A block of solid gold is at its melting point of 1064 ∘ C. It has a specific latent heat of fusion of 63kJ/kg. If the block is completely melted by supplying 2.0kJ of thermal energy, what is its mass, assuming that there is no resulting temperature change?

The heat of fusion for gold at 1,063 °C is 66.6 kJ/kg and the specific heat of gold is 0.128 kJ/kg °C. What is the energy needed to melt 100 grams of gold starting at 0 °C

Assume it takes 108 joules of energy to raise the temperature of a bar of gold from 25.0°C to 29.7°C. Given that the specific heat capacity of gold is 0.128 J/g °C, what is the mass (in grams) of the bar of gold?   5.6 x 10-3 g  65 g   129 g   1.8 x 102 g  none of the above

0. A sample of solid iridium is at its melting point of 2466 ∘ C. It has a specific latent heat of fusion of 0.135MJ/kg. How much iridium would be melted if 200 kJ of thermal energy is supplied, assuming that there is no resulting temperature change?

When 3.64×10 5 J of energy is absorbed by 2.0kg of a pure solid at its melting point, exactly half of it melts. What is the latent heat of fusion of this solid?

1,300 J of energy is transferred to the thermal store of a block of gold of mass 0.2 kg.  This causes its temperature to rise from 100 to 150 °C.  Use this information to calculate the specific heat capacity of gold.5.2 J/kg °C65 J/kg °C43.3 J/kg °C130 J/kg °C