rank the following compounds in order of increasing mass precetnage of nitrogen: NO, NO₂, N₂O.

Answer:

all are correct

Explanation:

AI Consist of 3 valence electrons we would make all tree images correct

H2NCH2CO2-

A chelating agent is a compound that can form multiple bonds with a metal ion, effectively surrounding and "grabbing onto" the ion. The H2NCH2CO2- molecule, also known as ethylenediaminetetraacetic acid (EDTA), contains multiple amine and carboxylate functional groups that can bind to metal ions, making it an effective chelating agent.

H2O, SCN-, and SH- are not typically considered chelating agents as they do not contain multiple functional groups that can bind to metal ions in the same way as EDTA. However, they may still have some ability to bind metal ions in certain circumstances, such as when the metal ion has a high affinity for the particular functional group present in the molecule.
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Answer:

Many metals (such as zinc, tin, lead, aluminium, and beryllium) form amphoteric oxides or hydroxides. Amphoterism depends on the oxidation states of the oxide. Al2O3 is an example of an amphoteric oxide.

Answer:

Lead (II) oxide and zinc (II) oxide

Answer: Good for her?

Explanation:

What is the experiment? your question don't have enough info.

(a) CH3CH2OH has a higher boiling point than CH3CH2CH3 due to hydrogen bonding. (b) NH3 has a higher boiling point than PH3 . (c) NO has a higher boiling point than N2.

(a) The substance with the higher boiling point is CH3CH2OH, as it can form intermolecular hydrogen bonds, which are stronger than the intermolecular forces in CH3CH2CH3.(b) The substance with the higher boiling point is NH3, as it can form hydrogen bonds, while PH3 can only form weaker London dispersion forces.(c) The substance with the higher boiling point is NO, as it has a polar covalent bond and can form stronger dipole-dipole interactions compared to N2, which is a nonpolar molecule and only has weak London dispersion forces.

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Answer:

2 vials

Explanation:

The concentration (C) of the drug in the solution is:

C= 500 mg/5 mL = 100 mg/mL

Each vial with a volume (V) of 10 mL, contains the following mass of drug:

V= 10 mL ⇒ C x V = 100 mg/mL x 10 mL = 1000 mg

As you need 2.00 g, and 1 gram is equivalent to 1000 mg, the mass needed is 2.00 g x 1000 mg/1 g = 2000 mg

Thus, you have to divide the mass you need into the mass of each vial:

(2000 mg)/(1000 mg/vial) = 2 vials

Therefore, you need 2 vials.

Answer: 0.071 moles of excess reactant \((O_2)\) will be left over.

Explanation:

To calculate the moles, we use the equation:

\(\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}\)

a) moles of \(NO\)

\(\text{Number of moles}=\frac{21.6g}{30.01g/mol}=0.720moles\)

b) moles of \(O_2\)

\(\text{Number of moles}=\frac{13.8g}{32g/mol}=0.431moles\)

\(2NO(g)+O_2(g)\rightarrow 2NO_2(g)\)

According to stoichiometry :

2 moles of \(NO\) require 1 mole of \(O_2\)

Thus 0.720 moles of  \(NO\) require=\(\frac{1}{2}\times 0.720=0.360moles\) of \(O_2\)

Thus \(NO\) is the limiting reagent as it limits the formation of product and \(O_2\) is the excess regaent.

moles of \(O_2\) left = (0.431-0.360) = 0.071 moles

A prosthetic group is a non-protein molecule that is tightly bound to a protein and is essential for its function. It can be either organic or inorganic. Examples of prosthetic groups include heme in hemoglobin and chlorophyll in photosynthesis.

A cofactor is a non-protein molecule that is required for the proper functioning of an enzyme. It can be either organic or inorganic. Cofactors can bind to the enzyme transiently or can be tightly bound to it. Examples of cofactors include metal ions such as zinc and magnesium.
A coenzyme is a type of cofactor that is an organic molecule. It acts as a carrier of chemical groups or electrons that are required for enzyme-catalyzed reactions. Coenzymes are often derived from vitamins. Examples of coenzymes include NAD+ and FAD in cellular respiration.

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To distinguish between a carboxylic acid, an ester, and an amine, you can perform a series of tests that take advantage of their unique chemical properties.

Here are some common tests that can help differentiate between these functional groups:

Acid-Base Reaction:

Add a small amount of each compound to separate test tubes. To test for carboxylic acid, add a few drops of a basic solution (such as sodium bicarbonate) to each test tube. Effervescence or the formation of bubbles indicates the presence of a carboxylic acid due to the release of carbon dioxide gas. Esters and amines do not show this reaction.

Reaction with Sodium Hydroxide (NaOH):

Add a few drops of sodium hydroxide solution to each compound in separate test tubes. Carboxylic acids will react with sodium hydroxide to form a water-soluble salt, producing effervescence or fizzing due to the release of carbon dioxide gas. Esters and amines do not show this reaction.

Reaction with Acidified Potassium Dichromate (K2Cr2O7):

Mix each compound with a few drops of acidified potassium dichromate solution (containing sulfuric acid). Carboxylic acids will undergo oxidation and change the orange solution of potassium dichromate to a green solution, indicating the formation of chromium(III) ions. Esters and amines do not show this reaction.

Reaction with Nitrous Acid (HNO2):

Treat each compound with nitrous acid, which is generated by adding a mixture of sodium nitrite and hydrochloric acid. Carboxylic acids will react with nitrous acid to form an alcohol and evolve nitrogen gas. This reaction is known as the carboxylic acid decarboxylation reaction. Esters and amines do not show this reaction.

Reaction with Ninhydrin:

Apply a few drops of ninhydrin solution to each compound on a piece of filter paper and heat the paper gently. Amines will react with ninhydrin to produce a colored product, typically purple or blue. Carboxylic acids and esters do not show this reaction.

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Answer:

b

Explanation:

Answer:

yh

Explanation:

welcome.This place is for learning

my favrit word is HI!

The enthalpy change, ΔH of the reaction is -74.1 kJ/mol.

The change in the enthalpy of a chemical reaction that takes place at constant pressure is known as the Heat of Reaction (also known as the Enthalpy of Reaction).

It is a thermodynamic unit of measurement that can be used to determine how much energy is released or created per mole during a reaction.

The enthalpy change, ΔH, of the given reaction is calculated as follows:

ΔH = ΔH₁ + ΔH₂ - ΔH₃

where;

ΔH₁ = -571.6 kJ

ΔH₂ = -393.5 kJ

ΔH₃ = -890.4 kJ

ΔH = -571.6 kJ + ( -393.5 kJ) - (-890.4 kJ)

ΔH = -74.7 kJ

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The mass of gum you need to chew to chew one mole of sugar is approximately 5.68 × 10-22 grams.

To calculate the mass of gum that you need to chew to chew one mole of sugar, you need to use the following steps:

Step 1: Find the molar mass of the sugar

The molar mass of sugar is 342.3 g/mol.

Step 2: Convert molar mass to gramsTo convert the molar mass to grams, you need to divide it by Avogadro's number (6.022 × 1023), which gives you 5.68 × 10-22 grams of sugar.

Step 3: Find the mass of gum needed since it is not provided how much sugar is present in a single piece of gum, we can assume that it is negligible.

Therefore, the mass of gum needed to chew one mole of sugar is approximately 5.68 × 10-22 grams.

Hence, the mass of gum you need to chew to chew one mole of sugar is approximately 5.68 × 10-22 grams.

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6.23L volume of h2 gas is produced at stp.

Given that one mole of dihydrogen (H2) weighs 2,0159 g/mol, the experimental density of hydrogen—which is 0,0899 g/L at 0 °C and 0,0837 g/L at 20 °C—can be used to compute the exact molar volume of hydrogen.

This implies that at STP, one mole of hydrogen also takes up 22.4 liters of space. Therefore, at STP, 10moles of hydrogen gas will take up =22.410=224litres of space. In other words, when 460g of salt combines with extra water at STP, 224litres (or 224000mL) of hydrogen gas are released.

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the question you are looking for is

A 5.00 g sample of Al reacts with excess H2SO4. What volume of H2 gas is produced at STP?

2Al(s) + 3H2SO4(aq)→ Al2(SO4)3(aq) + 3H2 (g)

Answer: A 13.88 mL of the concentrated acid would be required to make 250. mL of a 1.00 M \(H_{2}SO_{4}\) solution.

Explanation:

Given: \(M_{1}\) = 18.0 M,     \(V_{1}\) = ?

\(M_{2}\) = 1.00 M,         \(V_{2}\) = 250 mL

Formula used to calculate the volume of concentrated acid is as follows.

\(M_{1}V_{1} = M_{2}V_{2}\)

Substitute the values into above formula as follows.

\(M_{1}V_{1} = M_{2}V_{2}\\18.0 M \times V_{1} = 1.00 M \times 250 mL\\V_{1} = \frac{1.00 M \times 250 mL}{18.0 M}\\= 13.88 mL\)

Thus, we can conclude that 13.88 mL of the concentrated acid would be required to make 250. mL of a 1.00 M \(H_{2}SO_{4}\) solution.

Answer:

is cool is cool goodcripopo

Answer:

C

Explanation:

Mostly all of them but most likely C

Answer:

A

Explanation:

The more gas magma contains, the more explosive a volcanic eruption will be.

As the PMHNP, you decide to order a lithium level that comes back at 2.3mmol/l. The best line of action to take Examine other hypotheses for the cause of his symptoms and give him loperamide for diarrhoea and ropinirole for the tremors.

What do you mean by lithium level?

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Chemical substances known as oxygenates have oxygen as one of their constituent parts. Tech B is correct

Although technically any substance containing oxygen qualifies as an oxygenate, the term is most frequently used to refer to substances added to internal combustion engine vehicles.

Oxygenate fuel additives are either alcohols, like ethanol, or ethers, with methyl tertiary butyl ether, or MTBE, being the most often used. Any chemical compound that has at least one hydroxyl group, which is made up of oxygen and hydrogen and is connected to the carbon atom in an alkyl group, is referred to as alcohol. Alkyl groups are made up of hydrogen and carbon atom chains.

Alcohols are a crucial group in organic chemistry despite their lack of chemical specificity because of how many different compounds they can originate from and be transformed into.

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Hello!!!

Answer: Therefore elements with high ionization energies have more positive electron affinity whereas alkali metals having the lowest ionization energy do not tend to add electrons.

Explanation:  So energy is to be supplied for the addition of electrons and shows positive electron affinity.

Hope This Helps You Out! So... The Answer Your Looking For Is "True"

The statement is true as  all elements with high ionization energy have more electrons and hence have   high electron affinity​.

It is defined as a substance which cannot be broken down further into any other substance. Each element is made up of its own type of atom. Due to this reason all elements are different from one another.

Elements can be classified as metals and non-metals. Metals are shiny and conduct electricity and are all solids at room temperature except mercury. Non-metals do not conduct electricity and are mostly gases at room temperature except carbon and sulfur.

The number of protons in the nucleus is the defining property of an element and is related to the atomic number.All atoms with same atomic number are atoms of same element.

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76.33 grams of NaCl were collected after experiment 1.306 mol were

produced.

Every material has a molecular weight of 6.023 x 10²³. It may be used to quantify the chemical reaction's byproducts. The symbol mol is used to identify the unit. The molecular formula is written out as follows.

Mass of material / mass of one mole equals the number of moles.

We need to know the molar mass of NaCl in order to compute the number of moles of NaCl created.

The atomic weights of sodium (Na) and chlorine together make up the molar mass of sodium chloride (Cl). Na has an atomic mass of 22.99 g/mol, while Cl has an atomic mass of 35.45 g/mol. As a result, NaCl's molar mass is:

Molar mass of NaCl

= (1 x atomic mass of Na) + (1 x atomic mass of Cl)

= (1 × 35.45 g/mol plus 1 x 22.99 g/mol)

= 58.44 g/mol

The mass of gathered NaCl may now be converted into moles using the molar mass:

Mass of NaCl divided by its molar mass yields moles of NaCl.

moles of NaCl = 76.33 g / 58.44 g/mol

moles of NaCl = 1.306 mol

As a result, the experiment generated 1.306 moles of NaCl.

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Answer:

2Na+I2→2NaI

Explanation:

Therefore, the volume of the balloon when heated to 88°C is 2.432 L.

In the case of a gas, the volume is the amount of space that the gas occupies in a container. The volume of a gas can be affected by changes in pressure and temperature, as described by the ideal gas law. In this case, the volume is often expressed in terms of standard temperature and pressure (STP), which are defined as a temperature of 0°C and a pressure of 1 atmosphere (atm). In chemistry, volume is an important property for understanding the behavior of substances in chemical reactions. The volume of reactants and products can be used to determine the stoichiometry of a reaction, which is the relationship between the amounts of reactants and products in a chemical equation.

Here,

To solve this problem, we can use the ideal gas law, which states that:

PV = nRT

where P is the pressure of the gas, V is its volume, n is the number of moles of gas, R is the universal gas constant, and T is the temperature in Kelvin.

Since the pressure of the gas is assumed to remain constant, we can rearrange the ideal gas law to solve for V:

V1/T1 = V2/T2

where V1 is the initial volume of the balloon, T1 is the initial temperature in Kelvin (24°C = 297 K), V2 is the final volume we want to find, and T2 is the final temperature in Kelvin (88°C = 361 K).

Using this equation, we can plug in the given values and solve for V2:

V1/T1 = V2/T2

2.00 L / 297 K = V2 / 361 K

Multiplying both sides by 361 K, we get:

V2 = 2.00 L x (361 K / 297 K)

V2 = 2.00 L x 1.2162

V2 = 2.432 L

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Answer:

1.37dm³

Explanation:

To solve this problem, let us write the reaction expression:

               2KClO₃  →   2KCl  + 3O₂

Now, mass of KClO₃ is 5g, let us find the number of moles;

  Number of moles  = \(\frac{mass}{molar mass}\)  

  Molar mass of KClO₃  = 39 + 35.5 + 3(16) = 122.5g/mol

 Now;

 Number of moles  = \(\frac{5}{122.5}\)   = 0.04mole

  So;

       2 moles of KClO₃  will produce 3 moles of oxygen gas

       0.04 mole of KClO₃  will produce \(\frac{3 x 0.04} {2}\)   = 0.06moles

At STP;

        1 mole of gas has  a volume of 22.4dm³

       0.06 mole of oxygen gas will have a volume of 22.4 x 0.06 = 1.37dm³

If I accidentally left my working stock in room temperature, there are a few steps that I would take in order to assess the damage and salvage the situation. First, I would check the expiration date of the stock to see if it was still viable before being exposed to room temperature. If it had expired, then there may not be much I could do to save it.

Assuming the stock was still viable, I would then inspect it for any signs of contamination or degradation.

If the stock had become contaminated or had started to degrade, then it would need to be discarded.
If the stock appeared to be still usable, I would then perform a series of tests to determine if it was still functional.

I would conduct a viability assay, such as a colony forming unit (CFU) assay or a growth curve analysis, to determine if the stock was still capable of growing and dividing.

If the stock was still functional, then I would use it for experiments as planned, but with the understanding that it may not perform as well as a freshly prepared batch.
To prevent this situation from happening in the future, I would take steps to label and store my stocks properly and to set reminders for myself to check on their status regularly.

It's always better to be safe than sorry when it comes to important reagents and stocks in the lab.

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On the other end of the swing, the kinetic energy begins to change back into potential energy. The pendulum then comes to a complete stop! At the end of each swing, it comes to a complete stop for a brief moment. When the energy is "at rest," it is once again potential energy.

Answer:

2 hydrogen atoms

Explanation:

because the hydrogen atoms are two

Answer:

the answer is B Astroid Belt