Which bonds form in the reaction shown in the diagram? 2 2H, + 0 H-H O=0 H-H → 2H 0 H-0-H H-OH A. The bonds between the two hydr
ogen atoms and between the two oxygen atoms B. The bonds between the two hydrogen atoms C. The bonds between the oxygen and hydrogen atoms D. The bonds between the two oxygen atoms
2 answers:
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The given question is incomplete. The complete question is:
Suppose a current of 0.920 A is passed through an electroplating cell with an aqueous solution of agno3 in the cathode compartment for 47.0 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell.
Answer: 0.0484 g
Explanation:
where Q= quantity of electricity in coloumbs
I = current in amperes = 0.920 A
t= time in seconds = 47.0 sec
96500 Coloumb of electricity electrolyzes 1 mole of Ag
43.24 C of electricity deposits = of Ag
Thus the mass of pure silver deposited on a metal object made into the cathode of the cell is 0.0484 g
Answer:
1) Maximun ammount of nitrogen gas:
2) Limiting reagent:
3) Ammount of excess reagent:
Explanation:
<u>The reaction </u>
Moles of nitrogen monoxide
Molecular weight:
Moles of hydrogen
Molecular weight:
Mol rate of H2 and NO is 1:1 => hydrogen gas is in excess
1) <u>Maximun ammount of nitrogen gas</u> => when all NO reacted
2) <u>Limiting reagent</u>:
3) <u>Ammount of excess reagent</u>: