A sheet of gold weighing 12.0 g and at a temperature of 20.0°C is placed flat...

A sheet of gold weighing 12.0 g and at a temperature of 20.0°C is placed flat on a sheet of iron weighing 21.5 g and at a temperature of 59.4°C. What is the final temperature of the combined metals? Assume that no heat is lost to the surroundings.

A 34.51−g stainless steel ball bearing at 104.89 °C is placed in a constant-pressure calorimeter containing 116.9 g of water at 22.47°C. If the specific heat of the ball bearing is 0.474 J / (g ·°C)calculate the final temperature of both the water and steel when they equilibrate. Assume the calorimeter to have negligible heat capacity.

A quantity of 2.00 ×10² mL of 0.641 M HCl is mixed with 2.00 ×10² mL of 0.321 M Ba(OH)₂ in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)₂ solutions is the same at 21.87°C. For the process below, the heat of neutralization is −56.2 kJ/mol. What is the final temperature of the mixed solutions?

H⁺(aq) + OH⁻(aq) → H₂O(l)

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Expert Solution

queen_honey_blossom answered 9 months ago

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