A bottle of concentrated aqueous sulfuric acid, labeled 98.0 wt% h2so4, has a concentration of 18.0 m. (a) how many milliliters
1 answer:
You might be interested in
Answer:
There are necessaries 35,2g of NH₄NO₃ per 100,0g of water to decrease the temperature of the solution from 25,0°C to 5,0°C
Explanation:
To decrease the temperature of the solution there are necessaries:
4,184J/g°C×(5,0°C-25,0°C)×(100,0g+X) = -Y
8368J + 83,68J/gX = Y <em>(1)</em>
Where x are grams of NH₄NO₃ you need to add and Y is the energy that you need to decrease the heat.
Also, the energy Y will be:
Y = 25700J/mol×X
Y = 321J/g X <em>(2)</em>
Replacing (2) in (1)
8368J + 83,68J/g X = 321J/g X
8363J = 237,32J/gX
<em>X = 35,2g</em>
<em />
Thus, there are necessaries 35,2g of NH₄NO₃ per 100,0g of water to decrease the temperature of the solution from 25,0°C to 5,0°C
I hope it helps!
Explanation:
It is known that in one day there are 24 hours. Hence, number of seconds in 24 hours are as follows.
Hence, total charge passed daily is calculated as follows.
And, number of Faraday of charge is as follows.
= 134300.52 F
The oxidation state of aluminium in is +3.
So, if we have to produce 1 mole of Al(s) we need 3 Faraday of charge.
Therefore, from 134300.52 F the moles of Al obtained with 89% efficiency is calculated as follows.
= 39842.487 mol
or, =
Molar mass of Al = 27 g/mol
Therefore, mass in gram will be calculated as follows.
Mass in grams =
=
= 1075.7 kg/day
Thus, we can conclude that the daily aluminum production of given aluminium is 1075.7 kg/day.