Consider the reaction Mg₂Si(s) + 4 H₂O(ℓ) → 2 Mg(OH)₂(aq) + SiH₄(g). How many grams of silane gas (SiH₄) are formed if 25.0 g of Mg₂Si reacts with excess H₂O?
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Ответ:
10.60 grams of silane gas are formed.
Explanation:
From the reaction:
Mg₂Si(s) + 4H₂O(l) → 2Mg(OH)₂(aq) + SiH₄(g)
We know that the limiting reactant is Mg₂Si, so to find the mass of SiH₄ formed we need to calculate the number of moles of Mg₂Si:
Where:
m: is the mass of Mg₂Si = 25.0 g
M: is the molar mass of Mg₂Si = 76.69 g/mol
Now, the stoichiometric relation between Mg₂Si and SiH₄ is 1:1 so:
Finally, the mass of SiH₄ is:
Therefore, 10.60 grams of silane gas are formed.
I hope it helps you!
Ответ:
Answer 1) : To rank the species according to the decreasing energy needed to raise the temperature of 10 g of the substance by 25 °C, the oder of energy needed is given below as per their specific heat.
Which requires more energy as per their specific heats;
water 4.184aluminum 0.897cast iron 0.460Copper 0.385Silver 0.235Answer 2)To rank items as equivalent, overlap them.
The average kinetic energy of the molecules after point D,
The average kinetic energy of the molecules from point B to point C,
The average kinetic energy of the molecules before point A.