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GenaCL600 [577]

3 years ago

8

Explain how the models you developed show that when methane combines with oxygen to form carbon dioxide and water, no atoms are

left over from the reaction.

1 answer:

Xelga [282]3 years ago

3 0

Answer: the bonds in the methane and oxygen come apart, the atoms rearrange and then re-bond to form water and carbon dioxide

Explanation:^

You might be interested in

What is the molar mass of CaCL2•2 H2O

kotykmax [81]

Answer:

147 amu

Explanation:

CaCl2. 2H2O

=>40*1+35.5*2+2*1*2+2*16

=>40+71+4+32

=>147 amu..

I hope u will understand it:-):-)

6 0

3 years ago

In June there are fewer hours of daylight and less direct sunlight in the

Dafna11 [192]

<span>In June there are fewer hours of daylight and less direct sunlight in the Southern Hemisphere.

Your answer is <em>Southern Hemisphere</em><em></em>.

</span>

5 0

2 years ago

.....................?

liraira [26]

Answer:

Look at the periodic table of elements

Explanation:

Group 1 is the most reactive and to the right

Group 18 is least reactive and all the way to the left. The rest are in between. The groups go vertical.

You'd be able to solve with this information youre welcome

4 0

2 years ago

In the reaction of 675.9 grams of barium chloride and excess silver(I) nitrate, how many grams of silver(I) chloride should get

zvonat [6]

Taking into account the reaction stoichiometry, the mass of silver(I) chloride formed is 930.37 grams.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

2 AgNO₃ + BaCl₂ → 2 AgCl + Ba(NO₃)₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

AgNO₃: 2 moles
BaCl₂: 1 mole
AgCl: 2 moles
Ba(NO₃)₂: 1 mole

The molar mass of the compounds is:

AgNO₃: 169.87 g/mole
BaCl₂: 208.24 g/mole
AgCl: 143.32 g/mole
Ba(NO₃)₂: 261.34 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

AgNO₃: 2 moles ×169.87 g/mole= 339.74 grams

BaCl₂: 1 mole ×208.24 g/mole= 208.24 grams

AgCl: 2 moles ×143.32 g/mole= 286.64 grams

Ba(NO₃)₂: 1 mole×261.34 g/mole= 261.34 grams

<h3>Mass of silver(I) chloride formed</h3>

The following rule of three can be applied: if by reaction stoichiometry 208.24 grams of barium chloride form 286.64 grams of silver(I) chloride, 675.9 grams of barium chloride form how much mass of silver(I) chloride?

$mass of silver(I) chloride=\frac{675.9 grams of barium chloride x286.64 grams of silver(I) chloride }{208.24 grams of barium chloride}$

mass of silver(I) chloride= 930.37 grams

Finally, the mass of silver(I) chloride formed is 930.37 grams.

Learn more about the reaction stoichiometry:

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brainly.com/question/24653699

#SPJ1

8 0

1 year ago

Cerium (IV) ions are strong oxidizing agents in acid ic solution, oxidizing arsenio us acid to arsen ic acid accor ding to the f

kirill [66]

Answer:

0.2042 M is the original concentration of $Ce^{4+}$ (aq) in the titrating solution.

Explanation:

Mass of $As_2O_3$ = 0.217 g

Moles of $As_2O_3=\frac{0.217 g}{198 g/mol}=0.001096 mol$

1 mole of $As_2O_3$ have 2 mole of As and 1 mole of $H_3AsO_3$ have 1 mole of As.

So, from 1 mole of $As_2O_3$ we will have 2 moles of $H_3AsO_3$

Then from 0.001096 mol of $As_2O_3$ :

$2\times 0.001096 mol=0.002192 mol$ of $H_3AsO_3$

$2Ce^{4+}(aq)+H_3AsO_3(aq)+3H_2O(l)\rightarrow 2Ce^{3+}(aq)+H_3AsO_4(aq)+2H^+(aq)$

According to reaction, 1 mole of $H_3AsO_3$ reacts with 2 mole of cerium (IV) ions,then 0.002192 mol of

$\frac{2}{1}\times 0.002192 mol=0.004384 mol$ of cerium (IV) ions.

Volume of the acidic cerium{IV) sulfate = 21.47 ml =0.02147 L

1 mL = 0.001 L

$concentration = \frac{Moles}{Volume(L)}$

$[Ce^{4+}]=\frac{0.004384 mol}{0.02147 L}=0.2042 M$

0.2042 M is the original concentration of $Ce^{4+}$ (aq) in the titrating solution.

8 0

2 years ago