Considering the reaction of hydrogen and oxygen to produce water. If 24.6 g of water is produced and 2.9 g of hydrogen is used, the amount of oxygen needed is 21.87 grams
The best way to solve this question is to write out the reaction between hydrogen and oxygen that resulted in the formation of water.
So, we have:
From the above reaction;
2 moles of hydrogen gas reacted with 1 mole of oxygen to produce 2 moles of water.
If;
- 1 mole of O₂ = 32 grams of O₂
- 2 mole of H₂O = 2 × 18 grams of H₂O
- 2 mole of H₂O = 36 grams of H₂O
We can deduce that since 1 mole of O₂ produced 2 moles of H₂O;
Thus, 32 grams of O₂ is needed to produce 36 grams of H₂O.
∴
To produce, 24.6 grams of H₂O, we have:
= 21.87 grams of oxygen.
Therefore, we can conclude that the amount of oxygen needed is 21.87 grams.
Learn more about chemical reactions here:
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Answer:
the first one is balanced.
Answer: a. 0.26mol
b. 0.000479mol
c. 1.12mol
Explanation: Please see attachment for explanation
Answer:
0.0008 mole of HCl
Explanation:
From the balanced equation between HCl and NaOH:
1 mole of acid requires 1 mole of base for neutralization.
mole = molarity x volume
mole of NaOH = 0.02 x 0.04 = 0.0008 mole
mole HCl = 0.16 x 0.01 = 0.0016 mole
Since 1 mole of NaOH requires 1 mole of HCl for neutralization, it means that 0.0008 mole of NaOH will require 0.0008 mole of HCl. The remaining mole of HCl must have been neutralized by the antiacid:
0.0016 - 0.0008 = 0.0008 mole.
Therefore, 0.0008 mole of HCl must have been neutralized by the antiacid.
Answer:
I don't have any answer sorryyyy!!
Explanation:
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