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IRISSAK [1]
3 years ago
14

The following balanced equation shows the formation of water.

Chemistry
2 answers:
ss7ja [257]3 years ago
8 0
Mole ratio of H₂  :  O₂   is   2  :  1

∴ if mole of H₂  =  1.67 mol

then mole of O₂ =  \frac{1.67   mol}{2}

⇒ that mole of oxygen needed to react with H₂  =  0.835 mol

The answer is A
saveliy_v [14]3 years ago
8 0

Answer: A) 0.835 mol of O_2

Explanation: According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

As can be seen from the given balanced equation:

2H_2+O_2\rightarrow 2H_2O

2 moles of hydrogen are required to react completely with 1 mole of oxygen.

Thus 1.67 moles of hydrogen will react with=\frac{1}{2}\times 1.67=0.835 moles of oxygen.

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v is the amount of electrons, which in your example seems to be six (I'm not totally sure)
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Standard conditions is 1 mol, at 298.15K and 1 atm

To find E°cell, you have to look up the reduction potensials of Fe3+ and Mg2+, and solve like this:

E°cell = cathode - anode

Cathode is where the reduction happens, so that would be the element that recieves electrons. Anode is where the oxidation happens, so that would be the element that donates electrons. In your example Fe3+ recieves electrons, and should be considered as cathode in the equation above. 

When you have found E°cell, you can just solve with the numbers I gave you. 
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3 years ago
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A 70.-kg person exposed to ⁹⁰Sr absorbs 6.0X10⁵ β⁻ particles, each with an energy of 8.74X10⁻¹⁴ J.

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