If 980 Kj of energy are added to 6.2 L of water at 291 K, what will the final temperature of the water be?
1 answer:
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To begin calculating, there is one thing you need to remember :
Then we have
As you know decomposition of 2moles now has prodused <span>196kj
So, </span><span>q is made due </span>
I'm sure it will help.
Then we have
As you know decomposition of 2moles now has prodused <span>196kj
So, </span><span>q is made due </span>
I'm sure it will help.
Answer: 118.5 grams
Explanation:
Molarity is defined as the number of moles of solute dissolved per liter of the solution.
where,
n= moles of solute
= volume of solution in ml = 500 ml
moles = 0.75
moles of solute =
0.75 =
mass of = 118.5 grams
Thus mass of needed to prepare 500 mL of this solution iis 118.5 grams
The final temperature : 78.925°C
<h3>Further explanation </h3>Heat can be calculated using the formula:
Q = mc∆T
Q = heat, J
m = mass, g
c = specific heat, joules / g ° C
∆T = temperature difference, ° C / K
Energy releases = 130 kcal = 130 x 4.18 kJ=543.4 kJ
The final temperature :
Final temperature :
ΔT=final-initial
51.925°c=final-27°c
final = 51.925+27=78.925°C