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natima [27]
3 years ago
15

Which of these is an indication that a chemical reaction has occurred?

Chemistry
1 answer:
nevsk [136]3 years ago
3 0

Formation Of A Gas.

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Explanation:

The various functions of water in plants include: maintaining cell turgidity for structure and growth; transporting nutrients and organic compounds throughout the plant; comprising much of the living protoplasm in the cells; serving as a raw material for various chemical processes, including photosynthesis; and, through transpiration, buffering the plant against wide temperature fluctuations.

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Which image shows a foliated metamorphic rock?
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If 0.5 mole of zn is added to hydrochloric acid containing 0.6 mol of hcl, which reactant is in excess
ser-zykov [4K]
The balanced equation for the reaction is as follows;
Zn + 2HCl --> ZnCl₂ + H₂
stoichiometry of Zn to HCl is 1:2
limiting reagent is the reactant that is fully consumed in the reaction.
the amount of product formed depends on amount of limiting reactant present.
The excess reactant is when it has been provided in excess and only a fraction of the provided amount is used up in the reaction.
Amount of Zn moles - 0.5 mol
Amount of HCl moles - 0.6 mol
If Zn is provided, number of HCl moles reacted - 0.5 x 2 = 1.0 mol of HCl is required, but only 0.6 mol of HCl is provided.
HCl is therefore the limiting reactant, 
Number of Zn moles required - 0.6 mol /2 = 0.3 mol
But 0.5 mol are given, therefore 0.2 mol of Zn is in excess
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What properties do protons and electrons share
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What mass of nitrogen monoxide is formed in the reaction of 869kg ammonia and 2480kg oxygen gas? (Please show work)
USPshnik [31]

Answer:

1533.6 kg NO

Explanation:

The reaction that takes place is:

  • 4NH₃ + 5O₂ → 4NO + 6H₂O

First we <u>convert the masses of ammonia (NH₃) and oxygen gas (O₂) into moles</u>, using<em> their respective molar masses</em>:

  • NH₃ ⇒ 869 kg ÷ 17 kg/kmol = 51.12 kmol NH₃
  • O₂ ⇒ 2480 kg ÷ 32 kg/kmol = 77.5 kmol O₂

77.5 kmol of O₂ would react completely with (77.5 kmol O₂ * \frac{4kmolNH_3}{5kmolO_2}) 62 kmol of NH₃. There are not as many kmol of NH₃, so NH₃ is the limiting reactant.

Now we <u>calculate how many kmol of NO are produced</u>, using the <em>limiting reactant moles</em>:

  • 51.12 kmol NH₃ * \frac{4kmolNO}{4kmolNH_3} = 51.12 kmol NO

Finally we <u>convert kmol of NO to mass</u>, using its<em> molar mass</em>:

  • 51.12 kmol NO * 30 kg/kmol = 1533.6 kg NO
6 0
2 years ago
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