A sheet of gold weighing 12.0 g and at a temperature of 20.0°Cis placed flat on a sheet of iron weighing 21.5 g and at atemperature of 59.4°C. What is the final temperature of thecombined metals? Assume that no heat is lost to thesurroundings.
A 34.51−g stainless steel ball bearing at 104.89 °C is placed ina constant-pressure calorimeter containing 116.9 g of water at22.47°C. If the specific heat of the ball bearing is 0.474 J / (g·°C)calculate the final temperature of both the water and steelwhen they equilibrate. Assume the calorimeter to have negligibleheat capacity.
A quantity of 2.00 ×102 mL of 0.641 M HCl ismixed with 2.00 ×102 mL of 0.321 MBa(OH)2 in a constant-pressure calorimeter of negligibleheat capacity. The initial temperature of the HCl andBa(OH)2 solutions is the same at 21.87°C. For theprocess below, the heat of neutralization is −56.2 kJ/mol. What isthe final temperature of the mixed solutions?
H+(aq) + OH−(aq) →H2O(l)
