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2 years ago

The annual production of sulfur dioxide from burning coal, fossil fuels,

Chemistry

1 answer:

Citrus2011 [14]2 years ago

5 0

Answer:

1150g

Explanation:

The equation for producing sulphur dioxide is $S + O_{2} ==> SO_{2}$

Looking at the ratios, you need 1 mole of sulphur for every 1 mole of sulphur dioxide

Sulphur dioxide has a molar mass of 32 + (2 x 16) = 64g

2.30 x 1000 = 2300

2300 / 64 = 35.9375

35.9375 x 32 = 1150g of sulphur

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Write a balanced nuclear equation for the following: The nuclide astatine-218 undergoes alpha emission to give bismuth-214

galina1969 [7]

Answer:

$^{218}_{85}At\rightarrow ^{214}_{83}Bi+^{4}_{2}He$

Explanation:

Hello there!

In this case, since the radioactive reaction for the alpha emission of astatine-218 to bismith-214 involve the release of a helium atom as shown below:

$^{218}_{85}At\rightarrow ^{214}_{83}Bi+^{4}_{2}He$

Whereas the atomic number decreases by 2 and the mass number by 4 in agreement to the release of the Helium atom.

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2 years ago

Gold can be found in native or pure state in nature why? Write any one anyone application of sulphur

Gala2k [10]

Answer:

Sulphur is used in making car batteries and fertlizers

8 0

1 year ago

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A gas mixture at room temperature contains 10.0 mol CO and 12.5 mol O2. (a) Compute the mole fraction of CO in the mixture. (b)

zlopas [31]

Answer:

a. the mole fraction of CO in the mixture of CO and O2.

mole fraction = moles of CO/ Total moles of the mixture

Mole fraction of CO = 10/(10+12.5)=0.444

b. Reaction - CO(g)+½O2(g)→CO2(g)

Stoichiometry: 1 mole of CO react with 0.5mole of O2 to give 1 mole of CO2

So given,

At a certain point in the heating, 3.0 mol CO2 is present. Determine the mole fraction of CO in the new mixture.

3mol of CO2 is produced from 3 mols of CO and 1.5mol of O2

This means that unused mols are : 7mols of CO and 11mols of O2

Total product mixture = 3 + 7 + 11 = 21mols

mole fraction of CO = 7/21 = 0.33

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2 years ago

if kept at a constant temperature, what is the concentration at 865s if the initial concentration was 0.0225M

Anestetic [448]

Answer:

$[SO_2Cl_2]=0.0175M$

Explanation:

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In this case, considering that the decomposition reaction of SO2Cl2 is first-order, we can write the rate law shown below:

$r=-k[SO_2Cl_2]$

We also consider that the integrated rate law has been already reported as:

$[SO_2Cl_2]=[SO_2Cl_2]_0exp(-kt)$

Thus, by plugging in the initial concentration, rate constant and elapsed time we obtain:

$[SO_2Cl_2]=0.0225Mexp(-2.90x10^{-4}s^{-1}*865s)$

$[SO_2Cl_2]=0.0175M$

Best regards!

8 0

2 years ago

Which is an example of a beneficial mutation?

nata0808 [166]

Answer:

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2 years ago

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