When 1.50 g of Ba(s)is added to 100.00 g of water in a container open to the atmosphere,the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 33.10°C.If the specific heat of the solution is 4.18 J/(g ∙°C),calculate ΔH for the reaction,as written. Ba(s)+ 2 H₂O(l)→ Ba(OH)₂(aq)+ H₂(g)ΔH = ?

Question

Quizplus · Accepted Answer

The correct answer is A.The heat absorbed by the solution is:Q = m * c * ΔT = 100.00 g * 4.18 J/(g ∙°C) * (33.10°C - 22.00°C) = 4648 JThe heat released by the reaction is:ΔH = -Q = -4648 J = -4.65 kJTherefore, ΔH = -431 kJ.

When 150 G of Ba(s)is Added to 100