A sample of a compound contains 60.0 g C and 5.05 g H. Its molar mass is 78.12 g/mol. What is the compound’s molecular formula? CH C2H2 C6H6 C6H

Answer:

1.67m

Explanation:

Final answer:

J. J. Thomson discovered electrons, Ernest Rutherford found protons, and James Chadwick discovered neutrons, all of which conflicted with Dalton's theory of indivisible atoms.

Explanation:

Dalton's Atomic Theory stated that matter is made up of indivisible particles called atoms. However, subsequent scientists' discoveries supported or differed from Dalton's theory in the following ways:

Types of Bonds can be predicted by calculating the difference in electronegativity.

If, Electronegativity difference is,

                Less than 0.4 then it is Non Polar Covalent

                Between 0.4 and 1.7 then it is Polar Covalent 

                Greater than 1.7 then it is Ionic

For Be and F,

                    E.N of Fluorine          =   3.98

                    E.N of Beryllium        =   1.57

                                                   ________

                    E.N Difference                2.41          (Ionic Bond)

For H and Cl,

                    E.N of Chorine           =   3.16

                    E.N of Hydrogen        =   2.20

                                                   ________

                    E.N Difference                0.96          (Polar Covalent Bond)

For Na and O,

                    E.N of Oxygen          =   3.44

                    E.N of Sodium          =   0.93

                                                       ________

                    E.N Difference                2.51          (Ionic Bond)

For F and F,

                    E.N of Fluorine          =   3.98

                    E.N of Fluorine          =   3.98

                                                        ________

                    E.N Difference                0.00         (Non-Polar Covalent Bond)

Result:

           A polar covalent bond is formed between Hydrogen and Chlorine atoms.

Answer:

[tex]SO_4^-[/tex]

Explanation:

The sodium sulfate compound corresponds to a water soluble salt.

When a salt dissolves it will dissociate into the ions that compose it.

It dissociates into Cations (positively charged ions) and anions (negatively charged ions)

Sodium sulfate formula

[tex]Na_2SO_4[/tex]

Sodium sulfate when dissolved in water

[tex]Na_2SO_4\stackrel{H_2O}{\longrightarrow} 2Na^+SO_4^-[/tex]

Ions present in the solution:

[tex]Na^+[/tex] Cation

[tex]SO_4^-[/tex] Anion

Approximately 200.6 grams of Aluminum will be produced from the electrolysis of molten AlCl3 for 3.25 hours with an electrical current of 15.0 A, as determined through application of Faraday's law of electrolysis.

In order to determine the number of grams of aluminum produced from electrolysis of molten AlCl3, we need to use Faraday's law of electrolysis.

Faraday's law states that the amount of substance produced at an electrode during electrolysis is directly proportional to the number of moles of electrons (or amount of electrical charge) transferred at that electrode. The charge Q in coulombs (C) can be calculated using the formula Q = It, where I is the current in amperes (A) and t is the time in seconds.

For this scenario, we know that the current I is 15.0 A and the time t is 3.25 hours, which needs to be converted to seconds for the equation to work properly (3.25 hr × 3600 s/hr = 11700 s). Hence, Q = 15.0 A × 11700 s = 175500 C.

The quantity of a substance produced in an electrolytic cell is given by the equation  m = Q × M / F × n, where M is the molar mass of the substance, F is Faraday's constant (~96485 C/mol), and n is the number of electrons transferred per formula unit of the substance. In this case, M = 26.98 g/mol for Al, n = 3 for Al3+, so m = 175500 C × 26.98 g/mol / (96485 C/mol × 3) = 200.6 g

Therefore, approximately 200.6 g of Aluminum will be produced from the electrolysis of AlCl3 in 3.25 hours with an electrical current of 15.0 A.

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Answer:It might have 10 neutrons

Reason: This is because an isotope of the same element must have the same number of electrons and protons so it can be assumed that the amount of neutrons can be changed.

The molecule containing a special group attached to its side chain is a fundamental group. The molecules are acid, ether, ester, aldehyde, ketone, amine, and alcohol.

Functional groups are the specialized molecules that are attached to the main chain and vary the chemical and physical properties of the compound. The molecule containing hydroxide is acid, and the single oxygen atom is ether.

Compound with double-bonded oxygen to alkyl or aromatic group is ester, carbonyl group on carbon with hydrogen and R group is an aldehyde, carbonyl group attached to carbon-containing two alkyl or aromatic groups is a ketone.

The Amine group includes an aromatic or an alkyl group attached to two hydrogens of the nitrogen atom. The alcohol group is the attachment of the -OH group to a carbon-containing hydrogen and R group.

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Carbon generally has a higher electronegativity than aluminum, so a carbon atom has a stronger attraction for bonding electrons.

The strength of an atom's attraction for the electrons in a bond is measured by its electronegativity. Among the elements listed, carbon generally has a higher electronegativity than aluminum, which means that an atom of carbon will typically have a stronger attraction for the electrons in a bond. The concept of electronegativity is crucial in understanding the behavior of atoms in different chemical compounds and their ability to attract bonding electrons.

Saturated hydrocarbons, such as alkanes, are utilized in combustion processes for producing heat due to their single carbon-to-carbon bonds.

Saturated hydrocarbons, also known as alkanes, involve the direct use of hydrocarbons with only single carbon-to-carbon bonds. An example of an activity that most likely involves the direct use of saturated hydrocarbons is combustion processes for producing heat. These hydrocarbons are composed entirely of single bonds and are saturated with hydrogen.

Plants primarily obtain nitrogen from soil in the forms of nitrates (NO₃⁻) and ammonium ions (NH₄), which become available through the processes of nitrogen fixation and nitrification by certain bacteria.

Nitrogen is available to plants mostly in the form of nitrate and ammonium ions in the soil. Atmospheric nitrogen, which composes 78% of the air, is not directly usable by plants due to its strong triple bonds. Through the nitrogen cycle, nitrogen is converted into biologically available forms.

One such process is nitrogen fixation, where free-living or symbiotic bacteria, such as Rhizobium in legume roots, convert gaseous nitrogen (N₂) into ammonia (NH₃). This ammonia can become ammonium (NH₄) and is then available for plant uptake, or it can be further processed by nitrifying bacteria into nitrites (NO₂⁻) and subsequently into nitrates (NO₃⁻), which are absorbed by plant roots.

The availability of ammonia and nitrates in the soil is crucial for plants to synthesize essential compounds like proteins and nucleic acids, making nitrogen a limiting nutrient for plant growth.

Monomers are generally small molecules that make up a long polymeric chain. The monomer for lipids is triglycerides.

A triglyceride is an ester consisting of three fatty acids and glycerol. Triglycerides are the main components of human body fat.

Lipids are made up of long chains of triglycerides.

Thus, the correct option is B.

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Let's assume that both He and N₂ have ideal gas behavior.

Then we can use ideal gas law,
     PV = nRT
Where, P is the pressure of gas, V is the volume, n is moles of gas, R is universal gas constant and T is the temperature in Kelvin.

The P and V are same for the both gases.
R is a constant.

The only variables are n and T.

Let's say temperature of He is T₁ and temperature of N₂ is T₂.

n = m/M where n is moles, m is mass and M is molar mass.

Molar mass of He is 4 g/mol and molar mass of N₂ is 28 g/mol

Since mass (m) of both gases are same,
 moles of He = m/4
 moles of N₂ = m/28

Let's apply the ideal gas equation for both gases.
For He gas,
 PV = (m/4)RT₁              (1)

For N₂ gas,
 PV = (m/28)RT₂            (2)

(1) = (2)
(m/4)RT₁ = (m/28)RT₂ 
        T₁/4 = T₂/28
        T₁    = T₂/7
        7T₁  = T₂

Hence, the temperature of N₂ gas is higher by 7 times than the temperature of He gas.

Given the same mass and pressure, the temperature of the helium would be the same as the temperature of nitrogen. This is due to the ideal gas law, which connects the variables of pressure, volume, temperature, and the number of moles of a gas.

The temperature of the helium would be the same as the temperature of nitrogen, given that the quantities (in terms of mass) are the same and they are at the same pressure. This follows from the ideal gas law which states that pressure is directly proportional to temperature and the number of moles of the gas, and inversely proportional to volume. Considering this in context, helium and nitrogen have different molar masses. For a given mass, there will be more moles of helium (which has a lower molar mass) than of nitrogen (which has a higher molar mass). Therefore, if the mass, volume, and pressure are held constant, the temperature for equal masses of the two gases will also be constant. More moles of gas does not mean a higher temperature, contrary to what one might intuitively think.

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Factors affecting the rate of a chemical reaction in the context of a specific reaction equation.

The factors that affect the rate of the reaction Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) include:

Catalyst: Adding a catalyst can increase the rate of the reaction.

Surface area: Grinding the zinc solid into a fine powder increases its surface area, enhancing the reaction rate.

Concentration and Temperature: Increasing the concentration of HCl or raising the temperature can also speed up the reaction.

ANSWER: C temperature of the gas

Answer:

(C) The temperature of gas

Explanation:

It's correct for Plato

You need 1000 milliliters of a 1.0 M AgNO3 solution to provide 169.9 g of pure AgNO₃.

Step 1: Calculate the moles of AgNO₃ needed. To do this, use the given molar mass of AgNO₃, which is 169.87 g/mol.

Moles = mass / molar mass

Moles of AgNO₃ = 169.9 g / 169.87 g/mol = 1.000 mol

Step 2: Determine the volume of the 1.0 M AgNO₃ solution required to obtain 1.000 mol of AgNO₃.

Molarity (M) = moles of solute / liters of solution

Rearranging the formula to solve for volume (liters):

Volume (L) = moles of solute / Molarity

Volume (L) = 1.000 mol / 1.0 M = 1.000 liters

Since the question asks for the volume in milliliters:

Volume (mL) = Volume (L) * 1000

Volume (mL) = 1.000 L * 1000 = 1000 mL

Therefore, you need 1000 milliliters of a 1.0 M AgNO₃ solution to provide 169.9 g of pure AgNO₃.