6a. What event is occuring
Chemical Change or Physical Change

The number of moles of the gas present in the container at 1195 K and pressure of 1.65 atm is 0.45 mole

From the question given above, the following data were obtained obtained:

Using the ideal gas equation, we can obtain the number of mole present in the container as follow:

PV = nRT

1.65 × 27 = n × 0.0821 × 1195

44.55 = n × 98.1095

Divide both sides by 98.1095

n = 44.55 / 98.1095

n = 0.45 mole

Thus, we can conclude that the number of mole of the gas present in the container is 0.45 mole

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The formula of De Broglie is the following:

Remember that the mass of an electron is 9.11 x 10 ^(-31) kg, so replacing in the formula, we're going to obtain:

The answer is that the wavelength of an electron traveling at 1.48 x 10^(5) m/s is 4.91 x 10^(-9) m.

There are different types of reactions which are classified based on the mode of regrouping of atoms between the reactants. Some of the reaction types are synthesis, decomposition, displacement etc.

There are different types of reaction based on the regrouping of atoms to form a new product. Some of them are described below:

Synthesis reactions:

This type of reactions involves combination of two reactants to produce a single product as follows:

A + B →C

Decomposition reactions:

Decomposition of a compound into its constituent elements or compounds as written below:

AB₂ → A + 2B

Displacement reaction:

In displacement reactions, one or two group of the reactants are displacing each other.

AB + CD → AC + BD - double displacement

AB + C → AC + B - single displacement.

Combustion reaction:

This reaction is the reaction with oxygen forming carbon dioxide and water.

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Answer:

C. 7.4 kJ

Explanation:

Let assume that Mercury is at room temperature (25 °C). The energy required to boil the sample of mercury is the sum of sensible and latent heats. Mercury has a fussion and boiling points of -38.83 °C and 356.7 °C, respectively, and a specific heat of \(138\,\frac{J}{kg\cdot ^{\circ}C}\). Then:

\(Q = (25\,g)\cdot \left[\left(0.138\,\frac{J}{g\cdot ^{\circ}C} \right)\cdot (356.7^{\circ}C - 25^{\circ}C) + 296\,\frac{J}{g} \right]\)

\(Q = 8544.365\,J\)

The option that offers the best approximation to the result is C.

Answer:

crystallized by heating the salt solution

Salt solutions can be crystallized to give solid salts.

Answer:

The shapes of continents fit together like a puzzle.

Explanation:

Just look at the east coast of South America and the west coast of Africa—it's almost a perfect fit! Identical rocks have been found on different continents. These rocks formed millions of years ago before the continents separated.

Answer:

Because both the zones have different compositions.

Explanation:

The continental crust is composed of mainly graphite whereas the oceanic crust is made up of basalt. The oceanic plates are thinner than the continental plates. Also the oceanic plates are much denser as compared to the continental plates. Now the continental plates at the convergent boundary gained thickness as they are pushed upward. These plates or zones are of different composition an densities and so when they collide different features can be seen at the two conversion zones.

Answer:

Explanation:

Convert 55lbs to kg

(55 lb)*(453.6 g/lb) = 24948 g or 249.48 kg

Density of zinc = 7140 kg/m^3

Find the volume occupied by 249.48 kg:

  (249.48 kg)/(7140 kg/m^3) = 0.055 m^3

Density of silver = 10,490 kg/m^3

Mass of Ag in 0.055m^3:

  (0.055m^3)*(10,490 kg/m^3) = 577 kg

A 100.0 mL sample of natural water was titrated with 13.57 mL of 0.1123 M Na OH solution to reach a light pink  are the phenolphthalein end point. The number of millimoles of Na OH required for the titration is 1.525011 millimoles. Titration is a technique used in chemistry

to identify the quantity of a substance by adding a reactant until the chemical reaction is completed. In titration, a solution of known concentration (the titrant) reacts with a solution of unknown concentration (the analyte) to determine its concentration. Titration of natural water with Na OH In this case, we are titrating natural water with Na OH to find the concentration of the unknown solution. The balanced chemical reaction for the titration of natural water with Na OH is:H2O + Na OH → Na+ + OH- + H2O

The volume of NaOH required to reach the end-point of the titration is 13.57 mL. The molarity of Na OH used for the titration is 0.1123 M. We can use the following formula to calculate the number of millimoles of Na OH required for the titration Millimoles of Na OH = (Volume of Na OH × Molarity of NaOH) / 1000Substitute the given values in the above equation and solve for the millimoles of Na OH required for the titration. Millimoles of Na OH = (13.57 mL × 0.1123 M) / 1000= 0.001525011 millimoles Therefore, the number of millimoles of NaOH required for the titration is 1.525011 millimoles.

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Answer:

photosynthesis

Explanation:

Answer:its part of the process of photosynthesis

Explanation:

Answer:

A

Explanation:

........................

Answer:

push or pull i think..okay?

Answer: An overturned decomposing log or the underside of a rock in a stream are excellent examples of microhabitats. Both a habitat and a microhabitat have typical abiotic (e.g. water, temperature, light.

Explanation:

The larger ice cubes require more heat from the water to melt. To transfer more heat from the water requires more time. Therefore, it takes longer for the larger ice cubes to melt.

The energy that is released for the breaking of bonds is 229 kJ/mol.

We should be able to recall that the enthalpy of the reaction taken to be the energy that is evolved or absorbed in the reaction that is ongoing. We have to note that in the course of the reaction there would be the breaking and the making of bonds.

Now we know that;

The bond energy can be given as;

Sum energy of the broken bonds of reactants  - Sum of the energy of the formed bonds

Hence;

(945 + 498) - 2(607)

1443 - 1214

= 229 kJ/mol

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Given, Manganese dioxide (MnO2) = 28gHydrochloric acid (HCl) = 42g

To find, Theoretical yield of Cl2, We will find the limiting reagent and use its mole to find the theoretical yield of Cl2.MnO2 + 4HCl → MnCl2 + 2H2O + Cl2First we will find the limiting reagent.

The number of moles of MnO2 is, Moles of MnO2 = Mass/Molar mass = 28/86.94 = 0.322 mol The number of moles of HCl is, Moles of HCl = Mass/Molar mass = 42/36.46 = 1.151 mole will use the mole ratio of MnO2 and HCl to find the mole of Cl2. The mole of HCl required to react with 0.322 mol of MnO2 = 0.322 x 4 = 1.288 mol The number of moles of Cl2 will be, Moles of Cl2 = 0.322 x 1 / 4 = 0.0805 mol. The theoretical yield of Cl2 from the given reactants is,

Theoretical yield of Cl2 = Moles x Molar mass = 0.0805 x 70.9 = 5.71 g Chlorine gas will be produced with a theoretical yield of 5.71 g when 28 g of MnO2 and 42 g of HCl are mixed.

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Answer:

because the two are opposite compounds.

Explanation:

When Chlorine is passed through aqueous sodium fluorine then no reaction takes place between these two because of reactivity order of Fluorine and Chlorine

Displacement reaction is a reaction in which one atom replaces other atom from a molecule on the basis of reactivity strength.

The reason for such reactivity is that as we go down the group the number of shells increases so outermost shell is very far away from the nucleus. If any atom from outside coming to this nucleus then this nucleus is unable to attract the electron of that that atom. Reactivity of halogens is directly proportional to the electronegativity power of that element, that is power to attract electron. Reactivity of halogens decreases down the group.

So Chlorine is less reactive than Fluorine so Chlorine can not replace Fluorine from sodium fluoride. Hence no reaction will take place.

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Science is used to stop things the are incrediblu diffucult to deal with therefore jeg spiser ikke dreng

The answer is

It can identify the sources of polluted water.

Answer:  extremely sensitive to environmental changes caused by habitat destruction, climate change, pollution

Explanation:

Across the world, amphibians have been disappearing at an unprecedented rate — faster than any other group of animals. Frogs, toads, and salamanders are extremely sensitive to environmental changes caused by habitat destruction, climate change, pollution, and invasive species.

(a) First, we need to write the combustion reaction for ethanol (CH3CH2OH)

CH3CH2OH + O2 → CO2 + H2O

Then, we need to balance this equation. To do that, remember to start with C, then move on to H and finally balanced the amount of O:

CH3CH2OH + 3 O2 → 2 CO2 + 3 H2O

(b) Since this is a reaction that realeases heat (726.7 kJ /mol of ethanol), we know that is an exothermic reaction and the general scope of an enthalpy diagram would be like this:

Where, for the combustion of ethanol, the reactants would be CH3CH2OH + O2, the products would be CO2 + H2O, and ΔH would be -726.7 kJ/mol

There are approximately 0.0004995 carbon atoms in 10.0 mg of aspirin.

The molar mass of aspirin (C9H8O4) is 180 g/mol. Calculate the number of carbon atoms in 10.0 mg of aspirin. The molar mass of C9H8O4 = 9 x atomic mass of C + 8 x atomic mass of H + 4 x atomic mass of O= 9 x 12.011 + 8 x 1.008 + 4 x 15.999= 180.16 g/mol.

Hence, 1 mole of aspirin weighs 180.16 g and contains 9 moles of carbon atoms (1 mole of C9H8O4 contains 9 carbon atoms). Number of moles of aspirin in 10.0 mg = 10.0 mg/180.16 g/mol= 0.0000555 mol. Number of carbon atoms in 10.0 mg of aspirin= 9 x 0.0000555= 0.0004995.

Therefore, there are approximately 0.0004995 carbon atoms in 10.0 mg of aspirin.

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The molality of the sucrose solution is 1.16 m

The molality of a solution is defined as the mole of solute per unit kilogram (Kg) of water. Mathematically, it can be expressed as:

Molality = mole / mass (Kg) of water

Mole = mass / molar mass

Mole of sucrose = 37.4 / 342.2

Mole of sucrose = 0.109 mole

Molality = mole / mass (Kg) of water

Molality of sucrose = 0.109 / 0.0942

Molality of sucrose = 1.16 m

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The oxidizing agent are the substance that is reduced because it gains electrons.

An oxidizing agent is defined as the agent that is capable of undergoing oxidation reaction by losing an electron.

The following are the characteristics of an oxidizing agent:

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Answer:

D: the substance that is reduced because it gains electrons.

Explanation:

The lowest representational unit for an ionic compound is a formula unit.

The smallest unit in which a substance naturally exists is called a representative particle. The atom is the representative particle for most elements. The atom is the representative particle for most elements. Iron, carbon, and helium are made up of individual iron, carbon, and helium atoms.

Subatomic is defined as "less than an atom." Protons, neutrons, and electrons make up atoms. Even smaller particles known as quarks are the building blocks of protons and neutrons. Physicists believe quarks are elementary particles based on the evidence that is currently available.

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Answer:

Explanation:

They play a very important part. The geometry is not a straight line. It is an angle over 90 which means that the molecule has the same general shape as a boomerang. The two hydrogens and the 2 lone electron pairs try to get away as far as possible from each other. The actual shape results in a tetrahedron shape. But the two hydrogens and 1 oxygen actually look like the aforementioned boomerang.

Answer:

1.

a. Sodium

b.Hydrogen

c Carbon

d Oxygen

2.

a He

b S

c Cu

d Pb

Answer:

1.

a. Sodium

b.Hydrogen

c Carbon

d Oxygen

2.

a He

b S

c Cu

d Pb

Explanation:

Hope this will help

If the experiment is repeated at the pH 11 level, the enzyme activity will be less than at the pH 9 level.

We can arrive at this answer because:

In this case, we can say that if the experiment is repeated at pH 11, the enzyme activity level will be even lower, since from pH 5 onwards, as the pH rises, the enzyme activity goes down.

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Nanomaterials, whether natural, engineered, organic, or inorganic, offer various applications across industries. However, their environmental health and safety impacts need to be carefully evaluated and managed to mitigate any potential risks.

Understanding their properties, fate, and behavior in different environments is crucial for responsible development, use, and disposal of nanomaterials.

Natural Nanomaterials:

Examples: Carbon nanotubes (CNTs) derived from natural sources like bamboo or cotton, silver nanoparticles in natural colloids, clay minerals (e.g., montmorillonite), iron oxide nanoparticles found in magnetite.

Uses: Natural nanomaterials have various applications in medicine, electronics, water treatment, energy storage, and environmental remediation.

Environmental health and safety impacts: The environmental impacts of natural nanomaterials can vary depending on their specific properties and applications. Concerns may arise regarding their potential toxicity, persistence in the environment, and possible accumulation in organisms. Proper disposal and regulation of their use are essential to minimize any adverse effects.

Engineered Nanomaterials:

Examples: Gold nanoparticles, quantum dots, titanium dioxide nanoparticles, carbon nanomaterials (e.g., graphene), silica nanoparticles.

Uses: Engineered nanomaterials have widespread applications in electronics, cosmetics, catalysis, energy storage, drug delivery systems, and sensors.

Environmental health and safety impacts: Engineered nanomaterials may pose potential risks to human health and the environment. Their small size and unique properties can lead to increased toxicity, bioaccumulation, and potential ecological disruptions. Safe handling, proper waste management, and risk assessment are necessary to mitigate any adverse effects.

Organic Nanomaterials:

Examples: Nanocellulose, dendrimers, liposomes, organic nanoparticles (e.g., polymeric nanoparticles), nanotubes made of organic polymers.

Uses: Organic nanomaterials find applications in drug delivery, tissue engineering, electronics, flexible displays, sensors, and optoelectronics.

Environmental health and safety impacts: The environmental impact of organic nanomaterials is still under investigation. Depending on their composition and properties, they may exhibit varying levels of biocompatibility and potential toxicity. Assessments of their environmental fate, exposure routes, and potential hazards are crucial for ensuring their safe use and minimizing any adverse effects.

Inorganic Nanomaterials:

Examples: Quantum dots (e.g., cadmium selenide), metal oxide nanoparticles (e.g., titanium dioxide), silver nanoparticles, magnetic nanoparticles (e.g., iron oxide), nanoscale zeolites.

Uses: Inorganic nanomaterials are utilized in electronics, catalysis, solar cells, water treatment, imaging, and antimicrobial applications.

Environmental health and safety impacts: Inorganic nanomaterials may have environmental impacts related to their potential toxicity, persistence, and release into ecosystems. Their interactions with living organisms and ecosystems require careful assessment to ensure their safe use and minimize any negative effects.

Understanding their properties, fate, and behavior in different environments is crucial for responsible development, use, and disposal of nanomaterials.

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Two new compounds are the most likely description of the products of a double-displacement reaction (Option B).

A double displacement chemical reaction can be defined as a reaction where ions present in two different compounds react in order to generate one or more new compounds which are present in an aqueous media.

Therefore, with this data, we can see that a double displacement chemical reaction is based on the reaction of ionic compounds in order to generate two or more new compounds in water.

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