97.4 g/mol * 0.723
70.4g ZnO2
0.723 moles of ZnO2 would weigh approximately 141.6 grams. This is calculated by multiplying the number of moles (0.723) by the molar mass of ZnO2 (196.44 g/mol).
There is no such compound as ZnO2. Zinc oxide (ZnO) is a white powder commonly used in various applications ranging from pigments in paints to ingredients in sunscreen.
The formula is ZnO. Zn has an ion charge of 2+ and 0 has an ion charge of 2-. Therefore it cancels each other out only leaving Zn0.
Zinc and oxygen can form an ionic bond to create zinc oxide (ZnO) or a covalent bond in certain compounds like zinc peroxide (ZnO2). Both bonds involve the sharing or transfer of electrons between zinc and oxygen atoms to achieve a more stable configuration.
Zinc oxide is a white powder mineral compound made of zinc and oxygen. It is commonly used in skincare products like sunscreens for its ability to protect the skin from ultraviolet (UV) rays. Zinc oxide is also used in various other applications such as in the production of rubber, plastics, ceramics, and paints.
An amphoteric metal oxide is the oxide of a metal that can form either simple metal cations or oxyanions, depending on reaction conditions. If zinc oxide is reacted with a stong acid, a simple zinc salt including the anion of the reacting acid will form. In contrast, if zinc oxide is reacted with a strong alkali, a zincate salt containing the anion ZnO2-2 along with the cation of the strong alkali will result.
2
Formula: ZnO2
Zinc oxides are ZnO and ZnO2.
Zinc oxide is a white powder mineral compound made of zinc and oxygen. It is commonly used in skincare products like sunscreens for its ability to protect the skin from ultraviolet (UV) rays. Zinc oxide is also used in various other applications such as in the production of rubber, plastics, ceramics, and paints.
The formula is ZnO. Zn has an ion charge of 2+ and 0 has an ion charge of 2-. Therefore it cancels each other out only leaving Zn0.
The chemical formula Zn2O2 is incorrect. The correct chemical formula for zinc oxide is ZnO, which consists of one zinc atom (Zn) and one oxygen atom (O) per formula unit.
Micronutrients are actually abundant in our soils except those which are alkaline and calcareous.The total use of micronutrients in our country is 2-3%.From this you can assess hoe rich our soils are in these nutrients.Alkaline soils restrict the solubility and thus the availability of nutrients to the plants as the nutrients are converted to organic forms again;for instance zinc changes to Zn(OH)2 or ZnO2.
Word equation: Zinc oxide + Carbon → Zinc + Carbon monoxide Skeleton equation: ZnO + C → Zn + CO Balanced equation: 2 ZnO + 3 C → 2 Zn + 3 CO
An amphoteric metal oxide is the oxide of a metal that can form either simple metal cations or oxyanions, depending on reaction conditions. If zinc oxide is reacted with a stong acid, a simple zinc salt including the anion of the reacting acid will form. In contrast, if zinc oxide is reacted with a strong alkali, a zincate salt containing the anion ZnO2-2 along with the cation of the strong alkali will result.
Zinc+oxygen----> zincoxide
Metallic zinc dissolves in the alkaline solution, producing zincate ions and releasing hydrogen: Zn + 2OH– → ZnO2-- + H2 (visible as tiny bubbles on the surface of the zinc) You can get the same solution by adding zinc oxide to sodium hydroxide. (The zincate is probably hydrated with a couple of water molecules, but they only clutter up our equations, so we'll ignore them here.) Here's where it gets interesting: When copper is in contact with zinc* (bear with me for a few moments), in a conducting solution, an electrolytic cell is produced -- you have a battery. (In fact, you have Prof. Volta's original battery!) Electrons flow from the zinc* to the copper. At the surface of the copper coin, these electrons reduce the zincate: ZnO2-- + 2H2O + 2e- → Zn + 4OH– This produces the zinc plating you see on the coin. At the surface of the zinc*, the electrons that are being sent to the copper metal are generated by zinc dissolving to produce more zincate: Zn + 4OH– → ZnO2-- + 2H2O + 2e- Here's the cool thing: There is NO NET REACTION, but there is a net motion of zinc! The "zinc*" referred to above can be left-over zinc powder from the first step, or it can be zinc that's already built into the coin. Post-1981 US pennies, which are in fact mostly zinc with a thin copper cladding, work fine without an external zinc supply. It would seem that microscopic flaws in the cladding are necessary to let the zinc core contact the solution -- so perhaps "mint" condition pennies do need an external zinc source. (Science project, anyone?) The reaction seems at first glance to run against the electrochemical potentials of the metals, which perplexes many people. What makes it run, however, is the unseen dissolution of the metallic zinc*, which is particularly invisible in the case of a new US penny. (This is the same reaction that allows "sacrificial anodes" of zinc or magnesium to protect ship hulls against corrosion in salt water.) The experiment is more impressive, actually, with a true copper coin. Clean an old penny (1981 or earlier) by soaking it in hot vinegar until it's shiny, and drop it into the plating solution. Nothing will happen unless the penny is in contact with some zinc metal. Separate the penny from the zinc, and the plating will dissolve -- the penny returns to its original copper color. Touching the penny with a bit of zinc recreates the battery, and the zinc plating re-appears within seconds! Heating the zinc=plated penny, or just letting it sit around for several months, results in copper atoms dissolving into the zinc to produce brass - the "gold" coin is actually a brass-plated coin. This explanation, with more details and some great photos, can be found at http://woelen.scheikunde.net/science/chem/exps/copper+zinc/index.html -Jim Demers (9/4/2008)
intially: Zn2+ + 2OH- -->Zn(OH)2 excess hydroxide: Zn(OH)2 + 2OH- --> [Zn(OH)4]2- It is true that excess hydroxide reacts further, but the reaction is as under: Zn(OH)2 +2(OH)- ----> (ZnO2) 2- +2H2O or ZnSO4 + 4NaOH ------> 2Na2ZnO2 +2H2O, the white precipitate of zinc hydroxide dissolves with excess hydroxide and forms a soluble complex called sodium zincate. The solution becomes clear. No ppt.