Agoldsmith melts 12.4 grams of gold to make a ring. the temperature of the gold rises from 26°c to 1064°c, and then the gold melts completely. if gold’s specific heat is 0.1291 joules/gram degree celsius and its heat of fusion is 63.5 joules/gram, how much energy is gained by the gold?

2,448 J

Explanation:

1) The process in which the 12.4 g gold sample was melted can be splited in two differentiated stages: i) the increase of temperature from 26°C to 1064°C, and ii) the melting perse, which is at constant temperature.

Each stage is ruled by it specific thermodynamic model, which you can use to compute how much energy the gold gained.

2) Rising temperature

The heat energy gained by the gold to increase the temperature is given by the equation Q₁ = mCΔT.

Where m is the mass of gold, 12.4g, C is the specific heat, 0.1291 J/g°C, and ΔT is the change of temperature, 1,064°C - 26°C. Hence:

Q = 12.4g × 0.1291 J/g°C × (1,064°C - 26°C) = 1,661 J.

3) Melting

The heat energy during this stage is computed with the formula for the latent heat of fusion:

Q₂ = m × latent heat of fusion = 12.4  g × 63.5 J/g = 787.4 J ≈ 787 J.

3) The total heat energy gained, Q, is the sum of the energy gained during the two stages:

Q = Q₁ + Q₂ = 1,661 J + 787 J = 2,448 J ← answer

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.