Question

Suppose that 28 g of each of the following substances is initially at 26.0 ∘C. What is the final temperature of each substance upon absorbing 2.35 kJ of heat? Express your answer using two significant figures.

a) gold

b) silver

c) aluminum

d) water

Please anser all parts.

Answer 1

We know that,

Cp for gold = 0.129 J / g degree C

Cp for Silver = 0.235 J / g degree C

Cp for Aluminium = 0.897 J / g degree C

Cp for water = 4.184 J / g degree C

Mass of each = 28 g

Heat = 2.35 kJ = 2350 J

We know that,

Heat = m Cp (T2 - T1)

where,

m = 28 g

T1 = 26 degree C

a) Gold

2350 = 28 x 0.129 x (T2 - 26)

=> T2 = 676.6 degree C

b) Silver

2350 = 28 x 0.235 x (T2 - 26)

=> T2 = 383.14 degree C

c) Aluminium

2350 = 28 x 0.897 x (T2 - 26)

=> T2 = 119.57 degree C

d) Water

2350 = 28 x 4.184 x (T2 - 26)

=> T2 = 46.06 degree C