Answers
Answer: Option (B) is the correct answer.
Explanation:
A state of matter where molecules are held together by strong intermolecular forces of attraction are known as solid substances. As a result, they are unable to move from their initial place but they can vibrate at their mean position.
Hence, in solid substances the molecules have low kinetic energy.
In liquids, the molecules are held by less strong intermolecular forces of attraction as compared to solids. Due to which they are able to slide past each other. Hence, they have medium kinetic energy.
In gases, the molecules are held by weak Vander waal forces. Hence, they have high kinetic energy due to which they move rapidly from one place to another leading to more number of collisions.
Thus, we can conclude that water molecules are listed from A to B to C in least to greatest motion.
Related Questions
List a few of the physical properties of graphite.
Answers
How many total atoms are in 0.330 g of P2O5?
Answers
B) 1 mole of anything contains the Avogradro Number of molecules
So here it is 6.02 x 10^23 x Y molecules
C) work out how many atoms in each molecule 2P + 5O total 7
So multiply answer to B by 7 to get final answer
How many moles of CuCl2 are there if you have 650 grams of it?
Answers
Solution,
Molar mass of CuCl2 = 134.45 g
Given mass = 650 g
so,
No.of moles= 650 * 1 mole of CuCl2/ 134.45
= 4.8 moles
How many moles in 1.3g sodium bicarbonate
Answers
Find the g-f-m if sodium bicarbonate which is 84 g/mol.
To find the moles of sodium carbonate, you would divide the grams by the gfm.
1.3g
——= .015 mol
84 g/mol
(*** I rounded to 2 sig figs as the final answer***)
Your body's "thermostat" is called the _____. thyroid hypothalamus thalamus parathyroid
Answers
Your body's "thermostat" is called the hypothalamus!
Hydroxylamine is a weak molecular base with kb = 6.6 x 10-9. what is the ph of a 0.0500 m solution of hydroxylamine?
Answers
Kb(NH₂OH) = 1,8·10⁻⁵.
c₀(NH₂OH) = 0,0500 M =
0,05 mol/L.
c(NH₂⁺) = c(OH⁻) = x.
c(NH₂OH) = 0,05 mol/L - x.
Kb = c(NH₂⁺) · c(OH⁻) / c(NH₂OH).
0,0000000066 = x² / (0,05 mol/L - x).
solve quadratic equation: x = c(OH⁻) = 0,000018 mol/L.
pOH = -log(0,000018 mol/L) = 4,74.
pH = 14 - 4,74 = 9,23.
The pH of a 0.0500 M solution of hydroxylamine is 9.26.
To find the pH of a 0.0500 M solution of hydroxylamine, we need to find the hydroxide ion concentration [OH⁻] and then use the pOH-pH relationship.
Since hydroxylamine is a weak base, we can use the following equilibrium equation:
NH₂OH + H₂O ⇌ NH₃OH ⁺+ OH⁻
The base dissociation constant (Kb) is given as 6.6 x 10⁻⁹.
Let x be the concentration of hydroxide ions [OH⁻] formed. Then, the concentration of NH₃OH⁺ will also be x.
The initial concentration of hydroxylamine is 0.0500 M, and since it's a weak base, the amount of hydroxylamine that dissociates is very small compared to the initial concentration. Therefore, we can assume that the concentration of hydroxylamine remains approximately constant at 0.0500 M.
The equilibrium expression for Kb is:
Kb = [NH₃OH⁺][OH⁻] / [NH₂OH] = x² / 0.0500
Rearranging the equation to solve for x:
x² = Kb × 0.0500 = 6.6 x 10⁻⁹ × 0.0500 = 3.3 x 10⁻¹⁰
x = √(3.3 x 10⁻¹⁰) = 1.81 x 10⁻⁵ M
This is the concentration of hydroxide ions [OH⁻].
Now, we can find the pOH using the following equation:
pOH = -log[OH⁻] = -log(1.81 x 10⁻⁵) = 4.74
Finally, we can find the pH using the pOH-pH relationship:
pH + pOH = 14 pH = 14 - pOH = 14 - 4.74 = 9.26
Therefore, the pH of a 0.0500 M solution of hydroxylamine is 9.26.
what energy transformation occurs when an electric lamp is turned on
Answers
What is the maximum mass of ethanol that can be made from 15.5 kg of glucose?
Answers
The maximum mass of ethanol that can be made from 15.5 kg of glucose is 7,93 kg
The transformation of glucose into ethanol is called Alcoholic Fermentation. The general equation for this reaction is the following:
C₆H₁₂O₆ → 2C₂H₅OH + 2CO₂
To know how many grams of ethanol can be made from 15,5 kg of glucose, we'll need to apply the following conversion factor to go from mass of glucose to mass of ethanol, applying the reaction coefficients and molar masses:
[tex]15,5 kg Glc* \frac{1000g}{1kg} \frac{1 mol Glc}{180,156 g Glc}* \frac{2 mol EtOH}{1 mol Glc}* \frac{46,079g EtOH}{1 mol EtOH}* \frac{1kg}{1000g} \\ \\ = 7,93 kg EtOH [/tex]
Have a nice day!
Write a balanced complete ionic equation for: hi(aq)+rboh(aq)→
Answers
The complete ionic equation for the reaction is as follows:
[tex]\boxed{{{\mathbf{H}}^ + }\left( q \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right) + {\mathbf{O}}{{\mathbf{H}}^ - }\left( {aq} \right) \to {{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}\left( l \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right)}[/tex]
Further Explanation:
Double displacement reaction is defined as the reaction in which ions of two compound interchange with each other to form the product. For example, the general double displacement reaction between two compounds AX and BY is as follows:
[tex]{\text{AX}} + {\text{BY}} \to {\text{AY}} + {\text{BX}}[/tex]
The three types of equations that are used to represent the chemical reaction are as follows:
1. Molecular equation
2. Complete ionic equation
3. Net ionic equation
The reactants and products remain in undissociated form in molecular equation. In the case of complete ionic equation, all the ions that are dissociated and present in the reaction mixture are represented while in the case of net ionic equation only the useful ions that participate in the reaction are represented.
The steps to write the complete ionic reaction are as follows:
Step 1: Write the molecular equation for the reaction with the phases in the bracket.
In the reaction, HI reacts with RbOH to form RbI and [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex]. The balanced molecular equation of the reaction is as follows:
[tex]{\text{HI}}\left( {aq} \right) + {\text{RbOH}}\left( {aq} \right) \to {\text{RbI}}\left( {aq} \right){\text{ + }}{{\text{H}}_{\text{2}}}{\text{O}}\left( l \right)[/tex]
Step 2: Dissociate all the compounds with the aqueous phase to write the complete ionic equation. The compounds with solid and liquid phase remain same. The complete ionic equation is as follows:
[tex]{{\mathbf{H}}^ + }\left( q \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right) + {\mathbf{O}}{{\mathbf{H}}^ - }\left( {aq} \right) \to {{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}\left( l \right) + {{\mathbf{I}}^ - }\left( {aq} \right) + {\mathbf{R}}{{\mathbf{b}}^ + }\left( {aq} \right)[/tex]
Learn more:
1. Balanced chemical equation https://brainly.com/question/1405182
2. Oxidation and reduction reaction https://brainly.com/question/2973661
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Chemical reaction and equation
Keywords: Double displacement reaction, types of equation, molecular equation, complete ionic equation, net ionic equation, RbI, RbOH, H2O, HI, chemical reaction.
To write a balanced complete ionic equation, first write the balanced chemical equation and then break it down into its ionic components. Finally, combine the ions to form the complete ionic equation.
Explanation:To write a balanced complete ionic equation for the reaction between HI(aq) and RBOH(aq), we need to first write the balanced chemical equation:
HI(aq) + RBOH(aq) -> HRB(aq) + H2O(l)
Now, we can break down the equation into its ionic components:
HI(aq) -> H+(aq) + I-(aq)
RBOH(aq) -> RB+(aq) + OH-(aq)
HRB(aq) -> H+(aq) + RB-(aq)
H2O(l)
Putting it all together, the balanced complete ionic equation is:
H+(aq) + I-(aq) + RB+(aq) + OH-(aq) -> H+(aq) + RB-(aq) + H2O(l)
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Which electron configuration represents the element carbon (atomic number 6)? A)1s2 2s2 2p6 B)1s2 2s2 2p4 C)1s2 2s2 2p2 D)1s2 2s2
Answers
C) 1s2 2s2 2p2
Explanation:
We are given that carbon has atomic number 6. This means that carbon has 6 electrons.
1- The first level is composed of only one sublevel (s sublevel) and can hold only two electrons. Therefore, the first two carbon electrons will occupy 1s2
2- The second level is composed of two sublevels (s sublevel and p sublevel). The s sublevel can hold only two electrons while the p sublevel can hold up to six electrons. Since only four carbon electrons are to occupy the second level; two of them will be in the s sublevel (2s2) while the other two will occupy the p sublevel (2p2)
Combining the above, we will find that the configuration of carbon is:
1s2 2s2 2p2
Hope this helps :)
Final answer:
The electron configuration that represents carbon (atomic number 6) is 1s²2s²2p², reflecting two unpaired electrons in the 2p orbitals according to Hund's rule. So the correct option is C.
Explanation:
The correct electron configuration that represents the element carbon (atomic number 6) is C) 1s²2s²2p². Carbon has six electrons, and the way these electrons are distributed in the atom's orbitals determines the electron configuration. The first two electrons fill the 1s orbital, the next two fill the 2s orbital, and the remaining two occupy the 2p orbitals. According to Hund's rule, these two 2p electrons are unpaired in two different, but degenerate, p orbitals, maximizing the number of unpaired electrons and adhering to the Pauli exclusion principle. Thus, the electron configuration for carbon with its valence shell is represented as ns²np², where n represents the principal quantum number relevant to the orbital.
Some common fossil fuels are gasonline,____, coal and natural gas
Answers
hope it helps :)
Which situation would be considered pseudoscience?
Students gather to identify species of plants in their neighborhood.
A student’s lucky necklace helps her win another volleyball tournament.
Students are successful in petitioning for organic food in the cafeteria.
A student tries eating all natural foods for one month to see if she has more energy.
Answers
How many molecules of o2 are contained in a gas tank that contains 650. g of oxygen?
Answers
These units could be atoms that make up an element, or molecules making up a compound or ions as well.
1 mol of O₂ contains - 6.022 x 10²³ molecules of O₂
molecular mass of O₂ is (16*2) = 32 g/mol
1 mol of O₂ weighs = 32 g
Therefore in 32 g of O₂ - 6.022 x 10²³ O₂ molecules
gas tank contains O₂ weighing 650 g
in 1 g - 6.022 x 10²³/32 molecules
in 650 g - 6.022 x 10²³/32 * 650
= 2.96 x 10²² molecules of O₂
You carefully weigh out 10.00 g of caco3 powder and add it to 40.50 g of hcl solution. you notice bubbles as a reaction takes place. you then weigh the resulting solution and find that it has a mass of 46.40 g . the relevant equation is caco3(s)+2hcl(aq)→h2o(l)+co2(g)+cacl2(aq) assuming no other reactions take place, what mass of co2 was produced in this reaction?
Answers
The law of conservation of mass saying that the mass can't be created or destroyed. That means the total weight of reactant should be equal to the total weight of the product. But, if the reaction creates a gas product, the gas produced could fly away and makes the product lighter. The mass of the CO2 that goes away in this reaction would be:
reactant=product
caco3 + HCL solution = CO2 + resulting solution
10g + 40.5g= CO2+ 46.4
CO2= 50.5g- 46.4g= 4.1g
The mass of CO₂ produced in the reaction is 4.10 grams.
To find the mass of CO₂ produced, we can use the law of conservation of mass, which states that mass is neither created nor destroyed in a chemical reaction.
The total mass of the reactants must equal the total mass of the products.
We start with the given masses of the reactants:
Mass of CaCO₃ = 10.00 g Mass of HCl solution = 40.50 g
The total mass of the reactants is the sum of the masses of CaCO₃ and the HCl solution:
Total mass of reactants = mass of CaCO₃ + mass of HCl solution Total mass of reactants = 10.00 g + 40.50 g Total mass of reactants = 50.50 g
After the reaction, we have the following:
Mass of the resulting solution = 46.40 g The mass of the products can be calculated by subtracting the mass of the reactants from the mass of the resulting solution: Mass of the products = Mass of the resulting solution - Mass of the reactants Mass of the products = 46.40 g - 50.50 g Mass of the products = -4.10 gThe negative sign indicates that 4.10 grams of gas (CO₂) have been released from the solution, as the mass of the products is less than the mass of the reactants.
This is consistent with the observed bubbles, which are CO₂ gas being produced and escaping from the solution.
Therefore, the mass of CO₂ produced is 4.10 grams.
the mass number of a chronium atom is 52 and it has 24 protons. how many neutrons does this atom have?
Answers
The answer is "28 neutrons".
Reason:
The element Chromium has:
Protons:24
Neutrons:28
Electrons:24
If you need anymore help feel free to ask me!
Hope this helps!
~Nonportrit
Calculate the ph of a buffer that is 0.225 m hc2h3o2 and 0.162 m kc2h3o2. the ka for hc2h3o2 is 1.8 Ã 10-5. 4.60 9.26 4.74 4.89 9.11
Answers
Answer:
The pH of the buffer solution is 4.60.
Explanation:
Concentration of acid = [tex][HC_2H_3O_2]=0.225 M[/tex]
Concentration of salt = [tex][KC_2H_3O_2]=0.162 M[/tex]
Dissociation constant = [tex] K_a=1.8 \times 10^{-5}[/tex]
The pH of the buffer can be determined by Henderson-Hasselbalch equation:
[tex]pH=pK_a+\log\frac{[salt]}{[acid]}[/tex]
[tex]pH=-\log[1.8 \times 10^{-5}]+\log\frac{0.162 M}{0.225 M}[/tex]
pH = 4.60
The pH of the buffer solution is 4.60.
4.602
Further explanationGiven:
A buffer system consisting of 0.225 M HC₂H₃O₂ and 0.162 M KC₂H₃O₂.
The Ka for HC₂H₃O₂ is 1.8 x 10⁻⁵.
Question:
Calculate the pH of this buffer.
The Process:
Let us first observe the ionization reaction of the KC₂H₃O₂ salt below.
[tex]\boxed{ \ KC_2H_3O_2 \rightleftharpoons K^+ + C_2H_3O_2^- \ }[/tex]
The KC₂H₃O₂ salt has valence = 1 according to the number of C₂H₃O₂⁻ ions as a weak part.HC₂H₃O₂ and C₂H₃O₂⁻ are conjugate acid-base pairsHC₂H₃O₂ and C₂H₃O₂⁻ form an acidic buffer system.To calculate the specific pH of a given buffer, we need using The Henderson-Hasselbalch equation for acidic buffers:
[tex]\boxed{ \ pH = pK_a + log\frac{[A^-]}{[HA]} \ }[/tex]
where,
Ka represents the dissociation constant for the weak acid; [A-] represent the concentration of the conjugate base (i.e. salt); [HA] is the concentration of the weak acid.[tex]\boxed{ \ pH = pK_a + log\frac{[C_2H_3O_2^-]}{[HC_2H_3O_2]} \ }[/tex]
[tex]\boxed{ \ pH = -log(1.8 \times 10^{-5}) + log\frac{[0.162]}{[0.225]} \ }[/tex]
[tex]\boxed{ \ pH = 5-log \ 1.8 - 0.1427 \ }[/tex]
[tex]\boxed{ \ pH = 5 - 0.2553 - 0.1427 \ }[/tex]
[tex]\boxed{ \ pH = 4.602 \ }[/tex]
Thus, the pH of this buffer equal to 4.602.
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Answers
Ultraviolet (UV) rays, is the right answer.
The sun emits rays in an extended spectrum of wavelengths, the maximum of which is not visible to human eyes. The shorter wavelength means that the radiation is more energetic and that it has the greater potential for harm. Therefore, the UV Rays that has a wavelength between 290 and 400 NM, have great potential for harm to humans. Sunburn, Suntan are some of the common impacts of over-exposure of humans to UV. Skin cancer is another disease caused by the UV Rays. Thus, the most harmful sun rays to the human being are the Ultraviolet Rays.
A student decomposed 3.67g of copper (ii) hydroxide into copper (ii) oxide. how many ml of 3m h2so4 is need to react with all the copper (ii) oxide?
Answers
Cu(OH)₂ (s) ----> CuO (s) + H₂O (l)
upon decomposition, water is removed from Cu(OH)₂
the amount of Cu(OH)₂ decomposed - 3.67 g
number of moles of Cu(OH)₂ - 3.67 g / 97.5 g/mol = 0.038 mol
stoichiometry of Cu(OH)₂ to CuO is 1:1
therefore number of CuO moles formed are - 0.038 mol
CuO reacts with sulfuric acid to form CuSO₄
CuO + H₂SO₄ ---> CuSO₄ + H₂O
stoichiometry of CuO to H₂SO₄ is 1:1
therefore number of H₂SO₄ moles that should react is 0.038 mol
the molarity of H₂SO₄ is 3M
this means that in 1000 ml - 3 mol of H₂SO₄ present
so if 3 mol are present in 1000 ml
then volume for 0.038 mol = 1000/3 * 0.038
= 12.67 ml
What mass of natural gas (ch4) must you burn to emit 269 kj of heat? ch4(g)+2o2(g)âco2(g)+2h2o(g)δhârxn=â802.3kj express the mass in grams to three significant figures?
Answers
The mass of natural gas (CH₄) you need to burn to emit 269 kJ of heat is 5.38 g, expressed to three significant figures.
The combustion of methane is an exothermic reaction, meaning that it releases heat. The heat of combustion of methane is -802.3 kJ/mol, which means that 802.3 kJ of heat are released when 1 mole of methane is burned.
We can use this information to calculate the mass of methane needed to release 269 kJ of heat.
Mass of CH₄ = Heat / Heat of combustion
= 269 kJ / (-802.3 kJ/mol)
= 0.334 mol
= 5.38 g
Therefore, you need to burn 5.38 grams of methane to emit 269 kJ of heat.
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The mass of natural gas (CH4) that must be burned to emit 269 kJ of heat is 5.42 grams.
Explanation:To calculate the mass of natural gas (CH4) that must be burned to emit 269 kJ of heat, we can use the enthalpy of combustion per mole of methane. According to the given balanced chemical equation, the enthalpy change of the combustion reaction is -802.3 kJ.
From a previous similar question, we know that when 2.50 g of methane burns, 125 kJ of heat is produced. So, we can set up a proportion to find the mass of CH4 that corresponds to 269 kJ of heat:
(2.50 g methane)/(125 kJ heat) = (x)/(269 kJ heat)
Solving for x, we find that x = 5.42 g. Therefore, the mass of natural gas that must be burned to emit 269 kJ of heat is 5.42 grams (to three significant figures).
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Josh decided to mix some vinegar with baking soda. He knew that a reaction occurred because he made careful observations. He noted that the mixture started to foam up and bubble and was white in color. How did Josh know that a chemical reaction occured? He was sure a reaction occurred because of
A) the formation of a gas.
B) the color of the mixture.
C) the smell of the vinegar.
D) the volume of the mixture.
Answers
Hope this helps
~ Jordan ~
Answer: its A
Explanation: i did the test myself so i know its A
K12 3.10 Unit Assessment: Solutions, Part 1 does anyone have the answers for this quiz
Answers
The student is not provided with the direct answers to their K12 3.10 Unit Assessment (Chemistry). Instead, they are advised to review key concepts and principles from the unit, apply them to different contexts during the assessment, and utilise computational and analytical skills.
Explanation:While it's not appropriate to provide the direct answers to your K12 3.10 Unit Assessment: Solutions, Part 1, I can help you understand how to arrive at correct solutions. The assessment likely includes both multiple-choice and short-response questions from various topics you've studied during the unit.
Critical Thinking Questions usually require you to apply concepts and principles you've learned to different contexts or situations. You might have to use analytic and computational skills to solve some problems. For instance, an example of a chemistry AP question could be asking you to calculate molarity of a solution, given the mass of the solute and volume of the solution.
Finally, review the materials from your textbooks and lessons, particularly the areas you feel less confident about. Practice using the concept to solve problems and try to understand the underlying principles. Good luck with your assessment!
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A neutral atom of which of the four element has the smallest radius
Answers
Element 1
Explanation:
The ionization energy is defined as the energy required to remove electrons from the atoms.
We know that the nucleus of the atom attracts the electrons, thus, bound these electrons to the atom.
This means that as the radius decreases, the force of attraction between the nucleus and the electron will increase, therefore, the energy required to remove the electron would increase (and vice-versa).
Based on the above, the atom with the smallest radius would be the atom with the largest first ionization energy.
Hope this help :)
A sample of an ideal gas has a volume of 2.31 l at 287 k and 1.10 atm. calculate the pressure when the volume is 1.45 l and the temperature is 298 k.
Answers
The pressure of the Ideal Gas when the volume is 1,45 L and the temperature is 298 K is 1,82 atm.
To solve this problem we need to apply the Ideal Gas Law for the initial conditions and the final ones, clearing the equation for the number of moles (n) and the ideal gas constant (R) which remain constant:
[tex]P_n*V_n=n*R*T_n \\ \\ n*R= \frac{P_n*V_n}{T_n} [/tex]
Now we match n*R for the initial conditions (1) and the final ones (2), clearing the equation for P₂
[tex] \frac{P_1*V_1}{T_1}= \frac{P_2*V_2}{T_2} \\ \\ P_2= \frac{P_1*V_1*T_2}{T_1*V_2}= \frac{1,10 atm*2,31 L *298 K}{287K*1,45 L}=1,82 atm [/tex]
Have a nice day!
Final answer:
To calculate the new pressure of an ideal gas when the volume decreases to 1.45 L and the temperature increases to 298 K, the combined gas law is used. The final pressure is found to be approximately 1.803 atm after substituting the given initial conditions and solving for the final pressure.
Explanation:
The question relates to the behavior of an ideal gas when it undergoes changes in volume, pressure, and temperature. To solve for the new pressure when the volume and temperature of a gas sample change, we use the combined gas law, which states that the ratio of the product of pressure and volume to the temperature is constant for a fixed amount of gas (P₁ * V₁) / T₁ = (P₂ * V₂) / T₂).
Given:
P₁ = 1.10 atm
V₁ = 2.31 L
T₁ = 287 K
V₂ = 1.45 L
T₂ = 298 K
We need to find the final pressure P₂.
To find the final pressure P2, we rearrange the combined gas law equation:
P₂ = (P₁ * V₁ * T₂) / (V₂ * T₁)
Now we plug in the known values:
P₂ = (1.10 atm * 2.31 L * 298 K) / (1.45 L * 287 K)
P₂ = (750.38 atm*L*K) / (416.15 L*K)
P₂ = 1.803 atm (rounded to three significant figures)
The final pressure of the gas when the volume is 1.45 L and the temperature is 298 K is approximately 1.803 atm.
What is the expected oxidation state for the most common ion of element 2
Answers
Justification:
The ionization energies tell the amount of energy needed to release an electron and form a ion. The first ionization energy if to loose one electron and form the ion with oxidation state 1+, the second ionization energy is the energy to loose a second electron and form the ion with oxidation state 2+, the third ionization energy is the energy to loose a third electron and form the ion with oxidation state 3+.
The low first ionization energy of element 2 shows it will lose an electron relatively easily to form the ion with oxidations state 1+.
The relatively high second ionization energy (and third too) shows that it is very difficult for this atom to loose a second electron, so it will not form an ions with oxidation state 2+. Furthermore, given the relatively high second and third ionization energies, you should think that the oxidation states 2+ and 3+ for element 2 never occurs.
Therefore, the expected oxidation state for the most common ion of element 2 is 1+.
The most common ion of helium (element 2), which rarely forms, has an expected oxidation state of 0 due to helium's full valence electron shell and its nature as a noble gas.
The expected oxidation state for the most common ion of element 2, which is helium (He), is 0. Because helium is a noble gas, it rarely forms ions and typically remains unreactive due to its full valence electron shell. Therefore, the oxidation number of any noble gas in its elemental state, including helium, is 0.
Given the reaction: HSO4– + HPO42– ↔ SO42– + H2PO4-Which pair represents an acid and its conjugate base?
A) HSO4- and HPO42-
B) SO42- and H2PO4-
C) HSO4- and SO42-
D) SO42- and HPO42-
Answers
The pair which represents an acid and its conjugate base is HSO₄⁻ and SO₄⁻².
To know if a pair of substances represents an acid and its conjugate base, one should look at the chemical structure of each substance. The conjugate base of an acid has usually the same chemical formula than the acid, but with one less proton (H⁺). Of the pairs of substances on the list, only HSO₄⁻ and SO₄⁻² have similar structures, with the only difference being the number of protons. The chemical reaction of dissociation of HSO₄⁻ is the following:
HSO₄⁻ + H₂O ⇄ SO₄⁻² + H₃O⁺
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Calculate the vapor pressure at 50°c of a coolant solution that is 52.0:48.0 ethylene glycol-to-water by volume. at 50.0°c, the density of water is 0.9880 g/ml, and its vapor pressure is 92 torr. the vapor pressure of ethylene glycol is less than 1 torr at 50.0°c.
Answers
V(ethylene glycol - C₂H₆O₂) = 0,52 · 100 mL = 52 mL.
V(water) = 0,48 · 100 mL = 48 mL.
m(C₂H₆O₂) = 52 mL · 1,115 g/mL = 57,98 g.
n(C₂H₆O₂) = 57,98 g ÷ 62,07 g/mol = 0,934 mol.
m(H₂O) = 48 mL · 0,988 g/mL = 47,424 g.
n(H₂O) = 45,45 g ÷ 18 g/mol = 2,635 mol.
mole fraction of solvent: 2,635 mol / (2,635 mol + 0,934 mol) =0,73.
Raoult's Law: p(solution) = mole fraction of solvent · p(solvent).
p(solution) = 0,73 · 92 torr = 67,33 torr.
The combustion of 987.0 g of methane in the presence of excess oxygen produces 1.543 kg of carbon dioxide. What is the percent yield
Answers
Chemical reaction: CH₄ + 2O₂ → CO₂ + 2H₂O.
m(CH₄) = 987 g.
n(CH₄) = m(CH₄) ÷ M(CH₄).
n(CH₄) = 987 g ÷ 16 g/mol.
n(CH₄) = 61,68 mol.
From reaction: n(CH₄) : n(CO₂) = 1 : 1.
n(CO₂) = 61,68 mol.
m(CO₂) = 61,68 mol · 44 g/mol.
m(CO₂) = 2714,25 g ÷ 1000 g/kg = 2,714 kg.
yield = 1,543 kg ÷ 2,714 kg · 100 % = 56,85%.
Which of these collectively come under van der Waals forces?
Answers
London Dispersion forces, Hydrogen bonding and Dipole=dipole
interactions (otherwise known as permanent dipole- permanent dipole interactions)
Hoped this helped buddy!
Answer:
London dispersion forces and dipole-dipole interactions
Explanation:
Hello,
There are two intermolecular forces that are collectively referred to as Van der Waals Forces: London dispersion forces and dipole-dipole interactions.
London dispersion forces are the weakest intermolecular forces. They are temporary attractive forces that turn out when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles.
On the other hand, dipole-dipole interactions turn out when two dipolar molecules interact with each other through the containing space. In such a way, the partially negative portion of one of the polar molecules is attracted to the partially positive portion of the second polar molecule.
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Consider an amphoteric hydroxide, m(oh)2(s), where m is a generic metal. estimate the solubility of m(oh)2 in a solution buffered at ph
Answers
from this balanced equation:
M(OH)2(s) ↔ M2+(aq) + 2OH-(aq) and when we have Ksp = 2x10^-16
∴Ksp = [M2+][OH]^2
2x10^-16 = [M2+][OH]^2
a) SO at PH = 7
∴POH = 14-PH = 14- 7 = 7
when POH = -㏒[OH]
7= -㏒[OH]
∴[OH] = 1x10^-7 m by substitution with this value in the Ksp formula,
∴[M2+] =Ksp /[OH]^2
= (2x10^-16)/(1x10^-7)^2
= 0.02 M
b) at PH =10
when POH = 14- PH = 14-10 = 4
when POH = -㏒[OH-]
4 = -㏒[OH-]
∴[OH] = 1x10^-4 ,by substitution with this value in the Ksp formula
[M2+] = Ksp/ [OH]^2
= 2x10^-16 / (1x10^-4)^2
= 2x10^-8 M
c) at PH= 14
when POH = 14-PH
= 14 - 14
= 0
when POH = -㏒[OH]
0 = - ㏒[OH]
∴[OH] = 1 m
by substitution with this value in Ksp formula :
[M2+] = Ksp / [OH]^2
= (2x10^-16) / 1^2
= 2x10^-16 M
The solubility of an amphoteric hydroxide in a buffered solution depends on the pH of the solution. It can act as both an acid and a base. The Henderson-Hasselbalch equation can be used to estimate the solubility in a buffered solution.
Explanation:The solubility of an amphoteric hydroxide, M(OH)2, in a buffered solution depends on the pH of the solution. An amphoteric hydroxide can act as both an acid and a base. At low pH, the hydroxide ion concentration is low and the hydroxide ion reacts with the excess hydronium ions, reducing the solubility. At high pH, the hydronium ion concentration is low and the hydroxide ion concentration is high, increasing the solubility. In a buffered solution, the pH remains relatively constant due to the presence of a weak acid and its conjugate base. The solubility of the hydroxide in the buffered solution can be estimated using the Henderson-Hasselbalch equation.
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(r)-2-butanol reacts with potassium dichromate (k2cro4) in aqueous sulfuric acid to give a (c4h8o). treatment of a with sodium borohydride in ethanol gives b, which as the same boiling point and refractive index as (r)-2-butanol. draw the structure of
b.
Answers
Final answer:
The structure of compound B is 2-methyl-2-butanol, which is formed by the reduction of the carbonyl group of (R)-2-butanol. This reduction reaction converts the aldehyde group into a secondary alcohol group.
Explanation:
The structure of compound B, which has the same boiling point and refractive index as (R)-2-butanol, can be drawn as 2-methyl-2-butanol. The reaction of (R)-2-butanol with sodium borohydride in ethanol leads to the reduction of the carbonyl group of (R)-2-butanol, resulting in the formation of 2-methyl-2-butanol (compound B). This reduction reaction converts the aldehyde group of (R)-2-butanol into a secondary alcohol group.