What is the function of sulphur (IV) oxide in the reaction represented by the following equation? SO 2(aq) + 2H2S(g) -> 35 (s) + 2H 20 (l)

A. Dehydrating agent
B. Oxidising agent
C. Bleaching agent
D. Acid
E. Precipitant ​

Answer:

252.06492

Explanation:

How many grams (NH4)2Cr2O7 in 1 mol? The answer is 252.06492.

We assume you are converting between grams (NH4)2Cr2O7 and mole.

You can view more details on each measurement unit:

molecular weight of (NH4)2Cr2O7 or mol

The SI base unit for amount of substance is the mole.

1 grams (NH4)2Cr2O7 is equal to 0.0039672319337415 mole.

Note that rounding errors may occur, so always check the results.

Use this page to learn how to convert between grams (NH4)2Cr2O7 and mole.

Type in your own numbers in the form to convert the units!

Answer:

1562 g

Explanation:

Step 1: Given data

Number of atoms of copper: 1.480 × 10²⁵ atoms

Step 2: Calculate the moles corresponding to 1.480 × 10²⁵ atoms of copper

We will use the Avogadro's number: there are 6.022 × 10²³ atoms of Cu in 1 mole of atoms of Cu.

1.480 × 10²⁵ atom × (1 mol/6.022 × 10²³ atom) = 24.58 mol

Step 3: Calculate the mass corresponding to 24.58 moles of copper

The molar mass of Cu is 63.55 g/mol.

24.58 mol × 63.55 g/mol = 1562 g (with 4 significant figures)

true gase doesn't have no definite volume

Answer: Particles move independently of one another and are widely spaced.

Explanation:

The postulates of kinetic theory are:

1)All the molecules are made up of molecules which are rigid spheres

2) The molecules are identical for a particular gas and different for different gases.

3) All the molecules move in random motion in all direction.

4) During random motion they collide with each other as and hence exert pressure

5) During collision the molecules move in a straight line path known as free path

6) The size of the molecule of a gas is negligible as compare to the distance between the molecule.

Answer:

A

Explanation:

Right on edge

The balanced chemical equation for the decomposition of aspirin (acetylsalicylic acid) is:

\(2C_{9}H_{8}O_{4} (aspirin) → 2C_{7}H_{6}O_{3} (salicylic acid) + 2CO_{2} (Carbon dioxide) + H_{2}O (water)\)

In this reaction, the aspirin molecule breaks down into salicylic acid, carbon dioxide, and water. The reaction is typically catalyzed by heat or exposure to acidic or basic conditions.

Aspirin, or acetylsalicylic acid, contains ester functional groups that can undergo hydrolysis. Under suitable conditions, the ester bond in aspirin is cleaved, leading to the formation of salicylic acid, which is the primary decomposition product. Additionally, carbon dioxide and water are released as byproducts of the reaction.

The balanced equation shows that for every two molecules of aspirin, two molecules of salicylic acid, two molecules of carbon dioxide, and one molecule of water are formed. Understanding the decomposition of aspirin is important in pharmaceutical and chemical industries to ensure the stability and shelf-life of the compound, as well as to study its breakdown products and potential side reactions.

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Answer:

Substance C

Explanation:

Substance C would be the answer because Substance C has a lower attraction level. Because of this, it takes more energy to take out of in order to become a liquid.

Both the gas and the liquid will adapt their shape to that of their respective containers.

The gas will adjust its volume to fit inside the container. Solids are basically denser than liquids, which are again denser than gases. There is not much space between the particles in the solid, which are touching to each other.

The particles' energy content and interactions with other particles have an impact on how much they move around. The kinetic energy of the particles increases with the rate of vibration and particle movement. Solids basically have the lowest kinetic energy because they vibrate in place and are also closely packed.

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0.04 grams of zinc reacted

The Ideal gas law is the equation of state of a hypothetical ideal gas. It is a good approximation to the behaviour of many gases under many conditions, although it has several limitations. The ideal gas equation can be written as

                            PV = nRT

where,

P = Pressure

V = Volume

T = Temperature

n = number of moles

Given,

Volume = 670 ml = 0.67L

Pressure = 576 torr

Temperature = 25 degree celsius

PV = nRT

576 × 0.67 = n × 62.36 × 298

n = 0.02 moles

mass = moles × molar mass

= 0.02 × 2 = 0.04g

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Answer:

2.0 moles

Explanation:

I hope this helps you a little bit at least the answer is 2.0 but if you want to review more stuff check the photos

Approximately 70.57 mL of 1.00 M NaOH should be added to 250 mL of 0.50 M CH3CO₂H to produce a buffer with a pH of 4.50.

To determine the volume of 1.00 M NaOH required to produce a buffer with a pH of 4.50 when added to 250 mL of 0.50 M CH3CO₂H, we need to consider the Henderson-Hasselbalch equation and the stoichiometry of the reaction.

The Henderson-Hasselbalch equation for a buffer solution is given as:

pH = pKa + log([A-]/[HA])

In this case, CH3CO₂H (acetic acid) acts as the weak acid (HA) and CH3COO- (acetate ion) acts as its conjugate base (A-). We are given that the desired pH is 4.50, and we can determine the pKa value for acetic acid from reference sources, which is approximately 4.75.

Using the Henderson-Hasselbalch equation, we can rearrange it to solve for the ratio [A-]/[HA]:

[A-]/[HA] = 10^(pH - pKa)

[A-]/[HA] = 10^(4.50 - 4.75) = 10^(-0.25) = 0.5623

This means that the ratio of the acetate ion to acetic acid in the buffer solution should be approximately 0.5623.

To calculate the required volume of NaOH, we need to consider the stoichiometry of the reaction. Acetic acid reacts with hydroxide ions (OH-) to form acetate ions and water:

CH3CO₂H + OH- → CH3COO- + H2O

The stoichiometric ratio between acetic acid and hydroxide ions is 1:1. Therefore, the volume of 1.00 M NaOH needed can be calculated using the equation:

Volume (NaOH) × 1.00 M = Volume (CH3CO₂H) × 0.50 M × 0.5623

Volume (NaOH) = (Volume (CH3CO₂H) × 0.50 M × 0.5623) / 1.00 M

Volume (NaOH) = (250 mL × 0.50 M × 0.5623) / 1.00 M

Volume (NaOH) ≈ 70.57 mL

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When acetylene gas reacts with the 1.5 moles of oxygen gas, it produces 1.2 moles of carbon dioxide gas and the water vapor.

Let's  us consider the reaction for the complete combustion of acetylene.

C₂H₂(g) + 2.5 O₂(g) ⇒ 2 CO₂(g) + H₂O(l)

According to balanced equation, the molar ratio of  the O₂ to CO₂ is 2.5:2. The moles of  the carbon dioxide produced by the reaction of 1.5 mol of the  oxygen are:

When the acetylene gas reacts with 1.5 moles of oxygen gas, it produces 1.2 moles of carbon dioxide gas and the water vapor. It is a kind of combustion reaction where a hydrocarbon reacts with oxygen to form carbon dioxide and water vapors.

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Copper metal plus zinc sulfate solution : is not  possible because the copper metal is less reactive than zinc and copper cannot displace the zinc.

The copper metal with zinc sulfate reaction is not possible because copper is less reactive than the zinc cant cannot displace the zinc. so, the reaction :

Cu + ZnSO₄ ---->    no reaction

but the zinc plus copper sulfate is possible , copper is less reactive than zinc and zinc can displace the copper . and the reaction is called as displacement reaction the reacion is given as :

CuSO₄   +   Zn   ----->    ZnSO₄    +   Cu

Thus, Copper metal plus zinc sulfate solution : is not  possible because the copper metal is less reactive than zinc and copper cannot displace the zinc.

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Both I and II are true statements. The melting point of a solid is the temperature at which solid changes from a solid to a liquid.

Molecular solids are composed of molecules held together by weak intermolecular forces, such as dipole-dipole interactions, hydrogen bonds, and London forces.

These types of bonds are weaker than the ionic bonds that are present in ionic solids, which is why molecular solids have lower melting points than ionic solids.

In addition, the shape of the molecule will influence its melting point or boiling point. For example, molecules with a higher surface area will have a higher boiling point than molecules with a lower surface area.

This is due to the increased surface area leading to increased intermolecular forces and a higher boiling point.

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Both I and II are true statements. The melting point of a solid is the temperature at which solid changes from a solid to a liquid.

Molecular solids are composed of molecules held together by weak intermolecular forces, such as dipole-dipole interactions, hydrogen bonds, and London forces.

These types of bonds are weaker than the ionic bonds that are present in ionic solids, which is why molecular solids have lower melting points than ionic solids.

In addition, the shape of the molecule will influence its melting point or boiling point. For example, molecules with a higher surface area will have a higher boiling point than molecules with a lower surface area.

This is due to the increased surface area leading to increased intermolecular forces and a higher boiling point.

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Answer:

6059.63 kcal/kg.

Explanation:

CH4 consist of Hydrogen and carbon. Therefore, Hydrogen in CH4 = 12 × 4 = 48 kg,  carbon in CH4 = 12 × 12 = 144kg.

For ethane, the amount of hydrogen present = 2 × 6 = 12kg and that of carbon in ethane = 2 × 24 = 48kg.

The weight of carbon in CO = 15 × 12 = 18kg and the weight of Hydrogen in CO = 15 × 16 = 240kg.

For hydrogen, its weight in H2 = 50 × 2 = 100kg.

For CO2, carbon has = 4 × 12 = 48 kg and oxygen has = 4 × 32 = 128kg.

For C6H6, carbon has 2 × 72 = 144kg and hydrogen has 2 × 6 = 12kg.

For N2, the amount of nitrogen= 11 × 28 = 308 kg.

For CH2= CH2, carbon has 4 × 24 = 96kg and hydrogen = 4 × 4 = 16kg.

The gross calofiric value = 1/100 [ 8080 C + 34500 + ( H - O/8) + 22405].

Where the total weight = 128 + 180+ 48 + 240 + 100 + 144 + 48 + 12 + 48 + 16 + 96 + 308 + 12 + 144 = 1524 kg.

The percentage by weight of carbon = total weight of carbon/total weight × 100.

The total Weight of carbon= 48 + 180 + 144 + 48 +144 + 96 = 660kg.

The percentage weight of carbon = 660/1524 × 100 = 43.3 %.

The percentage weight of hydrogen = total weight of hydrogen/total weight × 100.

The total weight of hydrogen = 100 + 12 + 48 + 16 +12 = 188.

The percentage weight of Hydrogen = 188/ 1524 × 100 = 12.33%.

Percentage weight of oxygen = total weight of oxygen/total weight × 100.

Percentage weight of oxygen = ( 128 + 240) / 1524 × 100 = 24.15%.

The gross calorific value = 1/100 [ 8080 × 43.3 ,+ 34500 ( 13.33 - 24.15/8) ] = 6711.02 kcal/kg.

Net calorific value = 6711.02 - 0.09 × 12.3 × 587 = 6059.63kcal/kg.

The amount, in kJ, of heat needed to completely vaporize 50.0g of water at 100°C is 118.8 kJ.

The heat needed to completely vaporize 50.0g of water at 100°C can be calculated using the following formula:

q = m x Hv

where:

First, we need to convert 50.0g to moles by dividing by the molar mass of water which is approximately 18.015 g/mol3:

moles of water = 50.0 g / 18.015 g/mol moles of water = 2.776 mol

Thus:

q = (2.776 mol) x (40.65 kJ/mol) q = 112.8 kJ

In other words, 112.8 kJ of heat is needed to completely vaporize 50.0g of water at 100°C.

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Explanation:

1a) CaCO₃(s) → Ca²⁺(aq) + CO₃²⁻(aq)

1b) Remember, solids are not included in the equilibrium equation.

K = [Ca²⁺] [CO₃²⁻]

1c) Adding CO₃²⁻ ions will shift the reaction to the left, producing CaCO₃(s) until equilibrium is restored.

2) 2 SO₂(g) + O₂(g) → 2 SO₃(g)

Kc = 2.5×10¹⁰ = [SO₃]² / ([SO₂]² [O₂])

2a) SO₂(g) + ½ O₂(g) → SO₃(g)

Kc = [SO₃] / ([SO₂] [O₂]^½)

Kc² = [SO₃]² / ([SO₂]² [O₂])

Kc² = 2.5×10¹⁰

Kc ≈ 1.58×10⁵

2b) SO₃(g) → SO₂(g) + ½ O₂(g)

Kc = [SO₂] [O₂]^½ / [SO₃]

Kc = 1 / (1.58×10⁵)

Kc ≈ 6.33×10⁻⁶

2c) 3 SO₂(g) + ³/₂ O₂(g) → 3 SO₃(g)

Kc = [SO₃]³ / ([SO₂]³ [O₂]^³/₂)

Kc = ([SO₃] / ([SO₂] [O₂]^½))³

Kc = (1.58×10⁵)³

Kc ≈ 3.95×10¹⁵

3) H₂(g) + I₂(g) → 2 HI(g)

K = [HI]² / ([H₂] [I₂])

Make an ICE table.

\(\left[\begin{array}{cccc}&Initial&Change&Equilibrium\\H_{2}&0.400&-0.240&0.160\\I_{2}&1.60&-0.240&1.360\\HI&0&+0.480&0.480\end{array}\right]\)

K = (0.480)² / (0.160 × 1.360)

K = 1.06

Answer:

The energies of  combustion (per gram) for hydrogen and methane are as follows: Methane = 82.5 kJ/g;  Hydrogen = 162 kJ/g

Note: The question is incomplete. The complete question is given below:

To compare the energies of combustion of these fuels, the  following experiment was carried out using a bomb  calorimeter with a heat capacity of 11.3 kJ/℃.  When a 1.00-g sample of methane gas burned with

excess oxygen in the calorimeter, the temperature  increased by 7.3℃. When a 1.00 g sample of  hydrogen gas was burned with excess oxygen, the temperature increase was 14.3°C. Compare the energies of  combustion (per gram) for hydrogen and methane.

Explanation:

From the equation of the first law of thermodynamics, ΔU = Q + W

Since there is no expansion work in the bomb calorimeter,  ΔU = Q

But Q = CΔT

where C is heat capacity of the bomb calorimeter =  11.3
kJ/ºC; ΔT = temperature change

For combustion of methane gas:

Q per gram = (
11.3
kJ/ºC * 7.3°C)/1.0g

Q = 83 kJ/g

For combustion of hydrogen gas:

Q per gram = (
11.3
kJ/ºC * 14.3°C)/1.0g

Q = 162 kJ/g

Answer:

Gamma emission is a type of radioactive decay, but it is not a fission reaction.

Explanation:

BOOM

Yes. The model represents atoms rearranging to produce a new compound.

They are reactions involving the breakage of bonds and rearrangement of atoms in reactants to form products.

In the model, the bonds between hydrogen and chlorine were broken. Thereafter, each hydrogen and chlorine molecule linked up to form hydrogen chloride.

Thus, the model shows atoms rearranging to produce a new compound.

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There are 576 different ways to choose a meal.

Promotional offers. A promotional offer is a specific proposition to clients that specifies a reward and patron behavioral standards for earning a reward. the recognition and trouble of the praise are captured thru a retail transaction, purchaser order, rebate claim, rebate redemption, or different patron interplay. a discount is a difference between the unique charge and the lower charge it's far being bought at. a proposal is a deal wherein a product is normally bought at a reduction.

Calculation:-

There are 8 appetizers, 12 entrees, and 6 desserts.

Number of choices =  8 × 12 × 6

                                =  576

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There are several mechanisms that can be involved in the synthesis or reactions of alcohols and ethers, depending on the specific reaction and the type of alcohol or ether involved. Here are some common mechanisms that may be involved:

a. Nucleophilic substitution: This mechanism is often involved in the synthesis of ethers from alkyl halides or sulfonates. In this mechanism, a nucleophile attacks the electrophilic carbon of the alkyl halide or sulfonate, displacing the leaving group and forming a new carbon-oxygen bond. In the case of the Williamson ether synthesis, an alkoxide ion acts as the nucleophile and attacks the alkyl halide.

b. Dehydration: In the presence of acid catalysts, alcohols can undergo dehydration to form ethers. This mechanism involves the loss of a water molecule from two alcohol molecules and the formation of an ether linkage.

c. Acid-catalyzed cleavage: Ethers can be cleaved into two alcohol molecules using acid catalysts. This mechanism involves the protonation of the oxygen atom, followed by nucleophilic attack of water or alcohol.

d. Nucleophilic addition: Ethers can undergo nucleophilic addition reactions with strong acids such as HBr or HI to form alkyl halides and alcohols. This mechanism involves the protonation of the oxygen atom, followed by nucleophilic attack of the halide ion.

e. Oxidation: Primary alcohols can be oxidized to form ethers using oxidizing agents such as HIO4. This mechanism involves the oxidation of the alcohol to an aldehyde, which then reacts with another alcohol molecule to form the ether.

f. Acid-catalyzed transetherification: Ethers can react with alcohols in the presence of acid catalysts to form different ethers. This mechanism involves the protonation of one of the oxygen atoms, followed by nucleophilic attack of the alcohol on the other oxygen atom, leading to the formation of a new ether.

g. Acid-catalyzed dehydration of secondary alcohols: Secondary alcohols can undergo acid-catalyzed dehydration to form alkenes and ethers. This mechanism involves the loss of a water molecule from the alcohol, which can lead to the formation of an alkene or an ether depending on the reaction conditions.

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Answer:

i. 3 moles.

ii. 132.03 grams.

iii. 105.6 grams.

Explanation:

Hello!

In this case, given the balanced chemical reaction, we can proceed as follows:

i. By starting with 5 moles of oxygen, via the 5:3 mole ratio we compute the produced moles of CO2:

\(n_{CO_2}=5molO_2*\frac{3molCO_2}{5molO_2} =3molCO_2\)

ii. Now, since we have previously computed the moles of CO2 from the same moles of oxygen, by using its molar mass (44.02 g/mol), we obtain:

\(m_{CO_2}=3molCO_2*\frac{44.01gCO_2}{1molCO_2} =132.03gCO_2\)

iii. Now, we need to combine the previously used two proportional factors for the calculation of the mass of CO2 from 128.00 grams of oxygen (molar mass 32.00 g/mol):

\(m_{CO_2}=128.00gO_2*\frac{1molO_2}{32.00gCO_2}*\frac{3molCO_2}{5molO_2}*\frac{44.01gCO_2}{1molCO_2}\\\\m_{CO_2}=105.6gCO_2\)

Best regards!

Answer:

6598 mL = 6598 cm^3

Explanation:

Cubic centimeters (cc) and milliliters (mL) are both units of volume measurement. They are equivalent, meaning that 1 mL is equal to 1 cm^3. To convert from mL to cm^3, we simply multiply the volume in mL by 1.

To convert 6598 mL to cubic centimeters, we can use this conversion factor:

1 mL = 1 cm^3

Therefore, we can multiply 6598 mL by 1 to get the equivalent volume in cubic centimeters.

6598 mL x 1 cm^3/mL = 6598 cm^3

So, 6598 mL is equal to 6598 cm^3.

The partial atmospheric pressure (atm) of hydrogen in the mixture is 0.59 atm.

Partial pressure of particular gas will be calculated as:

p = nP, where

Moles will be calculated as:

Moles of Hydrogen gas = 2.02g / 2.014g/mol = 1 mole

Moles of Chlorine gas = 35.90g / 70.9g/mol = 0.5 mole

Mole fraction of hydrogen = 1 / (1+0.5) = 0.6

Partial pressure of hydrogen = (0.6)(748) = 448.8 mmHg = 0.59 atm

Hence, required partial atmospheric pressure of hydrogen is 0.59 atm.

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Answer:

A possible element with ns2np4 valence orbital is Oxygen(O)
A element that has the most electronegativity and soft is flourine(F)
for part C, it is scandium (Sc) with the last electron filled in the 3d orbital

According to the placement of elements in the periodic table and the atomic structure, protons from atom on right will attract electrons from atom on left.

Periodic table is a tabular arrangement of elements in the form of a table. In the periodic table, elements are arranged according to the modern periodic law which states that the properties of elements are a periodic function of their atomic numbers.

It is called as periodic because properties repeat after regular intervals of atomic numbers . It is a tabular arrangement consisting of seven horizontal rows called periods and eighteen vertical columns called groups.

Elements present in the same group have same number of valence electrons and hence have similar properties while elements present in the same period show gradual variation in properties due to addition of one electron for each successive element in a period.

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The atomic mass of sulfur trioxide (SO3) is 82 amu.

Sulfur trioxide (SO3) has one sulfur atom and three oxygen atoms.

The atomic mass of sulfur can be calculated by subtracting the total mass of the oxygen atoms in sulfuric acid (3 x 16 amu) from the mass of sulfuric acid (98 amu) and then subtracting the mass of the remaining oxygen atom:

The atomic mass of sulfur is 34 amu.

To find the atomic mass of sulfur trioxide, we add the atomic masses of one sulfur atom and three oxygen atoms:

Therefore, the atomic mass of sulfur trioxide (SO3) is 82 amu.

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the pressure required for 1.35 g of oxygen to dissolve in 1.5 L of water is 3.56 atm.

The first step in solving this problem is to identify the relevant equation.

Henry's law is the formula that relates the pressure of a gas above a liquid to the concentration of the gas that dissolves in the liquid.

In mathematical terms, Henry's law can be expressed as follows:P = kH * Cwhere P is the pressure of the gas, kH is Henry's law constant, and C is the concentration of the gas in the liquid.

To solve the problem, we need to first determine the value of kH using the given data.

kH can be calculated using the following formula:kH = P / CSubstituting the values given in the problem into this formula, we get:kH = 1.65 atm / (0.654 g / 1.5 L) = 3.97 atm/(g/L).

Now that we have the value of kH, we can use Henry's law to calculate the pressure required for 1.35 g of oxygen to dissolve in 1.5 L of water.

To do this, we simply rearrange the formula to solve for P:P = kH * CSubstituting the values of kH and C into this formula, we get:P = 3.97 atm/(g/L) * (1.35 g / 1.5 L) = 3.56 atm

Therefore, the pressure required for 1.35 g of oxygen to dissolve in 1.5 L of water is 3.56 atm.

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Answer:

number 7 is GROWTH

number 8 is TARGET CELLS

number 9 is pituitary gland