An electrochemical cell is powered by the half reactions shown below.

Ag+(aq) + e–  Ag(s)        Eo = +0.80 V
Pb2+(aq)  + 2e–  Pb(s)        Eo = –0.13 V

Which value represents the overall electric cell potential?
Use Ecell =  Ered, cathode – Ered, anode.

–0.13 V

–0.93 V

+0.67 V

+0.93 V

To find the density of sulfur dioxide (SO2) at 1.2 atmospheres and 271 Kelvin, we can use the ideal gas law equation. We need to know the molar mass of sulfur dioxide, which is 64.06 g/mol. Using the ideal gas law equation, we can calculate the volume of SO2 and find the density.

To find the density of sulfur dioxide (SO2) at 1.2 atmospheres and 271 Kelvin, we can use the ideal gas law equation:

density = (mass of SO2) / (volume of SO2)

We need to know the molar mass of sulfur dioxide, which is 64.06 g/mol. We also need to convert the given pressure to Pascals (Pa) and temperature to Kelvin (K).

Using the ideal gas law equation, we can calculate the volume of SO2:

volume of SO2 = (mass of SO2) / (density)

Finally, we substitute the given values into the equation to find the density:

density = mass of SO2 / volume of SO2

The concentration of the acid is the same as that of the base.

If equal volumes of acid and base are required, you can conclude that the concentrations must be the same.

they showed mandeleeves predictions were correct

Actually there are three established rules on counting how many significant figures are in a number:

Rule 1: Positive integers are always significant.

Rule 2: Any zeros between two significant digits are always significant.

Rule 3: A final zero or trailing zeros after the decimal point are always significant.

Since the given number is 10.0010 g, the two 1’s is under Rule 1, the three 0’s between the two 1’s is under Rule 2, and the zero after the last 1 is under Rule 3. Therefore all the digits are significant.

Answer: So the number of significant figures in the measurement is 6.

To calculate the atoms of an element in a given molecule, we need to multiply stoichiometry by the number that is written on the foot of that element. Therefore, the mass of  AgCl produced from 75.00 g of AgNO[tex]_3[/tex]. is 63.0g.

Stoichiometry is a part of chemistry that help us in making relationship between reactant and product from quantitative aspects.

The balanced reaction is  

NaCl + AgNO[tex]_3[/tex] → NaNO[tex]_3[/tex] + AgCl

Mass of AgNO[tex]_3[/tex]=75.00 g

Molar mass of AgNO[tex]_3[/tex]=169.87 g/mol

Moles of AgNO[tex]_3[/tex]=0.44mol

From 1 mole of  AgNO[tex]_3[/tex], 1 mole of  AgCl is produced.

So, from 0.44 of AgNO[tex]_3[/tex], 0.44 mole of AgCl  is produced.

Mass of AgCl =Molar mass of AgCl ×moles of AgCl

Mass of AgCl =143.32 g/mol  ×0.44 mole

Mass of AgCl =143.32 g/mol  ×0.44 mole

Mass of AgCl =63.0g

Therefore, the mass of  AgCl produced from 75.00 g of AgNO[tex]_3[/tex]. is 63.0g.

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Answer:

6

Explanation:

The Lewis structure represents the valence electrons at the atoms, which ones are shared and the lone pairs. Carbon is at group 4 at the periodic table, and so has 4 electrons in the valence shell; oxygen is at group 6, and so has 6 electrons at the valence shell.

That compound is an exception of the octet rule. A triple bond is done between the atoms, and so, 3 electrons of carbon are shared and 3 electrons of oxygen are shared. Thus, there are 6 bonding electrons, as shown below in red.

In this problem, we can formulate two equations.

First, the overall mass balance of the ointment. The mass of 30% salicylic acid ointment plus the mass of petrolatum must be 50 grams.

x + p = 50

Where x is the mass of 30% salicylic acid ointment and p is the mass of petrolatum

Second, the component mass balance of salicylic acid:

0.3 * x = 50 * 0.05

x = 8.33 g

Therefore the mass of petrolatum to be used is:

x + p = 50

p = 50 – x

p = 50 – 8.33

p = 41.67 g

Answer:

41.7

Answer: Option (c) is the correct answer.

Explanation:

When [tex]Al(NO_{3})_{3}[/tex] reacts with CaO then it results in the formation of aluminium oxide and calcium nitrate.

The chemical reaction equation will be as follows.

[tex]2Al(NO_{3})_{3} + 3CaO \rightarrow Al_{2}O_{3} + 3Ca(NO_{3})_{2}[/tex]

Thus, we can conclude that out of the given options [tex]Al_{2}O_{3}[/tex] is one of the products produced when [tex]Al(NO_{3})_{3}[/tex] and CaO react together.

Answer: The volume of water that must be added will be 1.417 L.

Explanation:

Concentration of a substance is defined as mass of solute (in grams) present in the given volume of a solution (in L).

The equation representing concentration is given as:

[tex]\text{Concentration of solute}=\frac{\text{Mass of solute}}{\text{Volume of solvent}}[/tex]

We are given:

Concentration = 3.81 g/L

Mass of sodium nitrate = 5.40 g

Putting values in above equation, we get:

[tex]3.81g/L=\frac{5.40g}{\text{Volume of water}}\\\\\text{Volume of water}=1.417L[/tex]

Hence, the volume of water that must be added will be 1.417 L.

The molar solubility of BaF2 in pure water is approximately 6.13 x 10⁻⁶ M.

The molar solubility of BaF2 in pure water can be calculated using the solubility product constant (Ksp) of BaF2. The equation for the dissolution of BaF2 is BaF2 → Ba²+ + 2F¯. The Ksp expression for BaF2 is Ksp = [Ba²+][F¯]². Since there is a 1:2 stoichiometric relationship between BaF2 and fluoride ions in solution, the molar solubility of BaF2 can be represented as x, which gives the concentrations of Ba²+ and F¯ as x and 2x, respectively. Substituting these values into the Ksp expression, we get:

Ksp = (x)(2x)² = 4x³ = 2.45 x 10⁻⁵

Solving for x, we find that the molar solubility of BaF2 in pure water is approximately 6.13 x 10⁻⁶ M.

To find the number of chlorine atoms in 5.0 g of chloral hydrate, calculate the moles of chloral hydrate and then use Avogadro's number to find the atoms. There are approximately 5.46 x 10²² chlorine atoms in 5.0 g of chloral hydrate.

The question asks us to determine the number of chlorine atoms in 5.0 g of chloral hydrate. To find this, we need the molar mass of chloral hydrate (C₂H₃Cl₃O₂) and the molar mass of chlorine. The atomic mass of chlorine is 35.45 u. Chloral hydrate contains three chlorine atoms per molecule.

First, calculate the molar mass of chloral hydrate:

Total molar mass = 165.394 u.

Next, we calculate the amount (in moles) of chloral hydrate:

5.0 g / 165.394 g/mol = 0.0302 mol. Since each molecule of chloral hydrate contains three chlorine atoms, we multiply the number of moles by Avogadro's number (6.022 x 10²³ atoms/mol) and then by three:

0.0302 mol x 3 x 6.022 x 10²³ atoms/mol = 5.46 x 10²²  chlorine atoms.

Therefore, there are approximately 5.46 x 10²² chlorine atoms in 5.0 g of chloral hydrate.

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Final answer:

To produce 30.6 moles of water vapor from the reaction of hydrogen gas with excess carbon dioxide, 30.6 moles of hydrogen gas are required according to the balanced chemical equation with a 1:1 molar ratio of hydrogen to water.

Explanation:

To determine how many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 30.6 moles of water vapor, we need the balanced chemical equation for the reaction between hydrogen gas (H2) and carbon dioxide (CO2) to produce water (H2O) and carbon monoxide (CO).

To determine the number of moles of hydrogen gas needed to react with excess carbon dioxide to produce 30.6 moles of water vapor, we need to use the balanced chemical equation for the reaction.

The balanced equation is:

2H2(g) + CO2(g) -> 2H2O(g)

From the equation, we can see that 2 moles of hydrogen gas react with 1 mole of carbon dioxide to produce 2 moles of water vapor. Therefore, the ratio of hydrogen gas to water vapor is 2:2.

Since we are given that 30.6 moles of water vapor are produced, we can calculate the moles of hydrogen gas as:

(30.6 moles of water vapor) x (2 moles of hydrogen gas / 2 moles of water vapor) = 30.6 moles

Therefore, 30.6 moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 30.6 moles of water vapor.

H2(g) + CO2(g) → H2O(g) + CO(g)

From the balanced equation, we see that the molar ratio of hydrogen gas to water vapor is 1:1. Therefore, to produce 30.6 moles of water vapor, 30.6 moles of hydrogen gas are needed:

30.6 moles H2O × 1 mole H2/1 mole H2O = 30.6 moles H2

Thus, 30.6 moles of hydrogen gas are required to react with excess carbon dioxide to produce 30.6 moles of water vapour.

Ten molecules of water are required to completely hydrolyze a polymer of 11 monomers.

A polymer can be described as a macromolecule which essentially is a combination of many subunits. From Polypropylene which is used widely around the world as plastic to the strand of our DNA, which is a naturally occurring biopolymer.

Polymers can be naturally found in plants and animals called natural polymers or can be man-made called synthetic polymers. Different types of polymers posses different physical and chemical properties.

Semisynthetic polymers are those which can be derived from naturally occurring polymers and can undergo further modification such as cellulose nitrate, and cellulose acetate.

Polymers can be broken down into monomers is called hydrolysis of polymer, which is a reaction in which a water molecule is utilized during the breakdown.

Given polymer has 11 monomers which are connected with each other through 10 bond links that can be broken by ten water molecules.

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B. mass being converted to energy when protons and neutrons bind together in a nucleus

An alpha emission is one in which an atomic nucleus emits an alpha particle (helium nucleus). Therefore in this reaction, the products of the decay are Helium and another element X. Helium has an atomic mass and atomic number of 4 and 2 respectively, therefore the complete reaction is:

U-234 (92) ---> He-4 (2) + X

Since atomic mass and number must be conserved therefore X = X-230 (90)

U-234 (92) ---> He-4 (2) + X-230 (90)

The element with atomic number of 90 is Thorium. Therefore the other product is Thorium-230 (90).

U-234 (92) ---> He-4 (2) + Th-230 (90)