What is the volume of 12.8 g of a liquid that has a density of 0.789 g/mL?

the number of protons and neutrons in an atom

Answer:

physcial chemist

Explanation:

k12 user. for all of those who understand nothing about this quiz.

First convert mass to number of moles. Molar mass of H2C2O2 • 2H2O = 94 / mol

1.89g / (94 g / mol) = .02 mol H2C2O2 • 2H2O

Then we divide by 0.1 L, or 100 mL, and we get a concentration of 0.2 M.

Since there are two positive ions (2 H+), therefore normality is:

0.4 N

Answer: was rejected by religious society and the church

Explanation:

At first, heliocentric theory was rejected by the Church and the religious public. Despite large amounts of evidence supporting the theory, the Catholic church prohibited scientists from teaching it as anything more than a hypothesis

Final answer:

When 2.00 moles of methane (CH₄) reacts with chlorine (Cl₂), according to the balanced chemical equation, the total amount of hydrogen chloride (HCl) produced is 8 moles.

Explanation:

The student is inquiring about the reaction between methane (CH₄) and chlorine (Cl₂) to produce carbon tetrachloride (CCl₄) and hydrogen chloride (HCl). We are given that 2.00 moles of methane react and asked to calculate the total amount of HCl produced, assuming that chlorine and hydrogen fluoride are present in excess.

First, we need to balance the chemical equation to understand the stoichiometry of the reaction:

CH₄ + 4 Cl₂ → CCl₄ + 4 HCl

From the balanced equation, we see that 1 mole of CH₄ reacts with 4 moles of Cl₂ and produces 4 moles of HCl. Therefore, if 2.00 moles of CH₄ reacts, it will produce:

mol HCl produced = 2 mol CH₄ × (4 mol HCl / 1 mol CH₄) = 8 moles of HCl

The 5p subshell of an atom can contain electrons with six different sets of quantum numbers, corresponding to pairs of electrons in each of the subshell's three p orbitals. These sets of quantum numbers are: {5,1,-1,-1/2}, {5,1,-1,+1/2}, {5,1,0,-1/2}, {5,1,0,+1/2}, {5,1,1,-1/2}, {5,1,1,+1/2}.

The 5p subshell of an atom can have electrons with a range of possible quantum numbers. A quantum number is a value assigned to describe the state of an electron in an atom. The 5p subshell has 3 orbitals, so it can contain up to 6 electrons.

When it comes to identifying the quantum number sets, the principal quantum number (n) will always be 5, representing the energy level. The azimuthal quantum number (l), which indicates the shape of the orbital, will be 1, representing a p-subshell. The magnetic quantum number (ml) can be -1, 0, 1, as there are 3 orbitals in a p-subshell. Finally, the spin quantum number (ms) can be -1/2 or +1/2, which indicates the spin orientation of an electron.

Therefore, all possible sets of quantum numbers for the electrons located in the orbitals of the 5p subshell are: {5,1,-1,-1/2}, {5,1,-1,+1/2}, {5,1,0,-1/2}, {5,1,0,+1/2}, {5,1,1,-1/2}, {5,1,1,+1/2}.

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A pure substance is a sample of matter with a constant composition and with all specimens possessing the exact same properties. Pure substances can either be elements, with only one type of atom, or compounds, composed of two or more types of atoms.

A sample of matter is considered a pure substance when it has a constant composition and all specimens have exactly the same properties. Pure substances can be classified into two categories: elements and compounds. Elements are pure substances that consist of only one type of atom and cannot be broken down by a chemical change while compounds are pure substances that consist of two or more types of atoms. For instance, any sample of sucrose (table sugar) is a pure substance consisting of 42.1% carbon, 6.5% hydrogen, and 51.4% oxygen by mass, having the same physical properties like melting point, color, and sweetness, irrespective of its source.

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Final answer:

For a quality control experiment with two parts, where each part can be acceptable, repairable, or scrapped, there are a total of 9 possible combinations of outcomes by multiplying the 3 outcomes of the first part with the 3 outcomes of the second part.

Explanation:

The question involves determining the number of possible outcomes for a quality control experiment with two parts. Each part can result in one of three outcomes: acceptable, repairable, or scrapped. Since there are three possible outcomes for the first part and the same three possible outcomes for the second part, we use the counting principle to find the total number of outcomes for the two parts.

To calculate this, we multiply the number of outcomes for the first part (3) by the number of outcomes for the second part (3), which gives us:

3 outcomes for the first part * 3 outcomes for the second part = 9 total possible outcomes.

The experiment regarding two parts can therefore have 9 different combinations of outcomes.

Final answer:

Unboiled water can be used to prepare an acetic acid solution because acetic acid is a weak acid and its equilibrium is not greatly affected by minor impurities. However, for a NaOH solution, unboiled water could introduce carbonate ions that react with and consume hydroxide ions, altering the solution's concentration and pH, making boiled water necessary.

Explanation:

The question concerns the preparation of solutions utilizing unboiled water, specifically in the context of acetic acid (CH₃COOH) and sodium hydroxide (NaOH) solutions. The reason unboiled water can be used for preparing an acetic acid solution but not for a NaOH solution stems from the nature of acetic acid as a weak acid and NaOH as a strong base.

Acetic acid is a weak acid, which means it only partially dissociates in water. Therefore, the presence of impurities or carbon dioxide (CO₂) from unboiled water doesn't significantly alter the proportion of acetic acid molecules that ionize. This results in a relatively stable solution where the equilibrium is not drastically affected by minor impurities.

In contrast, NaOH is a strong base that fully dissociates in water. Thus, using unboiled water, which may contain dissolved carbon dioxide, could lead to the formation of carbonate or bicarbonate ions. These ions could react with and consume hydroxide ions (OH-), affecting the accuracy of the solution's concentration. Hence, the preparation of a NaOH solution requires boiled water to remove dissolved CO₂, ensuring the reliability of the solution's concentration and pH level.

Answer:

Independent: exercise.

Dependent: concentration.

Explanation:

Hello,

In this case, as the statement says that the experiments is towards the effects of the exercise on concentration it is clear that the independent variable is the exercise as the concentration depends on the performed exercise. Therefore, the dependent variable is the concentration as it changes as a function of the specified exercise.

Best regards.

The mass of a liquid density of 3.2 g/ml and a volume of 25 ml will be 80gm.

The density of a material is the measure of how tightly it is packed together. It is expressed as mass per unit volume. Density Symbol: D.

Density Formula:

d = m/V

Where d is the density, m is the object's mass, and V is the object's volume.

Three of an object's most fundamental properties are mass, volume, and density.

Mass describes how heavy something is, volume describes its size, and density is defined as mass divided by volume.

Although mass and volume are everyday concepts, the concept of density is less obvious and requires careful consideration.

Here it is given that

Density = 3.2g/ml.

Volume = 25 ml.

Mass = ?

Density = mass/volume.

Mass = density x volume.

Mass = 3.2 x 25.

Mass = 80gm.

Thus, the mass of the substance is 80gm.

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Answer : Option A) independent variable.

Explanation : The dark closet (N) was a part of independent variable as it's variable does not depends on any other variable.

Also, growth factor which was the major aim of study was the dependent variable as it was dependent on closet where it was placed.

Constant was the water as the quantity of water was same for both the plants.

Control was the plant that was used for this experiment, as this was the standard that was used for the comparison of the growth.

Elements in the periodic table with similar properties are found within the same group or vertical column, based on the periodic law which links properties to atomic numbers. Examples include alkali metals and halogens.

In the periodic table, elements that typically have similar properties are grouped together in the same column or group. This is based on the periodic law, which states that the properties of the elements are periodic functions of their atomic numbers. For example, elements in the same vertical group have similar chemical behavior because they have the same number and distribution of electrons in their valence shells. This can be observed as you move down a group, with variations in characteristics such as atomic size, ionization energy, and electron affinity.

An example of this is the alkali metals in group 1, which all exhibit similar chemical properties. They are very reactive, especially with water, and tend to lose their single valence electron in chemical reactions. Similarly, halogens in group 17 also share properties, such as seven valence electrons and high electronegativity.

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The ion formed by aluminum has a charge of 3+, known as Al³+. This aluminum cation is formed when aluminum loses three electrons, representing three more positive charges than it has electrons. The charge of 3+ is typical for ions formed from group 13 elements on the periodic table, like aluminum.

The charge on the ion formed by aluminum is 3+. Aluminum, identified by the atomic number 13 on the periodic table, forms a cation when it loses three electrons, resulting in three more positive charges than it has electrons. This is the aluminum cation, represented as Al³+.

Aluminum falls into group 13 of the periodic table, wherein the charge of a cation formed by the loss of all valence electrons is equal to the group number minus 10. Hence, aluminum (in group 13) forms 3+ ions (known as Al³+).

In terms of reactivity, aluminum normally uses all of its valence electrons when reacting, resulting in compounds where it typically has an oxidation state of 3+ - making it a cation. Furthermore, many cations formed from aluminum, such as AlF3 and Al2(SO4)3, are even ionic.

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