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

i think it is d. e because the next one is igneous.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.