Answer:
156 g of AlCl₃ will be produced from 3.5 moles of HCl.
Explanation:
Given data:
Number of moles of HCl = 3.5 mol
Grams of AlCl₃ produced = ?
Solution:
Balanced Chemical equation:
3HCl + Al(OH)₃ → AlCl₃ + 3H₂O
Now we will compare the moles of AlCl₃ with HCl from balanced chemical equation.
HCl : AlCl₃
3 : 1
3.5 : 1/3×3.5 = 1.17 mol
Mass of AlCl₃ produced:
Mass = number of moles ×molar mass
Mass = 1.17 mol × 133.341 g/mol
Mass = 156 g
Thus 156 g of AlCl₃ will be produced from 3.5 moles of HCl.
The balanced chemical
reaction will be:
C3H8 + 5O2 = 3CO2 +4H2O
We are given the amount of propane gas to be burned. This will be
our starting point.
<span>38.95 </span><span>g C3H8 ( 1 mol C3H8 / 44.1 g C3H8 ) ( 5 mol O2/1
mol C3H8)(32 g O2 / 1 mol O2) =141.32 g O2
Therefore, the reaction consumes approximately 142 grams of oxygen gas.</span>
First off there are some issues in your questions but I can still help in answering this type of problem. First, there is no Sr-20. The 4 abundant form includes Sr-84, Sr-88, Sr-87, Sr-86, Sr-84.
More importantly, the half life of strontium must be given.
For demonstration sake, let us assume Sr-85 is the isotope. It has a half-life of 64.853 days and I'm assuming the units of 87.3 is in days.
A/Ao = e^-(ln2/t)T
where A- final amount Ao -initial amount t- halflife T-total time elapsed
% = <span>e^-(ln2/64.853)(87.3) = 0.3933 or 39.33%
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Answer: England and Canada
Explanation:
Yes
Answer:
Hydrochloric Acid is the chemical name for HCI
