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inysia [295]
3 years ago
14

Formula for zinc + nitric acid = zinc nitrate

Chemistry
1 answer:
Maslowich3 years ago
4 0

Answer:

<em>Zinc nitrate is an inorganic chemical compound with the formula Zn(NO3)2. This white, crystalline salt is highly deliquescent and is typically encountered as a hexahydrate Zn(NO3)2•6H2O. It is soluble in both water and alcohol.</em>

Explanation:

correct me if im wrong please

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Why do you think the older scientist disregarded the younger scientist's prediction?
Svetach [21]

Answer:

The older scientist were ignorant

Explanation:

they thought that they were better than the younger scientist. to put it in simply they were ignorant to think younger is worse

5 0
3 years ago
Read 2 more answers
What is the formula and name of the compound produced at the end of the virtual lab, and what caused it to have a different appe
Iteru [2.4K]

Answer: SnO_2 , NO_2 and H_2O are formed at the end of the reaction. They are named as tin (IV) oxide or stannic oxide, nitrogen dioxide and water respectively.

Explanation: Reaction of tin and nitric acid is given as:

Sn(s)+4HNO_3(aq.)\rightarrow SnO_2(s)+4NO_2(g)+2H_2O(l)

Three products are formed at the end of the reaction which are:

  • SnO_2 which is termed as stannic oxide or Tin (IV) oxide. This is a white colored solid.
  • NO_2 which is termed as nitrogen dioxide. These are brown colored fumes.
  • H_2O which is termed as water.

At the starting tin was a silvery-white colored solid and after the reaction, it changed the color to milky-white. This change in color is due to the chemical reaction happening between tin and nitric acid.

Release of brown fumes are also an indication that a chemical reaction has taken place.

6 0
3 years ago
Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is th
kolbaska11 [484]

Answer: When using 645 L /s  of O2 in a temperature and pressure of  195°C,  0.88 atm  respectively, we will get 0.355Kg /s NO

Explanation:

  • First we review the equation that represents the oxidation process of the NH3 to NO.

4NH3(g) + 5O2(g) ⟶4 NO(g) +6 H2O(l)  

  • Second we gather the information what we are going to use in our calculations.

O2 Volume Rate = 645 L /s

Pressure = 0.88 atm

Temperature = 195°C + 273 = 468K

NO molecular weight = 30.01 g/mol  

  • Third, in order to calculate the amount of  NO moles produced by 645L/ s of O2, we must find out, how many moles (n) are 645L O2 by using the general gas equation PV =n RT

Let´s keep in mind that using this equation our constant R is 0.08205Lxatm/Kxmol

PV =n RT

n= PV / RT

n= [ 0.88atm x 645L/s] / [ (0.08205 Lxatm/Kxmol) x 468K]

n= 14.781 moles /s of O2

  • Fourth, now by knowing the amount of moles of O2, we can use the equation to calculate how many moles of NO will be produced and then with the molecular weight, we will finally know the total mass per second .

14.781 moles /s of O2 x 4moles NO / 5 moles O2 x  30.01g NO / 1 mol NO x 1Kg NO /1000g NO = 0.355Kg /s NO

6 0
3 years ago
Which Domains would you find single cell organisms
kogti [31]
Archaea and Bacteria
8 0
3 years ago
How many moles of N₂ are essential for generating 0.08 moles of Li₃N in the given reaction?
joja [24]
Each mole of N₂ generates 2 moles of Li₃N. Thus,
0.08 moles of Li₃N will require:
0.08 / 2
= 0.04 moles of N₂

The second option is correct.
4 0
3 years ago
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