What are the answer choices?
Answer:
18.9 moles
Explanation:
We have the following data:
V = 50 L
P = 12.4 atm
T= 127°C + 273 = 400 K
R = 0.082 L.atm/K.mol (it is the gas constant)
We use the ideal gas equation to calculate the number of moles n of the gas:
PV = nRT
⇒ n = PV/RT = (12.4 atm x 50 L)/(0.082 L.atm/K.mol x 400 K) = 18.9 mol
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Answer: The molarity of the borax solution is 0.107 M
Explanation:
The neutralization reaction is:
According to neutralization law:
where,
= basicity of 
= 2
= acidity of borax = 2
= concentration of = 1.03 M
= concentration of borax =?
= volume of = 2.07ml
= volume of borax = 20.0 ml
Now put all the given values in the above law, we get the molarity of borax:
By solving the terms, we get :
Thus the molarity of the borax solution is 0.107 M
The balanced equation for the above reaction is as follows;
2H₂ + O₂ --> 2H₂O
stoichiometry of O₂ to H₂O is 1:2
number of O₂ moles reacted - 40.3 g / 32 g/mol = 1.26 mol
according to molar ratio
number of water moles produced = 2 x number of O₂ moles reacted
number of water moles formed - 1.26 x 2 = 2.52 mol
mass of water produced = 2.52 mol x 18 g/mol = 45.4 g
45.4 g of water produced
