Potential enegry because it not being used yet
Answer:
0.886 J/g.°C
Explanation:
Step 1: Calculate the heat absorbed by the water
We will use the following expression
Q = c × m × ΔT
where,
- c: specific heat capacity
- ΔT: change in the temperature
Q(water) = c(water) × m(water) × ΔT(water)
Q(water) = 4.184 J/g.°C × 50.0 g × (34.4 °C - 25.36 °C) = 1.89 × 10³ J
According to the law of conservation of energy, the sum of the energy lost by the solid and the energy absorbed by the water is zero.
Q(water) + Q(solid) = 0
Q(solid) = -Q(water) = -1.89 × 10³ J
Step 2: Calculate the specific heat capacity of the solid
We will use the following expression.
Q(solid) = c(solid) × m(solid) × ΔT(solid)
c(solid) = Q(solid) / m(solid) × ΔT(solid)
c(solid) = (-1.89 × 10³ J) / 32.53 g × (34.4 °C - 100. °C) = 0.886 J/g.°C
Potassium hydroxide (KOH) is the base.
Answer:
2,0 M of Al³⁺ and 6,0M of NO₃⁻.
Explanation:
In water, Al(NO₃)₃ dissociates as follows:
Al(NO₃)₃ → Al³⁺ + 3 NO₃⁻
That means in water, you will have 1 mole of Al³⁺ and 3 moles of NO₃⁻ per mole of Al(NO₃)₃.
Now, as the solution of Al(NO₃)₃ is 2,0M, you will have
<em>2,0 M of Al³⁺ and 6,0M of NO₃⁻.</em>
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I hope it helps!