Theoretical yield) × 100 = (0.997/1.1909 g) × 100 = 83.71 %

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INFORMATION:

We have the neutralization of a weak base and a strong acid, and we must determine what should be the product of the reaction

STEP BY STEP EXPLANATION:

To determine it, we need to know that:

- The neutralization of a strong acid and strong base has a pH equal to 7. The neutralization of a strong acid and weak base will have a pH of less than 7, and conversely, the resulting pH when a strong base neutralizes a weak acid will be greater than 7.

In our case, we have the neutralization of a weak base and a strong acid, so our product would have a pH of less than 7. Then, knowing that a pH less than 7 represents an acidic, we can state that the product of the reaction will be an acidic.

A strong acid and a weak base yield a weakly acidic solution, not because of the strong acid involved, but because of the conjugate acid of the weak base.

ANSWER:

d. acidic

When a potent acid, like hydrochloric acid, HCl, is combined with a potent base, such sodium hydroxide, NaOH, the result can be complete neutralization. Strong bases and acids dissociate entirely into their individual ions when they dissolve in water.

An element's valency is its capacity for combination. The periodic table groups have identical elements with the same valency.. How many electrons make up the outer shell of an element determines its valency. The group number.

Valency is simply the amount of electrons that an element's atom gains, loses, or shares to obtain the closest configuration to that of a noble gas. The valency of sodium (Na), magnesium (Mg), chlorine (Cl), and other elements, for instance, is 1.

When there are equal moles of strong acid and strong base, the strong acid and strong base completely neutralize one another. An aqueous solution with a pH of 7 is the end product.

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Taking into account definition of percent yield, the percent yield of the reaction if 3.35 g of N₂H₄ reacts with excess oxygen and produces 0.350 L of N₂ is 13.82%.

In first place, the balanced reaction is:

N₂H₄ + O₂ → N₂ + 2 H₂O

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

The molar mass of the compounds is:

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P×V = n×R×T

where:

The percent yield is the ratio of the actual return to the theoretical return expressed as a percentage.

The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:

percent yield= (actual yield÷ theoretical yield)× 100%

where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.

In this case, you know:

Replacing in the ideal gas law:

1 atm×0.350 L = n×0.082 [tex]\frac{atmL}{molK}[/tex]× 295 K

Solving:

n= (1 atm×0.350 L) ÷ (0.082 [tex]\frac{atmL}{molK}[/tex]× 295 K)

n= 0.01447 moles

Finally, the actual yield of N₂ is 0.01447 moles.

Considering the limiting reagent, the following rule of three can be applied: if by reaction stoichiometry 32 grams of N₂H₄ form 1 mole of N₂, 3.35 grams of N₂H₄ form how many moles of N₂?

moles of N₂= (3.35 grams of N₂H₄× 1 moles of N₂)÷ 32 grams of N₂H₄

moles of N₂= 0.1047 moles

Finally, the theoretical yield of N₂ is 0.1047 moles.

In this case, you know:

Replacing in the definition of percent yield:

percent yield= (actual yield÷ theoretical yield)× 100%

Solving:

percent yield= (0.01447 moles÷ 0.1047 moles)× 100%

percent yield= 13.82%

Finally, the percent yield for the reaction is 13.82%.

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The number of the moles of the P₂H₄ is equal to 1.734 moles, which will generate 1.76×10²³ molecules of P₄.

The equation in which the total mass of substances on the reactant side is equal to the total mass of substances on the product side is known as a balanced chemical equation.

The law of conservation of mass must obey by a balanced chemical equation. The given balanced chemical reaction of the reaction of P₂H₄ is :

6 P₂H₄  → 8 PH₃  +   P₄

The number of molecules of the phosphorous  P₄ formed = 1.76 × 10²³

The number of moles of  P₄ = 1.76 × 10²³/(6.022 × 10²³) = 0.292 mol

One of the phosphorous P₄ is formed from  P₂H₄ = 6 mol

Then  0.292 mol of P₄ will form from  P₂H₄ = 6× 0.292 = 1.734 mol

Therefore, the 1.734 moles of P₄ are required to form 1.76×10²³ molecules of P₂H₄.

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A chemist measures the enthalpy change ∆H during the reaction COCl2(g)+4NH3(g)--->CO(NH2)2(s)+2NH4Cl(s). Then ∆H = -140 KJ.

The amount of heat that gets released or absorbed during a reaction and that takes place under constant pressure is referred to as the enthalpy change. The sign for it is H, which can be read as “∆H.”

Note that only reactions carried out under constant pressure are covered by the phrase “enthalpy change.”

The main distinction that comes in between enthalpy and entropy, which exists despite the fact that they are both components of a thermodynamic system, is that the enthalpy is expressed as the total amount of heat content whereas altogether the entropy is the level of disorder.

The whole internal energy is represented by enthalpy. And volume times pressure. The enthalpy of a system cannot be measured, although enthalpy variations can be observed.

[tex]CoCl_{2}[/tex] + [tex]4NH_{3}[/tex] →[tex]CO(NH_{2} )_{2} + 2 NH_{4}Cl\\[/tex]

∆H = -559 Kj

Then reverse the above reaction and multiply with 2 as sign of ∆H changes from -ve to +ve

[tex]2CO(NH_{2})_{2} + 4NH_{4}Cl[/tex] → [tex]2COCl_{2} + 8NH_{3}[/tex]

∆H = -559 x 2

= 1118 Kj

[tex]CoCl_{2}[/tex] + [tex]4NH_{3}[/tex] →[tex]CO(NH_{2} )_{2} + 2 NH_{4}Cl\\[/tex]

∆H = -559 Kj

Reverse the above reaction ∆H changes from -ve to +ve

[tex]CO(NH_{2})_{2} + 2NH_{4}Cl[/tex] → [tex]COCl_{2} + 4NH_{3}[/tex]

∆H = +559 Kj

[tex]CoCl_{2}[/tex] + [tex]4NH_{3}[/tex]  → [tex]CO(NH_{2} )_{2} + 2 NH_{4}Cl\\[/tex]

∆H = -559 Kj

Above equation is divided with 4

[tex]\frac{1}{4}[/tex][tex]CoCl_{2}[/tex] + [tex]NH_{3}[/tex] → [tex]\frac{1}{4}[/tex] [tex]CO(NH_{2} )_{2} + \frac{1}{2} NH_{4}Cl\\[/tex]

∆H = -559/4 KJ

= -139.8 KJ

≈ -140 KJ

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The 1.662 × 10¹⁸ protons per second will shine on the chemistry text from a 250 W bulb.

A photon or light quantum, is an energy packet of electromagnetic radiation. Einstein suggested the presence of discrete energy packets during the transmission of light and deduced that the light quantum is associated with momentum (hν/c).

A photon is defined as a discrete bundle of electromagnetic energy that also moves at the speed of light (3 × 10⁸ m/s).

The energy of a single photon with a wavelength (λ) of 550 nm can be calculated from the following equation:

E = hc/λ

Where h is Planck's constant has a value equal to 6.626*10⁻³⁴ J·s.

E = (6.626 × 10⁻³⁴ J·s × 3×10⁸ m/s) / (550 ×10⁻⁹m)

E = 3.614 × 10⁻¹⁹ J.

It means that the energy of one photon is equal to 3.614 × 10⁻¹⁹ J.

[tex]1J/s \times \frac{1photon}{3.614 \times 10^{-19} J.}[/tex]

= 2.77 × 10¹⁸ proton/s = 1 Watt

Given, a 200 W bulb converts 5% of its output into light, therefore

200* 5/100 = 6 W

Then 6 watts has photons = [ 2.77 ×10¹⁸ proton/s * 6 ] = 16.62 × 10¹⁸ proton/s

If only 10% of the light will shine on year chemistry textbook, Then

16.62 × 10¹⁸ proton/s × 10/100 = 1.662 × 10¹⁸ protons/s

The number of photons shining on chemistry text = 1.662 × 10¹⁸ protons

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System and surroundings:

A system is defined as a matter or region on which analysis is done. The system is separated from the surroundings by the boundary. Everything external to the system is surrounding.

Specific heat function:

The amount of heat that must be added to one unit of mass of the substance in order to cause an increase of one unit in temperature.

Enthalpy changes:

We could say that it is equal to the difference between the energy used to break bonds in a chemical reaction and the energy gained by the formation of new chemical bonds in the reaction.

Standard enthalpy of formation: ​

It is a measure of the energy released or consumed when one mole of a substance is created under conditions from its pure elements.

For a structure of the CH3Br structure, see attached image.

A covalent compound is represented by a lewis structure structure, in which valence electrons, lone pairs, and bonding electrons are represented by dots. Sir G.N. Lewis first described the method in his 1916 article "Atom and Molecule."

They are also known as molecular dot electron diagrams. The CH3Br molecule has fourteen electrons in total. As may be plainly seen in the attached image, each element's atom is surrounded by dots to represent its valence electrons.

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Answer:

Demonstrative evidence

Based on the balanced chemical equation, the volume of 0.250 M  K₂S₂O₃ (aq) needed to completely react with 37.32 mL of 0.125 M KI₃ (aq) is 37.32 mL.

The reaction between K₂S₂O₃ (aq) and KI₃ (aq) is a redox reaction.

The balanced chemical equation of the reaction is given as follows:

2 S₂O₃²⁻ (aq) + I₃⁻ (aq) ---> S₄O₆²⁻ (aq) + 3 I⁻ (aq)

Based on the balanced equation of the reaction:

2 moles of K₂S₂O₃ (aq) are required to react with one mole KI₃ (aq).

Moles of KI₃ (aq) in  37.32 mL of 0.125 M solution;

Moles of  KI₃ (aq) = 37.32 * 0.125 M

Moles of  KI₃ (aq) = 4.665 mmoles

Moles of K₂S₂O₃ (aq) required = 2 *  4.665 mmoles

Moles of K₂S₂O₃ (aq) required = 9.33 mmoles

Volume of K₂S₂O₃ (aq) required =moles / molarity

The volume of K₂S₂O₃ (aq) required = 9.33 / 0.25

The volume of K₂S₂O₃ (aq) required = 37.32 mL

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Answer:

0.686 M

Explanation:

To find the molarity of C₂H₆O, you need to (1) convert grams to moles (using the molar mass of C₂H₆O) and then (2) calculate the molarity (using the molarity ratio). The final answer should have 3 sig figs like the given values.

(Step 1)

Atomic Mass (C): 12.011 g/mol

Atomic Mass (H): 1.008 g/mol

Atomic Mass (O): 15.999 g/mol

Molar Mass (C₂H₆O): 2(12.011 g/mol) + 6(1.008 g/mol) + 15.999 g/mol

Molar Mass (C₂H₆O): 46.069 g/mol

  74.6 g C₂H₆O               1 mole
-------------------------  x  --------------------  =  1.62 moles C₂H₆O
                                      46.069 g

(Step 2)
Molarity = moles / volume (L)

Molarity = 1.62 moles C₂H₆O / 2.36 L

Molarity = 0.686 M

Answer:

400CaO and 0g C02

Explanation: 400 has more moiul

The pressure at which balloon bursts is 3.07 psi , when expands and bursts after ascending until the temperature is -35 degree celsius.

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