<h3>
Answer:</h3>
32.98°C
<h3>
Explanation:</h3>
We are given the following;
Mass of Aluminium as 125 g
Initial temperature of Aluminium as 182°C
Mass of water as 265 g
Initial temperature of water as 22°C
We are required to calculate the final temperature of the two compounds;
First, we need to know the specific heat capacity of each;
Specific heat capacity of Aluminium is 0.9 J/g°C
Specific heat capacity of water is 4.184 J/g°C
<h3>Step 1: Calculate the Quantity of heat gained by water.</h3>
Assuming the final temperature is X°C
we know, Q = mcΔT
Change in temperature, ΔT = (X-22)°C
therefore;
Q = 365 g × 4.184 J/g°C × (X-22)°C
= (1527.16X-33,597.52) Joules
<h3>Step 2: Calculate the quantity of heat released by Aluminium </h3>
Using the final temperature, X°C
Change in temperature, ΔT = -(X°- 182°)C (negative because heat was lost)
Therefore;
Q = 125 g × 0.90 J/g°C × (182°-X°)C
= (20,475- 112.5X) Joules
<h3>Step 3: Calculating the final temperature</h3>
We need to know that the heat released by aluminium is equal to heat absorbed by water.
Therefore;
(20,475- 112.5X) Joules = (1527.16X-33,597.52) Joules
Combining the like terms;
1639.66X = 54072.52
X = 32.978°C
= 32.98°C
Therefore, the final temperature of the two compounds will be 32.98°C
= 0.35 mol CO₂