When 1.104 grams of iron metal are mixed with 26.023g of hydrochloric acid in a coffee cup calorimeter, the temperature rises from 25.2 °C to a maximum of 33.5 °C. The reaction that occurs is given below. 2Fe (s) + 6HCl (aq) → 2FeCl3 (aq) + 3H2 (g) (a) Determine the amount of heat (in J) absorbed by the reaction mixture. Assume that the specific heat capacity of the mixture is the same as the specific heat capacity of water. (b) How much heat (in J) was released by the reaction that occurred?

1) No heat is absorbed since the temperature rose by 8.3 degrees. There will be heat absorbed, when the temperature cools down.

2) There is 903.71 Joules of energy release. This is an exothermic reaction, so ΔH will be negative.

Explanation:

Step 1: Data

Mass of iron metal = 1.104 grams

Mass of hydrochloric acid = 26.023 grams

The temperature rises from 25.2 °C to a maximum of 33.5 °C

Step 2: The balanced equation

2Fe (s) + 6HCl (aq) → 2FeCl3 (aq) + 3H2 (g)

(a) Determine the amount of heat (in J) absorbed by the reaction mixture.

No heat is absorbed since the temperature rose by 8.3 degrees. There will be heat absorbed, when the temperature cools down.

(b) How much heat (in J) was released by the reaction that occurred?

q = m*C*∆T

⇒ with q = the heat transfer (in Joule)

⇒ with m = the mass (in grams)

⇒ with C = the specific heat of water = 4.184 J/g°C

⇒ with ΔT = The change in temperature = T2 - T1 = 33.5 °C - 25.2 °C = 8.3 °C

q = (26.023g) * (4.184 J/g°C) (8.3 deg) = 903.71 J of heat released

There is 903.71 Joules of energy release. This is an exothermic reaction, so ΔH will be negative.