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3 years ago

What is the relationship between atomic size and bond length for H2O / H2S and CO2 / CS2?

1 answer:

4 0

H2O bond length is 95.84 pm while H2S bond length is 133.6 pm. The atomic size and bond length for H2O is less than that of H2S. Co2 bond length is 116.3 pm while CS2 bond length is 155.3 pm.

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A 0.69-g sample of lime (CaO) is dissolved in enough water to make 1535 mL of solution. Calculate the pH of of the solution.

Marizza181 [45]

Answer:

pH = 12.2

Explanation:

Given data:

Mass of lime = 0.69 g

Volume = 1535 mL (1535 / 1000 = 1.535 L)

pH of solution = ?

Solution:

First of all we will determine the molarity.

Molarity = moles of solute / volume in litter

Number of moles = mass / molar mass

Number of moles = 0.69 g / 56.1 g/mol

Number of moles = 0.0123 mol

Molarity = moles of solute / volume in litter

Molarity = 0.0123 mol / 1.535 L

Molarity = 0.008 M

One mole of CaO neutralize two mole of OH⁻.

0.008 M×2 = 0.016 M

[OH⁻] = 0.016 M

pOH = -log [OH⁻]

pOH = [0.016]

pOH = 1.8

14 = pH +pOH

pH = 14 - pOH

pH = 14-1.8

pH = 12.2

4 0

3 years ago

A sample taken from a layer of mica in a canyon has 2.10 grams of potassium-40. A test reveals it to be 2.6 billion years old. H

Setler79 [48]

Problem One

Formula

N(t) = No * (1/2)^[t/t_1/2]

Givens

N(t) = the current mass of the sample = 2.10 grams

No = The original mass of the sample = No [We're trying to find this].

t = time elapsed which is 2.6 billion years or 2.6 * 10^9 years.

t1/2 = the 1/2 life time which is 1.3 billion years of 1.3 *10^9

Solution

2.10 grams = No (1/2)^(2.6*10^9/1.3 * 10^9)

The 10^9s cancel and you are left with 2.6/1.3 = 2

2.10 grams = No (1/2)^2

2.10 grams = No (1/4) Multiply both sides by 4

2.10 * 4 = No (1/4)*4

8.4 grams = No

which is how many grams you originally had.

Answer B.

Problem Two

$_{1}^{2}\text{H} + _{1}^{2}\text{H} \longrightarrow _{z}^{y}\text{x}+_{0}^{1}\text{n}$

Solve for y

2 + 2 = y + 1

4 = y + 1

y = 3

Solve for z

1 + 1 = z + 0

z = 2

The 2 tells you that it is the second member on the periodic table. That's Helium. So the answer looks like this.

$_{2}^{3}\text{He}$

The mass of the Helium is 3 and its number is two.

5 0

3 years ago

A key step in the extraction of iron from its ore isFeO(s) + CO(g) ⇄ Fe(s) + CO₂(g) Kp = 0.403 at 1000°CThis step occurs in the

Kisachek [45]

A key step in the extraction of iron from its ore isFeO(s) + CO(g) ⇄ Fe(s) + CO₂(g) Kp = 0.403 at 1000°CThis step occurs in the 700°C to 1200°C zone within a blast furnace. the partial pressure of CO2 at equilibrium is 1.58 atm.

The complete reaction of the problem, for better illustration, is

FeO(s) + CO(g) <--> Fe(s) + CO2(g)

The double-tailed arrow signifies that the reaction is in a dynamic chemical equilibrium. When the system is in equilibrium, the forward and the backward reaction rates have an equal ratio of Kp = 0.403 at 1000°C. The formula for Kp is

Kp = [partial pressure of products]/[partial pressure of reactants]

So, first, let's find the partial pressure of the compounds in the reaction.

FeO(s) + CO(g) <--> Fe(s) + CO2(g)

Initial x 1.58 0 0

Change -1.58 -1.58 +1.58 +1.58

------------------------------------------------------------------

Equilbrium x-1.58 0 1.58 1.58

Kp = [(1.58)(1.58)]/[(x-1.58)] = 0.403

x = 7.77 atm (this is the amount of excess FeO)

Therefore, the partial pressure of CO2 at equilibrium is 1.58 atm. There is no more CO because it has been consumed due to excess FeO.

To know more about partial pressure of CO2 at equilibrium

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6 0

2 years ago

Helppp its qboutt cellsss

fredd [130]

Answer:

sorry if this is wrong but B

Explanation:

3 0

3 years ago

Sulfuric acid, H 2 S O 4 , is an important industrial chemical, typically synthesized in a multi-step process. What is the perce

STatiana [176]

Answer:

71.8%

Explanation:

The percent yield of a process or a chemical reaction is calculated as:

percent yield = actual yield/theoretical yield x 100%

From the problem we have:

theoretical yield = 3.9 kg

actual yield = 2.8 kg

Thus, we calculate the yield of H₂SO₄ production as follows:

percent yield = (2.8 kg/3.9 kg) x 100 = 71.79 % ≅ 71.8%

3 0

3 years ago