Is mixing a peanut,pretzel and cereal mixture chemical or physical change?

The atoms get smaller as move left to right of the periodic table which is because this attraction is much stronger than the relatively weak repulsion between electrons.

Periodic table is tabular form of the chemical elements with increasing order by their atomic number and the elements are arranged in groups on the basis of similar properties.

Elements of the periodic table which are arranged from left to right and top to bottom with respect to increasing atomic numbers.

Elements in the same group will have the same valence electron configuration have same chemical properties while elements  will have an increasing order of valence electrons.

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Since the density of water is 1 g /mL, hence there is 100 g of H2O. So total mass is:

m = 100 g + 5 g = 105 g

=> The heat of reaction can be calculated using the formula:

δhrxn = m C ΔT

where m is mass, C is heap capacity and ΔT is change in temperature = negative since there is a decrease

δhrxn = 105 g * 4.18 J/g°C * (-2.30°C)

δhrxn = -1,009.47 J

=> However this is still in units of J, so calculate the number of moles of NaCl.

moles NaCl = 5 g / (58.44 g / mol)

moles NaCl = 0.0856 mol

=> So the heat of reaction per mole is:

δhrxn = -1,009.47 J / 0.0856 mol

δhrxn = -11,798.69 J/mol = -11.8 kJ/mol

The general properties of the elements to the right in the modern periodic table are low melting and boiling point, high ionization energy, high electron affinity, poor conductor, and lack of metallic luster.

The elements present on the right-hand side of the modern periodic table are nonmetals. Nonmetals are the elements that form negative ions by gaining electrons and have 4, 5, 6, or 7 electrons in their outermost shell.

Non-metals lack all metallic attributes and are good insulators of heat and electricity. They are generally gases at room temperature and sometimes liquid.

Nonmetals are high ionization energies and high electronegativity so they gain electrons when reacting with other compounds, to form covalent bonds.

Nonmetals have high electronegativities so they have a strong tendency to attract electrons. Nonmetals exist as liquids or gases therefore, they have low melting and boiling points under normal conditions.

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Pure substances are made by a single kind of matter and it cannot be separated whereas, mixtures are substance formed by the mixing of two or more pure substances. Thus, option A is correct.

Mixtures are combination of two or more substances which are mixed in a homogenous or heterogenous fashion. Homogenous mixtures are those which appear to be one component like salt solution where only one phase exists.

Heterogenous mixtures forms different phases and the individual components are not uniform will seen separately. Mixtures can be separated based on the properties of the individual components such as using distillation, filtration, chromatography etc.

Pure substances are formed by single type of atoms for example pure water, fruit pies, pure acids etc. They contains their own particles only. Hence, option A is correct.

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Answer:

Boiling point of water = 100 C. It is an intensive property.

Explanation:

Properties of matter can be broadly classified into two categories:

1) Chemical

2) Physical

Physical properties can be further classified as intensive and extensive properties

Intensive properties are properties that do not depend on the amount of matter. For example: Temperature, color, boiling point, melting point

Extensive properties are properties that  depend on the amount of matter. For example: Volume, mass, length

Water boils at a temperature of 100 C; this value is a constant irrespective of the volume (amount) of water. Hence boiling point is an intensive property.

Fluorine and Nitrogen are both non-metals which posses non polar covalent bonds. BaO on the other hand is a combination of a metal (Ba) and non metal (O) hence making it an ionic bond. So in this case, only SO2 has polar covalent bond.

Answer:

SO2

Sulfur dioxide (SO2) is a substance with polar covalent bonds among the given options. It has atoms with different electronegativities, hence the unequal sharing of electrons. SO2's bent molecular shape also contributes to its overall polarity.

The substance with polar covalent bonds among N2, BaO, F2, and SO2 is SO2 (sulfur dioxide). Polar covalent bonds occur when there is an unequal sharing of electrons between atoms with different electronegativities.

Nitrogen (N2) and Fluorine (F2) are both diatomic molecules of the same element and thus have nonpolar covalent bonds because they share electrons equally. Barium oxide (BaO) is an ionic compound because it is composed of a metal and a nonmetal.

Sulfur dioxide (SO2), on the other hand, has atoms with different electronegativities which leads to an unequal sharing of electrons and the formation of polar covalent bonds. The molecule is also bent in shape, which contributes to its overall polarity.

Answer:

Lewis Dot Diagram

Explanation:

Answer:

Compounds can be broken down into simpler substances by chemical means.

Each compound is composed of two or more types of atoms

Explanation:

im doing a 50 question quiz and this is my answer

Conserving mass in a chemical reaction means the atoms of each type should be the same on both the reactant and the product side.

Further explanation:

Balanced chemical reaction:

The chemical reaction that contains an equal number of atoms of the different elements in the reactant as well as in the product side is known as a balanced chemical reaction. The chemical equation is required to be balanced to follow the Law of conservation of mass.

Law of conservation of mass:

According to this law, the mass of an isolated system can neither be created nor be destroyed in any chemical reaction. The mass of reactants and the products should be equal in accordance with this law. In other words, the number of atoms of each type should be same on both sides of the chemical reaction. The reactant is the substance that undergoes a change in itself in a chemical reaction whereas the product is the one that is formed as a result of the chemical reaction.

For example, the balanced chemical reaction between [tex]{{\text{P}}_{\text{4}}}[/tex] and [tex]{\text{C}}{{\text{l}}_{\text{2}}}[/tex] occurs as follows:

[tex]{{\text{P}}_4} + 10{\text{C}}{{\text{l}}_2} \to 4{\text{PC}}{{\text{l}}_5}[/tex]

Here,

[tex]{{\text{P}}_{\text{4}}}[/tex] and [tex]{\text{C}}{{\text{l}}_{\text{2}}}[/tex] are the reactants.

[tex]{\text{PC}}{{\text{l}}_5}[/tex] is the product.

In the above reaction, the number of potassium atoms on both reactant and product side is 4 while the number of chlorine atoms on both sides is 20. So Law of conservation of mass is followed.

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Answer details:

Grade: High School

Subject: Chemistry

Chapter: Basic concepts of chemistry

Keywords: balanced chemical reaction, law of conservation of mass, reactant, product, P4, Cl2, PCl5, 10 Cl2, 4 PCl5, atoms, same.

Final answer:

There are 6.022 × 1023 oxygen atoms in 0.500 mol of carbon dioxide, calculated by doubling the moles of CO2 for oxygen and then multiplying by Avogadro's number.

Explanation:

The question asks how many oxygen atoms are present in 0.500 mol of carbon dioxide (CO2). To find this, we need to use Avogadro's number, which is 6.022 × 1023 atoms/mole, and the fact that each molecule of CO2 contains two oxygen atoms. Here is the calculation:

First, determine the number of moles of oxygen atoms. Since there are 2 moles of oxygen atoms for every mole of CO2, we have 0.500 mol × 2 = 1.000 mol of oxygen.

Next, multiply the number of moles of oxygen by Avogadro's number to get the total number of oxygen atoms: 1.000 mol × 6.022 × 1023 atoms/mole = 6.022 × 1023 oxygen atoms.

Therefore, 0.500 mol of carbon dioxide contains 6.022 × 1023 oxygen atoms.

In 0.500 mol of CO2, there are approximately 6.022 × 10^23 oxygen atoms, calculated using Avogadro's number and stoichiometry.

To determine the number of oxygen atoms in 0.500 mol of carbon dioxide (CO2), we can use Avogadro's number and the stoichiometry of the compound. Avogadro's number (6.022 x 10^23) represents the number of entities (atoms, molecules, ions) in one mole of a substance.

The chemical formula for carbon dioxide is CO2, which indicates that one mole of CO2 contains one mole of carbon atoms and two moles of oxygen atoms.

Given that the molar mass of oxygen (O) is approximately 16 g/mol, and CO2 has a molar mass of approximately 44 g/mol, we can find the moles of oxygen in 0.500 mol of CO2.

Moles of O = Moles of CO2 × (Moles of O / Moles of CO2)

Moles of O = 0.500 mol × (2 / 1) = 1.000 mol O

Now, using Avogadro's number, we can find the number of oxygen atoms:

Number of oxygen atoms = Moles of O × Avogadro's number

Number of oxygen atoms ≈ 1.000 mol × 6.022 × 10^23 atoms/mol

Number of oxygen atoms ≈ 6.022 × 10^23 atoms

The three main subatomic particles in an atom are protons, neutrons, and electrons. Protons have a mass of 1.0073 amu and a charge of +1, neutrons have a mass of 1.0087 and no charge, and electrons have a mass of 0.00055 amu and a charge of -1. The sum of the particles' masses doesn't equal an atom's actual mass which is termed as a mass defect in nuclear chemistry.

The question refers to the basic properties of three primary subatomic particles found in an atom: protons, neutrons, and electrons. A proton has a mass of 1.0073 atomic mass units (amu) and a charge of +1. A neutron has a slightly higher mass of 1.0087 amu and is neutral, holding no charge. An electron has a much lighter mass of about 0.00055 amu and it carries a charge of -1.

However, it's interesting to note that if you add up the mass of these subatomic particles, the total doesn't equal the actual mass of an atom. For instance, the total mass of six protons, six neutrons, and six electrons is approximately 12.0993 amu, a bit larger than the known 12.00 amu of a carbon atom. The discrepancy is referred to as the mass defect and is explained in detail in the field of nuclear chemistry.

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To determine the number of atoms in 3.08 mol of pure aluminum, multiply the number of moles by Avogadro's number.

In order to determine the number of atoms in 3.08 mol of pure aluminum, we need to use Avogadro's number. Avogadro's number is a fundamental constant in chemistry that represents the number of atoms or molecules in one mole of a substance. It is approximately equal to 6.022 × 10²³ atoms/mol.

To find the number of atoms in 3.08 mol of pure aluminum, you can use the following calculation:

Number of atoms = 3.08 mol × (6.022 × 10²³ atoms/mol)

By performing this calculation, you will find the number of atoms in 3.08 mol of pure aluminum.

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First of all, convert given masses to number of moles:

H2 = 15 kg / (2 kg / kmol) = 7.5 kmol

N2 = 15 kg / (28 kg / kmol) = 0.5357 kmol

NH3 = 13.7 kg / (17 kg/ kmol) = 0.8059 kmol

The balanced chemical reaction is:

N2 + 3H2  -->  2NH3

We can see that N2 is the limiting reactant and for every 1 mole of N2, there are 2 moles of NH3 produced, hence:

NH3 theoretically produced = 0.5357 kmol * (2 / 1) = 1.0714 kmol

Therefore the percent yield assuming that the reaction is complete is:

% yield = (0.8059 kmol / 1.0714 kmol) * 100

% yield = 75.22%

The percent yield of ammonia produced from 15.0 kg each of H₂ and N₂, with 13.7 kg of product recovered, assuming the reaction goes to completion, is approximately 75.7%.

To calculate the percent yield, we first need to determine the theoretical yield, which is the amount of product that would be formed if the reaction went to completion with 100% efficiency.

The balanced chemical equation for the production of ammonia from hydrogen (H₂) and nitrogen (N₂) is:

[tex]\[ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \][/tex]

From the stoichiometry of the reaction, 1 mole of N₂ reacts with 3 moles of H₂ to produce 2 moles of NH₃. The molar masses of N₂, H₂, and NH₃ are approximately 28.02 g/mol, 2.016 g/mol, and 17.03 g/mol, respectively.

First, we calculate the moles of N₂ and H₂:

[tex]\[ \text{Moles of } N_2 = \frac{15.0 \times 10^3 \text{ g}}{28.02 \text{ g/mol}} \approx 535.4 \text{ mol} \][/tex]

[tex]\[ \text{Moles of } H_2 = \frac{15.0 \times 10^3 \text{ g}}{2.016 \text{ g/mol}} \approx 7439.7 \text{ mol} \][/tex]

Since the reaction requires 3 moles of H₂ for every mole of N₂, and we have more than enough H₂, N₂ is the limiting reactant. Therefore, the theoretical yield of NH₃ is determined by the amount of N₂:

[tex]\[ \text{Theoretical yield of } NH_3 = 535.4 \text{ mol} \times \frac{2 \text{ mol } NH_3}{1 \text{ mol } N_2} \times \frac{17.03 \text{ g}}{1 \text{ mol } NH_3} \][/tex]

[tex]\[ \text{Theoretical yield of } NH_3 \approx 18037.4 \text{ g} \approx 18.0374 \text{ kg} \][/tex]

Now, we calculate the percent yield using the actual yield (13.7 kg) and the theoretical yield:

[tex]\[ \text{Percent yield} = \left( \frac{\text{Actual yield}}{\text{Theoretical yield}} \right) \times 100\% \][/tex]

[tex]\[ \text{Percent yield} = \left( \frac{13.7 \text{ kg}}{18.0374 \text{ kg}} \right) \times 100\% \approx 75.97\% \][/tex]

The correct number of neutrons in the nucleus of the second isotope of rubidium is 50.

To solve this problem, we can use the weighted average of the atomic masses of the two isotopes to find the number of neutrons in the second isotope. Let's denote the number of neutrons in the second isotope as [tex]\( n \)[/tex].

We know the following:

- The first isotope has 48 neutrons and a natural abundance of 72%.

- The calculated atomic mass of rubidium is 85.5.

- The second isotope has \( n \) neutrons and a natural abundance of [tex]\( 100\% - 72\% = 28\% \)[/tex].

The atomic mass of an isotope is calculated by adding the number of protons and neutrons in its nucleus. Since rubidium has 37 protons, the atomic mass of the first isotope is [tex]\( 37 + 48 = 85 \)[/tex].

Now, let's set up the equation for the weighted average atomic mass:

[tex]\[ 0.72 \times 85 + 0.28 \times (37 + n) = 85.5 \][/tex]

Solving for [tex]\( n \)[/tex]:

[tex]\[ 61.2 + 0.28n = 85.5 \] \[ 0.28n = 85.5 - 61.2 \] \[ 0.28n = 24.3 \] \[ n = \frac{24.3}{0.28} \] \[ n = 86.79 \][/tex]

Since the number of neutrons must be a whole number, we round to the nearest whole number:

[tex]\[ n \approx 87 \][/tex]

However, we must subtract the number of protons (37) to find the number of neutrons:

[tex]\[ n_{\text{neutrons}} = 87 - 37 \][/tex]

[tex]\[ n_{\text{neutrons}} = 50 \][/tex]

Therefore, the second isotope of rubidium contains 50 neutrons in its nucleus.

The ph of a solution that is 0.278 m in sodium formate (NaHCO₂)  and 0.222 m in formic acid (HCO₂H) is 3.84

To calculate the pH of the solution containing sodium formate (NaHCO₂) and formic acid (HCO₂H), we first need to determine the concentrations of the formate ion (HCO₂⁻) and the formic acid (HCO₂H) in the solution.

Given:

1. Since sodium formate dissociates completely in water, the concentration of formate ion (HCO₂⁻) is equal to the concentration of sodium formate

2. The formic acid (HCO₂H) will partially dissociate in water according to the equilibrium equation:

Let x be the concentration of H⁺ ions formed from the dissociation of formic acid. Therefore, at equilibrium:

3. The equilibrium constant expression for the dissociation of formic acid is given by:

Substitute the expressions in terms of x into the equation above:

4. Calculation of pH

Therefore, The ph of a solution that is 0.278 m in sodium formate (NaHCO₂)  and 0.222 m in formic acid (HCO₂H) is 3.84