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Aliun [14]
2 years ago
15

The reaction of nitrogen with methane in excess oxygen produces water, ________, and ___________. N2(g) + O2(g) + CH4(g) → CO2(g

) + H2O(g) + NO2(g) A) carbon oxide, nitrogen oxide B) carbon oxygen, nitrogen oxygen C) carbon dioxide, nitrogen dioxide D) dicarbon oxide, dinitrogen oxide
Chemistry
1 answer:
IrinaVladis [17]2 years ago
3 0

Answer:

C.

Explanation:

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A
Aleksandr [31]

Answer:

D. Using a battery

3 0
3 years ago
what temperature change will be observed if a sample of 100 g of ethylene glycol antifreeze solution (specific heat capacity = 3
ivolga24 [154]

Answer:

1°C temperature change will be observed if a sample of 100 g of ethylene glycol antifreeze solution.

Explanation:

Mass of ethylene glycol = m = 100 g

Specific heat capacity of ethylene glycol = c = 3.5 J/g°C

Change in temperature of ethylene glycol = ΔT

Heat loss by the ethylene glycol = Q = 350 J

Q=mc\Delta T

\Delta T=\frac{Q}{mc}=\frac{350 J}{100 g\times 3.5 J/g^oC}

ΔT = 1°C

1°C temperature change will be observed if a sample of 100 g of ethylene glycol antifreeze solution.

3 0
3 years ago
The theoretical yield is the amount of product actually produced. <br><br> a. True<br> b. False
jolli1 [7]

Answer:

a. True

Explanation:

Theoretical yield is the amount of product that could be obtained if a chemical reaction has 100% efficiency.

Hope it helps...

6 0
3 years ago
Read 2 more answers
When two species A and B form an electron-pair bond and A does not provide its electrons for bonding, the bond present between A
vichka [17]

Answer:

Ionic

Explanation:

If A does not have electron to bond, it just receives one electron from B.

It can´t be covalent because A don´t have any electrons to bond with B.

5 0
3 years ago
Ammonia, NH 3 , may react with oxygen to form nitrogen gas and water. 4 NH 3 ( aq ) + 3 O 2 ( g ) ⟶ 2 N 2 ( g ) + 6 H 2 O ( l )
Alex Ar [27]

Answer:

The limiting reactant is NH₃

0.0186moles of N₂ are the one produced by the limiting reactant

0.020 moles of N₂ are the one produced by the reactant in excess

Explanation:

This is the reaction

4NH₃ + 3O₂  → 2N₂ + 6H₂O

We should calculate the moles of each reactant

Mass / Molar mass = Moles

3.55 g / 17g/m = 0.208 moles NH₃

5.33 g / 32g/m = 0.166 moles O₂

4 moles of ammonia react with 3 moles of oxygen

0.208 moles of ammonia react with (0.208  .3)/4 = 0.156 moles O₂

We have 0.166 moles of O₂ and we need 0.156 moles, so O₂ is the reactant in excess.

3 moles of O₂ react with 4 moles of NH₃

0.166 moles of O₂ react with (0.166 . 4)/ 3 = 0.221 moles

We have 0.208 moles NH₃ and we need 0.221, so NH₃ is the limiting reactant.

To know the moles of N₂, let's apply the Ideal Gas Law

P.V =n.R.T

1atm . 0.450L = n . 0.082 . 295K

0.450 / (0.082 .295) = 0.0186 moles

If we have 100 % yield reaction:

4 moles NH₃ make 2 moles N₂

0.208 moles NH₃ make (0.208  .2)/4 = 0.104 moles

So the % yield reaction is.

0.104 moles ___ 100%

0.0186 moles ___ 17.9%

0.0186moles of N₂ are the one produced by the limiting reactant.

3 moles of O₂ produce 2 moles N₂

0.166 moles O₂ produce  (0.166  .2)/3 = 0.111 moles

Now, we apply the yield.

100% ____ 0.111 moles

17.9% = 0.020 moles

8 0
3 years ago
Read 2 more answers
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