University:
Cameron University
Course:
1364 | General Chemistry I
Academic year:

2024
Views:

38

Pages:

1
Author:

Kaeden Hicks

Heat Energy A 500.0 g piece of iron is heated in a flame and dropped into 400.0 g of water at 10 degree C C. The temperature of the water rises to 90.0 C. How hot was the iron when it was removed from the flame? (The specific heat of iron is 0.473 J/ g C) Heat lost by iron = Heat gained by water q(iron) = q(water) q = m. c. ∆t X = initial temperature of iron. 𝑱 We know: The specific heat of water is : (𝟒. 𝟏𝟖𝟒 𝒈 ℃) (𝟓𝟎𝟎. 𝟎 𝒈) (𝟎. 𝟒𝟕𝟑 (𝟐𝟑𝟕 𝑱 ℃ 𝑱 𝑱 ) (𝒙 − 𝟗𝟎. 𝟎℃) = (𝟒𝟎𝟎. 𝟎 𝒈) (𝟒. 𝟏𝟖𝟒 𝒈 ℃) (𝟗𝟎. 𝟎℃ − 𝟏𝟎. 𝟎 ℃) 𝒈℃ ) 𝒙 − 𝟐. 𝟏𝟑 × 𝟏𝟎𝟒 𝑱 = 𝟏. 𝟑𝟒 × 𝟏𝟎𝟓 𝑱 (𝟐𝟑𝟕 𝒙= 𝑱 ) 𝒙 = 𝟏. 𝟓𝟓 × 𝟏𝟎𝟓 𝑱 ℃ 𝟏. 𝟓𝟓 × 𝟏𝟎𝟓 𝑱 ℃ = 𝟔𝟓𝟒 ℃ 𝟐𝟑𝟕 𝑱 A 20.0 g piece of metal at 203 C is dropped into 100 water at 25.0 C . The water temperature rose to 29.0 C. Calculate the specific heat of metal (J/g C). Assume that all of the heat lost by the metal is transferred to the water and no heat is lost to the surroundings. q(metal) = q(water) q = m. c. ∆t X = the specific heat of metal. 𝑱 We know: The specific heat of water is : (𝟒. 𝟏𝟖𝟒 𝒈 ℃) (20.0 𝑔)(𝑥)(203. ℃) = (100.0 𝑔) (4.184 𝐽 ) (29.0℃ − 25.0℃) 𝑔℃ (3480 𝑔℃)𝑥 = 1674 𝐽 𝑥= 1674 𝐽 𝐽 = 0.48 3480 𝑔℃ 𝑔℃