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Marina86 [1]
3 years ago
6

If this element loses

Chemistry
1 answer:
Lorico [155]3 years ago
7 0

Answer:

KEDal

Explanation:

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What steps have power plants taken to reduce the amount of sulfur oxides released into the air?
Ann [662]
Emissions of SO2 generated during the combustion of fossil fuels can be reduced<span> by treating the flue gases before they are emitted into the atmosphere via the stack; this is termed Flue Gas Desulphurisation (FGD). Flue gas desulphurisation systems can be classified as either Regenerable or Non-regenerable.

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5 0
3 years ago
A chemist must dilute of aqueous potassium dichromate solution until the concentration falls to . He'll do this by adding distil
Phantasy [73]

The question is incomplete; the complete question is;

A chemist must dilute 99.4 mL of 152 mM aqueous potassium dichromate (K_2Cr_2O_7) solution until the concentration falls to 55.0 mM He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Be sure your answer has the correct number of significant digits.

Answer:

0.275 L

Explanation:

From C1V1 = C2V2

Where;

C1= initial concentration of the solution 152 × 10^-3 M

V1= initial volume of the solution = 99.4 × 10^-3 L

C2 = concentration after dilution = 55 × 10^-3 M

V2 = volume after dilution = the unknown

V2 = C1 V1/C2

V2 = 152 × 10^-3 × 99.4 × 10^-3 / 55 × 10^-3

V2 = 0.275 L

5 0
3 years ago
What happens when the pressure of a gas is decreased?
Serggg [28]

Answer:

The combined gas law states that the pressure of a gas is inversely related to the volume and directly related to the temperature. If temperature is held constant, the equation is reduced to Boyle's law. Therefore, if you decrease the pressure of a fixed amount of gas, its volume will increase.

Explanation:

3 0
3 years ago
Calcium oxide or quicklime (CaO) is used in steelmaking, cement manufacture, and pollution control. It is prepared by the therma
Elena-2011 [213]

Answer:

The yearly release of CO_2 into the atmosphere is 6.73\times 10^{10} kg.

Explanation:

CaCO_3(s)\rightarrow CaO(s) + CO_2(g)

Annual production of CaO = 8.6\times 10^{10} kg=8.6\times 10^{13} g

Moles of CaO :

\frac{8.6\times 10^{13} g}{56 g/mol}=1.53\times 10^{12} moles

According to reaction, 1 mole of CaO is produced along with 1 mole of carbon-dioxide.

Then along with  1.53\times 10^{12} moles of CaO moles of carbon-dioxide moles produced will be:

\frac{1}{1}\times 1.53\times 10^{12} moles=1.53\times 10^{12} moles of carbon-dioxide

Mass of 1.53\times 10^{12} moles of carbon-dioxide:

1.53\times 10^{12}mol\times 44 g/mol=6.73\times 10^{13} g =6.73\times 10^{10} kg

The yearly release of CO_2 into the atmosphere is 6.73\times 10^{10} kg.

6 0
3 years ago
Assume that you take 0.46 mol of KBr and do some chemistry on it such that all of the potassium and bromine are separated. How m
erastovalidia [21]

Answer:

We'll have 13.85 grams of potassium

Explanation:

Step 1: Data given

Moles KBr = 0.46 mol

Molar mass KBr = 119.00 g/mol

Molar mass K = 30.10 g/mol

Step 2: The balanced equation

2KBr ⇆ 2K + Br2

Step 3: Calculate moles of K

For 2 moles KBr consumed we'll have 2 moles K and 1 mol Br2

For 0.46 moles KBr we'll have 0.46 moles K

Step 4: Calculate mass of K

Mass K = moles K * molar mass K

Mass K = 0.46 moles * 30.10 g/mol

Mass K = 13.85 grams

We'll have 13.85 grams of potassium

3 0
4 years ago
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