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2 moles of CaSO4 are required to produce 128 g of SO2 in 3CaSO4 + CaS → 4CaO + 4SO2 in this equation.

The term mole is defined as a standard scientific unit for measuring large quantities of very small entities such as atoms, molecules, or other specified particles.

1 mole = 6.023 × 10²³ molecules

The balance equation is as follows:

3CaSO4 + CaS → 4CaO + 4SO2

1 mole = 6.023 × 10²³ molecules

1 mole SO₂ = 6.023 × 10²³ molecules

128 mole = ?

Molar mass of SO₂ = 64 gram

The numbers of moles in 128 gram SO₂ = 1 / 64 ×128

= 2 moles

Thus, 2  moles of CaSO4 are required to produce 128 g of SO2.

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Answer:

One mole of Al weighs 27g.

2.5 moles of Al weigh 67.5g.

The arrow in a chemical reaction can be translated to mean:

- O yields

- O react to form

Therefore, the correct options are "O yields" and "O react to form".

Answer:

The options (A) -The rate law for a given reaction can be determined from a knowledge of the rate-determining step in that reaction's mechanism.  and (C) -The rate laws of bimolecular elementary reactions are second order overall ,is true.

Explanation:

(A) -The rate law can only be calculated from the reaction's slowest or rate-determining phase, according to the first sentence.

(B) -The second statement is not entirely right, since we cannot evaluate an accurate rate law by simply looking at the net equation. It must be decided by experimentation.

(C) -Since there are two reactants, the third statement is correct: most bimolecular reactions are second order overall.

(D)-The fourth argument is incorrect. We must track the rates of and elementary phase that is following the reaction in order to determine the rate.

Therefore , the first and third statement is true.

Answer:

1.61 x 1024 molecules

Explanation:

See image below for step-by-step explanation

Answer:

0.2 mole of H2.

Explanation:

We'll begin by calculating the number of mole in 4.71 g of magnesium (Mg). This can be obtained as follow:

Mass of Mg = 4.71 g

Molar mass of Mg = 24 g/mol

Mole of Mg =?

Mole = mass /Molar mass

Mole of Mg = 4.71 /24

Mole of Mg = 0.2 mole

Next, we shall write the balanced equation for the reaction.

This is illustrated below:

Mg + 2HCl —> MgCl2 + H2

From the balanced equation above,

1 mole of Mg reacted to produce 1 mole of H2.

Finally, we shall determine the number of mole of H2 produced from the reaction. This can be obtained as illustrated below:

From the balanced equation above,

1 mole of Mg reacted to produce 1 mole of H2.

Therefore, 0.2 mole of Mg will also react to produce 0.2 mole of H2.

Thus, 0.2 mole of H2 was obtained from the reaction.

The number of moles of H₂ that can be formed if a 4.71 g sample of Mg reacts with excess HCl is 0.19625 moles

Let's represent the reaction with a chemical equation

Mg + HCl → MgCl₂ + H₂

Mg + 2HCl → MgCl₂ + H₂

HCl is in excess according to the question. This means Mg is the limiting reagent and therefore determine the amount of product.

Therefore,

24 g of Mg gives 2g of  H₂

4.71 g of Mg will give ? H₂

cross multiply

mass of H₂ = 4.71 × 2 / 24

mass of H₂ = 9.42 / 24 = 0.3925 g

moles of H₂ = mass / molar mass

moles of H₂ = 0.3925 / 2

moles of H₂ = 0.19625 moles

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Answer:

5

Explanation:

2P₂O₅=P₄+5O₂

Answer:

The reaction between carbon (C) and water (H2O) forms carbon monoxide (CO) and hydrogen gas (H2). The balanced chemical equation for this reaction is:

C(s) + H2O(g) -> CO(g) + H2(g)

According to this balanced equation, one mole of carbon reacts with one mole of water to produce one mole of carbon monoxide and one mole of hydrogen gas.

First, calculate the number of moles of carbon in 34 grams. The molar mass of carbon is approximately 12.01 grams/mole.

Moles of carbon = 34 grams / 12.01 grams/mole = 2.831 moles

As the stoichiometry of the reaction shows a 1:1 ratio between carbon and hydrogen, the moles of hydrogen produced would also be 2.831 moles.

The molar mass of hydrogen (H2) is approximately 2 grams/mole.

So, the mass of hydrogen produced = 2.831 moles * 2 grams/mole = 5.662 grams

Therefore, if 34 grams of carbon reacts with an unlimited amount of water, approximately 5.66 grams of hydrogen gas would be formed.

Explanation:

Approximations followed for answer.

Answer:

BBBBBBBB ITS B

Explanation:

Answer:

hello your question is incomplete attached below is the complete question

answer : To 2 significant digits = 5500 kg

Explanation:

Given

C(s) + O2 (g)  ----------> CO2  ( g )

mass of CO2 = 8.9 * 10^6 g

number of moles =  8.9 * 10^6 / 12  = 7.416 * 10 ^5  mol

same amount of moles is needed by O2 hence

attached below is the detailed  solution

The option that will have the greatest effect on the ability of soil to hold water is the size of the soil particles (option B).

Soil water holding capacity is the amount of water that a given soil can hold for crop use. It is measured as the total quantity of water that can be absorbed by the soil per gram.

This characteristic is closely connected to the affinity that soil molecules have for water and other solutes in the environment.

The different soil types we have possess different water holding capacities. However, the size of each particle is a major determinant of this characteristics.

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genetics and reproduction is all about dna.

Balancing a chemical equation is the process of ensuring that the number of atoms of each element in the reactants is equal to the number of atoms of that same element in the products.

Balance the chemical eqations given in the problem?

Chemical equations are used to describe the reactants and products in a chemical reaction. These equations are written using chemical formulas and symbols, indicating the types and numbers of atoms or molecules involved in the reaction. However, these equations must be balanced to obey the law of conservation of mass, which states that the total mass of the reactants must equal the total mass.

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Answer:457

Explanation:

Answer: An object can change velocity in a number of ways: it can slow down, it can speed up, or it can change direction. A change in speed, or a change in direction, or a change in both speed and direction means that the object has a change in velocity.

Explanation:

Answer:

increasing the positive charge of the positively charged object and increasing the negative charge of the negatively charged object would make the oppositely charged objects attract each other more.

Answer:

hope this helps

Explanation:

see pictures try to put them in order

Answer: b) calcium sulfide

Explanation:

Answer:

the relationship between the relative quantities of substances taking part in a reaction or forming a compound, typically a ratio of whole integers.

Explanation:

G o o g l e

Explanation:

Stoichiometry is the calculation of reactants and products in chemical reactions in chemistry.

The highest electric force exerted by charges -4 ×10⁻⁵ C and 3 ×10⁻⁵ C  placed 0.5 m apart is equal to 43.15 N.

The lowest electric force exerted by charges 3 ×10⁻⁵ C and 3 ×10⁻⁵ C  placed 1 m apart is equal to 8.10 N.

According to Coulomb’s law, the force of attraction between two charges is equal to the product of their charges and is inversely proportional to the square of the distance. This electric force applies along the line joining the two charges.

The magnitude of the electric force can be written as follows:

\(\displaystyle F = k\frac{q_1q_2}{r^2}\)

where k is constant proportionality = 8.99 × 10⁹ N.m²/C².

Given the charge on one point charge, q₁ =  4 ×10⁻⁵ C

The charge on the other point charge, q₂ = - 3 × 10⁻⁵C

The distance between these two charges, r = 0.5 m

The magnitude of electric force between the charges  will be:

\(\displaystyle F = 8.99\times 10^{9}\times \frac{4\times 10^{-5}\times 3\times 10^{-5}}{(0.5)^2}\)

F = 43.15 N

Given the charge on one point charge, q₁ =  3 ×10⁻⁵ C

The charge on the other point charge, q₂ = 3 × 10⁻⁵C

The distance between these two charges, r = 1 m

The magnitude of force between the charges will be:

\(\displaystyle F = 8.99\times 10^{9}\times \frac{3\times 10^{-5}\times 3\times 10^{-5}}{(1)^2}\)

F = 8.1 N

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Answer:

The problem provides you with the solubility of potassium chloride,

KCl

, in water at

20

∘

C

, which is said to be equal to

34 g / 100 g H

2

O

.

This means that at

20

∘

C

, a saturated solution of potassium chloride will contain

34 g

of dissolved salt for every

100 g

of water.

As you know, a saturated solution is a solution that holds the maximum amount of dissolved salt. Adding more solid to a saturated solution will cause the solid to remain undissolved.

In your case, you can create a saturated solution of potassium chloride by dissolving

34 g

of salt in

100 g

of water at

20

∘

C

.

Now, your goal here is to figure out how much potassium chloride can be dissolved in

300 g

of water at this temperature. To do that, use the given solubility as a conversion factor to take you from grams of salt to grams of water

Some types of solids that are insoluble in water are:

Many solids are insoluble in water, meaning they do not dissolve in water to a significant extent. Here are some examples of common solids that are generally insoluble in water:

Metals: Most metals, such as gold, silver, platinum, and copper, are insoluble in water.

Non-Metallic Elements: Many non-metallic elements, such as carbon (in the form of graphite or diamond), sulfur, phosphorus, and iodine, are insoluble in water.

Metal Oxides: Some metal oxides, particularly those of less reactive metals, are insoluble in water. Examples include aluminum oxide (Al2O3), iron(III) oxide (Fe2O3), and lead(II) oxide (PbO).

Metal Carbonates: Most metal carbonates are insoluble in water. Examples include calcium carbonate (CaCO3), lead(II) carbonate (PbCO3), and copper(II) carbonate (CuCO3).

Metal Sulfides: Many metal sulfides are insoluble in water. Examples include lead(II) sulfide (PbS), silver sulfide (Ag2S), and mercury(II) sulfide (HgS).

Insoluble Salts: Certain salts have limited solubility in water. Examples include silver chloride (AgCl), lead(II) iodide (PbI2), and calcium sulfate (CaSO4).

It's important to note that while these solids are generally insoluble in water, they may exhibit some solubility to a small extent. The solubility of a solid in water can vary depending on factors such as temperature, pressure, and the presence of other solutes.

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A pure substance is indeed a single kind of matter with a uniform and definite composition. In contrast, a mixture is made up of two or more substances that are together in the same place, but each substance maintains its own properties.

Mixtures can be classified as either homogeneous or heterogeneous. A homogeneous mixture has a uniform composition throughout, meaning its components are evenly distributed and not easily distinguishable. Examples include solutions, such as saltwater or air.

On the other hand, a heterogeneous mixture has an uneven distribution of its components, and its individual substances can be easily identified. Examples include sand and water, or oil and water.

One key distinction between a pure substance and a mixture is that a pure substance has a fixed composition, while the composition of a mixture can vary. This means that mixtures can be separated into their individual components through physical processes like filtration, evaporation, or distillation, without undergoing any chemical changes.

In summary, a pure substance is a single type of matter with a definite and uniform composition, while a mixture consists of two or more substances that are combined in the same place, but each substance retains its individual properties. Mixtures can be homogeneous or heterogeneous and can be separated into their components through physical methods.

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The amount of heat required to raise the temperature of the 34.2 g sample of aluminum by 34 oC is 1043.52 J.

What is Temperature?

Temperature is a measure of the average kinetic energy of the particles in a substance. It is a physical property that determines the direction of heat flow between two objects or systems in contact with each other. Temperature is measured in degrees Celsius (°C) or Fahrenheit (°F), or in kelvin (K) in the International System of Units (SI).

The amount of heat (q) required to raise the temperature of a substance can be calculated using the formula:

q = m x c x ΔT

Where:

m = mass of the substance (in grams)

c = specific heat of the substance (in J/g oC)

ΔT = change in temperature (in oC)

Plugging in the values given:

m = 34.2 g

c = 0.9 J/g oC

ΔT = 34 oC

q = (34.2 g) x (0.9 J/g oC) x (34 oC)

q = 1043.52 J

Therefore, the amount of heat required to raise the temperature of the 34.2 g sample of aluminum by 34 oC is 1043.52 J.

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The final concentration of the reactant of a first order reaction can be determined from the rate constant equation. The concentration of ammonium carbonate after 39 s will be 0.003 M.

Rate constant of a reaction is the rate of reaction when one molar concentration of the reactant is involved in the reaction. The expression for the rate constant k for first order reaction is :

k = 1/t ln (C0/Ct)

Where C0 be the initial concentration and Ct be the concentration after t seconds.

Given that C0 of ammonium nitrate = 0.957 M

rate constant = 0.196 /s

t = 39 s.

The concentration after 39 seconds is calculated as follows:

0.196 /s = 1/39s ln (0.957 M / Ct)

Ct = 0.957 / (ln⁻¹ (0.196 × 39))

    = 0.003 M.

Therefore, the concentration of ammonium carbonate after 39 seconds will be 0.003 M.

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