For lunch today, I ate an apple. What type of carbohydrate did I ingest?

Answer:

option D

Explanation:

Increasing the temperature increases the yield of ammonia and speeds up the reaction as chemical reaction is affected by temperature.

Answer:

increasing the temperature decreases the yield of ammonia but speeds up the reaction

Explanation:

first pressure have no effect in chemical reaction

Answer:

See picture below

Explanation:

In the attached picture, you have the mechanism of all this reaction.

In the first step, as this is Friedel Craft acylation, we need to use either AlCl₃ or FeCl₃. So, this compound (I will use FeCl₃) will attach to the Chlorine group of the CH₃COCl.

In the second step, the whole CH₃CO is attached to the furan, because of the attack of the double bond of the ring.

After this, it occurs several resonance structure, to give a more stable structure, and the Hydrogen in the 2 position is substracted to give the final product of acylation.

Hope this helps.

Answer:

181.403 g/mol is the answer as it is Zinc chromate

Explanation:

Answer:

181.403 g/mol

Explanation:

Molar mass of ZnCrO4 = 181.3737 g/mol. This compound is also known as Zinc Chromate. Convert grams ZnCrO4 to moles or moles ZnCrO4 to grams. 65.38 + 51.9961 + 15.9994*4

Answer:

Al₂O₃ + 2 NaOH + 3 H₂O = 2 NaAl(OH)₄

Answer:

6

Explanation:

As , 2H2 + O2 = 2H2O

with 6 H2, 4O2 is excess.

H2O molecules formed = 6

Answer:

a. 87.8g/mol is the molar mass of the acid.

b. The answer is in the explanation.

Explanation:

To solve this question we must find the moles of the monoprotic acid using the reaction with NaOH (1mole of monoprotic acid reacts with 1 mole of NaOH). With the moles and the mass of the unknown we can find the molar mass.

Moles of NaOH added:

0.04121L * (0.150moles / L) = 6.1815x10⁻³ moles NaOH = Moles monoprotic acid

Molar mass is:

0.543g / 6.1815x10⁻³ moles = 87.8g/mol is the molar mass of the acid

b. I can't see the image you are giving because has a low resolution. But the identity of the acid can be obtained because the acid:

Has the same molar mass.

Is a monoprotic acid.

(a) The molecular mass of the unknown monoprotic acid will be 87.84 g/moles.

(b) The acid can be butyric acid, as it is a monoprotic and have mass near about 87.84 g/mol.

(a) The endpoint by the addition of NaOH has been reached when the monoprotic acid has been completely utilized. Since the NaOH has been monobasic. The moles of NaOH will be equal to the moles of acid.

Moles of NaOH = moles of acid

The molarity of NaOH = 0.15 M

Volume of NaOH = 41.21 ml

Molarity = [tex]\rm \dfrac{moles}{volume\;(L)}[/tex]

Moles = molarity [tex]\times[/tex] volume (L)

Moles of NaOH = 0.15 [tex]\times[/tex] 0.04121 L

Moles of NaOH = 0.00618 moles

Moles of NaOH = moles of acid

moles of acid = 0.00618 moles.

Mass of acid dissolved = 0.543 grams

Molecular weight of acid = [tex]\rm \dfrac{weight}{moles}[/tex]

Molecular weight of acid = [tex]\rm \dfrac{0.543}{0.006815}[/tex]

Molecular weight of acid = 87.84 g/moles.

(b) The acid with the molecular mass of 87.84 g/mol with being the monoprotic acid can be butyric acid. The butyric acid has a molecular weight of 88 g/mol.

For more information about monoprotic acid, refer to the link:

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Answer:

Option B, HCO3 1-

Explanation:

The valence of Sodium ion is +1 and the valence of HCO3 is -1. Thus, sodium ion has an extra electron to be donated to complete its outer shell  while HCO3 needs an electron to complete its outer shell

Hence Na will combine with HCO3 to form NaHCO3

Option B is correct

The polyatomic ion which will form an ionic compound with a single sodium ion is; HCO3 ¹-

In chemical bonding between ions;

The major criteria is a balance of charges within the compound formed.

As such, all polyatomic ions in the option are di-ionic except for HCO3 1- which can perfectly form an ionic compound with 1 single sodium ion.

Read more on ionic compounds:

https://brainly.com/question/13539062

Answer:

[tex]H^++NH_3\rightleftharpoons NH_4^+[/tex]

Explanation:

Hello there!

In this case, since the buffer is not given, we assume it is based off ammonia, it means the ammonia-ammonium buffer, whereas the ammonia is the weak base and the ammonium ion stands for the conjugate acid. In such a way, when adding HI to the solution, the base of the buffer, NH3, reacts with the former to promote the following chemical reaction:

[tex]H^++NH_3\rightleftharpoons NH_4^+[/tex]

Because the HI is totally ionized in solution so the iodide ion becomes an spectator one.

Best regards!

Answer:

the above answer is wrong

Explanation:

its really not but the mastering chemistry says it is

Answer:

As we move from left to right across a period, the ionization energy of elements increases. This is due to the decrease in the size of atoms across a period.

Answer:

[tex]\huge\boxed{Answer\hookleftarrow}[/tex]

____________________

ʰᵒᵖᵉ ⁱᵗ ʰᵉˡᵖˢ

# ꧁❣ RainbowSalt2²2² ࿐

Answer:

probably the sun

.

Explanation:

because the sun's heat result to evaporation

Answer:

B. The [H1+] >[OH1-] and the solution is acidic

Answer:

[tex]HCl conc=2.2M[/tex]

Explanation:

From the question we are told that:

Mass of zinc [tex]Mass_{z_n}=2.5g[/tex]

Initial conc of HCl [tex]HConc_1=6.0M[/tex]

Initial volume of HCl [tex]Hvol_1=20.0mL[/tex]

Molar mass of zinc [tex]M_{Z_n}=65.38g/mol[/tex]

Generally the equation for reaction  is mathematically given by

[tex]2HCL+Zn\implies ZnCl_2 +H_2[/tex]

Generally the equation for moles of zinc [tex]m_{z_n}[/tex] is mathematically given by

[tex]m_{z_n}=\frac{Mass_{Z_n}}{M_{Z_n}}[/tex]

[tex]m_{z_n}=\frac{2.5g}{M_{65.38}}[/tex]

[tex]m_{z_n}=0.038molZn[/tex]

Generally the equation for moles of [tex]m_{HCl}[/tex] is mathematically given by

[tex]m_{HCl}=HConc_1*Hvol_1[/tex]

[tex]m_{HCl}=6.0M*20.0mL[/tex]

[tex]m_{HCl}=6.0M*20.0*10^{-3}L[/tex]

[tex]m_{HCl}=0.12\ mol\ HCl[/tex]

Generally the reacted moles of HCl [tex]HCl_[reacted][/tex] is mathematically given by

Since

Zn:HCl =1:2

Therefore

[tex]HCl_[reacted]=0.038*\frac{2}{1}[/tex]

[tex]HCl_[reacted]=0.076mol \ HCl[/tex]

Generally the moles of HCl after Zn oxidization X is mathematically given by

[tex]x=0.12-0.076[/tex]

[tex]x=0.044 mol HCl[/tex]

Generally the conc of hydrochloride acid X is mathematically given by

[tex]X=\frac{0.044}{0.020}[/tex]

[tex]X=2.2 M Hcl[/tex]

Therefore Conc of HCl

[tex]HCl conc=2.2M[/tex]

Answer:

The answer is 200mL each amount have the same mass

Explanation:

100mL +100ML= 200mL mass in each container

Answer:

200ml

Explanation:

Answer:

General Characteristics of Acids:

Sour taste (though you should never use this characteristic to identify an acid in the lab) Reacts with a metal to form hydrogen gas. Increases the H+ concentration in water. Donates H+ ions. Turns blue litmus indicator red.

Answer:

a) 2,4-dinitrobenzoic acid: the most acidic compound, p-nitrobenzoic acid: _______, p-bromobenzoic acid: the least acidic compound

b) oxalic acid: the most acidic compound, acetic acid: the least acidic compound, formic acid: _______.

c) p-cyanobenzoic acid: the least acidic compound, benzoic acid: the most acidic compound, p-aminobenzoic acid: _______.

Explanation:

a) 2,4-dinitrobenzoic acid is the most acidic compound of this set because it has two strong electronegative substituents (nitrogen dioxide) which increases the acidity of benzoic acid, while p-bromobenzoic acid is the least acidic compound because bromine is a weaker electron withdrawing group than nitrogen dioxide.

b) The presence of 2 -COOH group makes Oxalic acid the most acidic compound of this set, while decrease in acidity of carboxylic acid due to the presence of methyl group on carbon of -COOH group makes acetic acid the least acidic compound of this set.  

(c) Benzoic acid has a higher acid dissociation constant value (4.45 Ka) therefor it is the most acidic compound of this set, while p-cyanobenzoic acid is the least acidic compound of this set as it has the least acid dissociation constant value (16 Ka).

Answer:

B

Explanation:

Answer:

Atoms

Explanation:

Atoms are the smallest thing meaning they form molecules which are made of atoms.

Also, your question is not 93 points but whatever lol.

Answer:

Atoms

Explanation:

I took the test

Answer - 1.50 M Na

Explanation -

3.00 moles of Na over 2.00 L of water.

3.00/2.00 = 1.50 M Na

I cannot be entirely sure. But it's an educated guess.

Answer:

At 10 ∘C , the solubility of potassium chloride is measured to be 31.2⋅g per 100⋅g of water.

Explanation:

Answer:

Chlorine gas bleaches the damp litmus (red or blue). Bleaching is an oxidation process.

Explanation:

Answer:

Chlorine gas bleaches the damp litmus (red or blue). Bleaching is an oxidation process. If you are considering the colour change only - refer to it as bleaching. If you are considering the reaction mechanism and how the chemicals which provide the colour are changed, then refer to it as oxidation.

Explanation:

Answer:

option first is right answer

Answer:

Explanation:

The number of molecules can be found by using the formula

N = n × L

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question we have

N = 3 × 6.02 × 10²³

We have the final answer as

Hope this helps you

Answer: OB. 1.806 x 1024

Explanation:

Answer:

1. 2.41 × 1023 formula units

2. 122 L

3. 7.81 L

Explanation:

1. Equation of the reaction: 2 Na(NO3) + Ca(CO3) ---> Na2(CO3) + Ca(NO3)2

Mole ratio of NaNO3 to CaCO3 = 2 : 1

Moles of CaCO3 = mass/molar mass

Mass of CaCO3 = 20 g; molar mass of CaCO3 = 100 g

Moles of CaCO3 = 20 g/100 g/mol = 0.2 moles

Moles of NaNO3 = 2 × 0.2 moles = 0.4 moles

1 Mole of NaNO3 = 6.02 × 10²³ formula units

0.4 moles of NaNO3 = 0.4 × 6.02 × 10²³ = 2.41 × 1023 formula units

2. Equation of reaction : 2 H2O ----> 2 H2 + O2

Mole ratio of oxygen to water = 1 : 2

At STP contains 6.02 × 10²³ molecules = 1 mole of water

6.58 × 10²⁴ molecules = 6.58 × 10²⁴ molecules × 1 mole of water/ 6.02 × 10²³ molecules = 10.93 moles of water

Moles of oxygen gas produced = 10.93÷2 = 5.465 moles of oxygen gas

At STP, 1 mole of oxygen gas = 22.4 L

5.465 moles of oxygen gas = 5.465 moles × 22.4 L/1 mole = 122 L

3.Equation of reaction: 6 K + N2 ----> 2 K3N

Mole ratio of Nitrogen gas and potassium = 6 : 1

Moles potassium = mass/ molar mass

Mass of potassium = 90.0 g, molar mass of potassium = 39.0 g/mol

Moles of potassium = 90.0 g / 39.0 g/mol = 2.3077moles

Moles of Nitrogen gas = 2.3077 moles / 6 = 0.3846 moles

At STP, 1 mole of nitrogen gas = 22.4 L

0.3486 moles of oxygen gas = 0.3486 moles × 22.4 L/1 mole = 7.81 L

1. Volume of oxygen 2.41 × 1023   units

2. Nitrogen gas 122 L

3. 7.81 L

Equation of the reaction:

[tex]\rm 2Na(No_3)+Ca(Co_3)---- > Na_2(Co_3)+Ca(No_3)_2[/tex]

[tex]NaNo_3\ and \ CaCo_3=\dfrac{2}{1}[/tex]

[tex]\rm Moles \ of \ CaCo_3=\dfrac{Mass}{Molar\ Mass}[/tex]

Mass of CaCO3 = 20 g; molar mass of CaCO3 = 100 g

[tex]\rm \ Moles \ of \ CaCo_3=\dfrac{20}{100} =0.2[/tex]

[tex]Moles \ of \ NaNo_3=2\times 0.2=0.4\ moles[/tex]

[tex]1\ mole\ of \ NaNo_3=6.02\times10^{23}[/tex]

0.4 moles of NaNO3 = [tex]0.4\times 6.02\times 10^{23}=2.41\times 10^{23}[/tex]  

2. Equation of reaction :[tex]2H_2o---- > 2H_2+o_2[/tex]  

The mole ratio of oxygen to water =  [tex]\dfrac{2}{1}[/tex]

At STP contains

 [tex]\dfrac{6.02\times 10^{24}\times 1 \ mole \ of \ water}{6.02\times 10^{23}} =10.93\ moles \ of \ water[/tex]

Moles of oxygen gas produced =

[tex]\dfrac{10.93}{2} =5.465\ Moles \ of \ oxygen \ gas[/tex]

At STP, 1 mole of oxygen gas = 22.4 L

5.465 moles of oxygen gas =    [tex]5.465\times 22.4=122\ L[/tex]  

3. Equation of reaction:

[tex]6k+N_2---- > 2K_3N[/tex]6

The mole ratio of Nitrogen gas and potassium =   [tex]\dfrac{6}{1}[/tex]

[tex]Moles\ of \ potassium = \dfrac{Mass}{Molar\ Mass}[/tex]

Mass of potassium = 90.0 g,

molar mass of potassium = 39.0 g/mol

[tex]Moles\ of \ potassium = \dfrac{90}{39}=2.3077\ moles[/tex]

[tex]Moles\ of \ Nitrogen = \dfrac{ 2.3077}{6}=0.3846\ moles[/tex]

At STP, 1 mole of nitrogen gas = 22.4 L

0.3486 moles of oxygen gas =

[tex]0.3486\times 22.4=7.81\ L[/tex]

Thus

1. Volume of oxygen 2.41 × 1023   units

2. Nitrogen gas 122 L

3. 7.81 L

To know more about Stoichiometry follow

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0.52 molar is the molarity of a solution in which 0.257 moles of HNO2 is dissolved in 490ml of water.

The term molarity is defined as the number of moles of solutes are dissolved in per litre of solution. It is represented by the symbol "M". The unit of molarity is molar(M).

To calculate the molarity of a solution, divide the moles of solute by the volume of the solution expressed in liters.

The formula of molarity = a number of moles of solutes /  litre of solution

Given:

Number of moles = 0.257 moles

Volume = 490ml = 0.49 litre

Molarity = ?

According to the definition of molarity,

Molarity = Number of moles of solute / litre of solution

Molarity =  0.257 moles / 0.49 litre

Molarity = 0.52 molar

Thus, the molarity of a solution in which 0.257 moles of HNO2 is dissolved in 490ml of water is 0.52 molar.

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Answer:

B

Explanation:

Answer:

Percentage yield = 61.7%

Explanation:

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

2AgNO₃ + Cu —> Cu(NO₃)₂ + 2Ag

Next, we shall determine the mass of AgNO₃ that reacted and the mass of Ag produced from the balanced equation. This is illustrated below:

Molar mass of AgNO₃ = 108 + 14 + (16×3)

= 108 + 14 + 48

= 170 g/mol

Mass of AgNO₃ from the balanced equation = 2 × 170 = 340 g

Molar mass of Ag = 108 g/mol

Mass of Ag from the balanced equation = 2 × 108 = 216 g

SUMMARY:

From the balanced equation above,

340 g of AgNO₃ reacted to produce 216 g of Ag.

Next, we shall determine the theoretical yield of Ag. This can be obtained as follow:

From the balanced equation above,

340 g of AgNO₃ reacted to produce 216 g of Ag.

Therefore, 51 g of AgNO₃ will react to produce = (51 × 216)/340 = 32.4 g of Ag.

Thus, the theoretical yield of Ag is 32.4 g.

Finally, we shall determine the percentage yield of Ag. This can be obtained as follow:

Actual yield = 20 g

Theoretical yield = 32.4 g

Percentage yield =?

Percentage yield = Actual yield /Theoretical yield × 100

Percentage yield = 20 / 32.4 × 100

Percentage yield = 61.7%