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2 years ago

Which example best demonstrates stewardship of the atmosphere

Chemistry

1 answer:

Margarita [4]2 years ago

3 0

Incomplete question. However, I provided a specific example of stewardship of the atmosphere.

Explanation:

First, note that the term stewardship refers to the belief that humans are obligated to take care and look after our environment (which includes the atmosphere.

An example of this is: deciding to change our mode of transportation: What this entails is that we may decide to switch to riding a bicycle to places rather than going by car. By so doing you will be reducing the number of greenhouse gases emitted into the environment as bicycles do not emit harmful gases when used.

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Barium oxalate is used as a colorant to produce the green color in fireworks. Imagine that you have been assigned to prepare bar

JulsSmile [24]

Answer:

2.1

Explanation:

Calculation of moles of $Ba(OH)_2.8H_2O$

Mass of copper = 5.3 g

Molar mass of copper = 315.46 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{5.3\ g}{315.46\ g/mol}$

Moles of $Ba(OH)_2.8H_2O$ = 0.0168 moles

According to the reaction,

$Ba(OH)_2.8H_2O + H_2C_2O_4.2H_2O\rightarrow BaC_2O_4 + 12 H_2O$

1 mole of $Ba(OH)_2.8H_2O$ react with 1 mole of $H_2C_2O_4.2H_2O$

0.0168 moles of $Ba(OH)_2.8H_2O$ react with 0.0168 moles of $H_2C_2O_4.2H_2O$

Moles of $H_2C_2O_4.2H_2O$ = 0.0168 moles

Molar mass of $H_2C_2O_4.2H_2O$ = 126.07 g/mol

Thus,

Mass = Moles * Molar mass = 0.0168 moles * 126.07 g/mol = 2.1 g

Answer - 2.1

5 0

2 years ago

A large flask is evacuated and weighed, filled with argon gas, and then reweighed. When reweighed, the flask is found to have ga

Elden [556K]

Answer:

100.52

Explanation:

from the ideal gas equation PV=nRT

for a given container filled with any ideal gas P and V remains constant.So T is also constant.R is as such a constant.

So n i.e no of moles will also be constant.

no of moles of Ar=3.224/40=0.0806

no of moles of unknown gas=0.0806

molecular wt of unknown gas=8.102/0.0806=100.52

8 0

2 years ago

50cm3 of sodium hydroxide solution was titrated against a solution of sulfuric acid. The concentration of the sodium hydroxide s

miskamm [114]

Answer:

49 g/L is the concentration of the acid

Explanation:

Firstly, we proceed to write the equation of reaction.

2NaOH + H2SO4 ——-> Na2SO4 + 2H2O

We can see that 1 mole of the base reacted with two moles of the acid.

kindly note that dm^3 is same as liter

Firstly, we need to get the concentration of the reacted sulphuric acid in g/L

we use the simple titration equation below;

CaVa/CbVb = Na/Nb

From the question;

Ca = ?

Va = 25 cm^3

Cb = 20 g/L

we convert this to concentration in mol/L

Mathematically, that is concentration in g/L divided by molar mass in g/mole

molar mass of NaOH = 40 g/mol

so we have; 20g/L / 40 = 0.5 mol/L

Vb = 50 cm^3

Na = 1

Nb = 2

Where C represents concentrations, V volumes and N , number of moles

Now, substitute the values;

Ca * 25/0.5 * 50 = 1/2

25Ca/25 = 0.5

So Ca = 0.5 mol/L

Now to get the concentration of H2SO4 in g/L

What we do is to multiply the concentration in mol/L by molar mass in g/mol

That would be 0.5 * 98 = 49 g/L

4 0

2 years ago

2.1. The lithium ion in a 250,00 mL sample of mineral water was

juin [17]

Answer:

11482 ppt of Li

Explanation:

The lithium is extracted by precipitation with B(C₆H₄)₄. That means moles of Lithium = Moles B(C₆H₄)₄. Now, 1 mole of B(C₆H₄)₄ produce the liberation of 4 moles of EDTA. The reaction of EDTA with Mg²⁺ is 1:1. Thus, mass of lithium ion is:

Moles Mg²⁺:

0.02964L * (0.05581mol / L) = 0.00165 moles Mg²⁺ = moles EDTA

Moles B(C₆H₄)₄ = Moles Lithium:

0.00165 moles EDTA * (1mol B(C₆H₄)₄ / 4mol EDTA) = 4.1355x10⁻⁴ mol B(C₆H₄)₄ = Moles Lithium

That means mass of lithium is (Molar mass Li=6.941g/mol):

4.1355x10⁻⁴ moles Lithium * (6.941g/mol) = 0.00287g. In μg:

0.00287g * (1000000μg / g) = 2870μg of Li

As ppt is μg of solute / Liter of solution, ppt of the solution is:

2870μg of Li / 0.250L =

4 0

1 year ago

An increase in temperature will effect vapor pressure by:

-BARSIC- [3]

Answer: Increases.

Explanation: As the temperature of a liquid or solid increases its vapor pressure also increases. Conversely, vapor pressure decreases as the temperature decreases.

5 0

1 year ago