30 g of ice is put into a glasss of water. The specific latent heat of fusion for ice is 330,000 J/kg. Calculate the energy required to melt all of the ice.

As radioactive plutonium isotopes decay, they generate heat as a byproduct. Pu-239 generates 1.9W/kg of heat. How much heat will 1.25molof Pu-239 release after decaying for three hours? Express this quantity in units of calories. Assume Pu-239 has a molecular weight of 244g/mol.

19. The following fission reaction (shown below) occurs in a nuclear power plant. There are 1.50 x 1016 uranium-235 atoms that are simultaneously undergoing this reaction. The uranium is surrounded by 17.5 kg of heavy water, which has a specific heat capacity of 4.70 x 10³ J/kg °C. If 90% of the energy released in the nuclear reactions is absorbed as thermal energy by the heavy water, determine the increase in temperature of he heavy water. ✔✔✔✔ 235U+n→ Zr + 139 Te + 3(n) 92 40 52 mzr-94 = 93.906 u MTe-139 = 138.935 u Mu-235 = 235.044 u

A food product containing 80% moisture content is being frozen. Estimate the specific heat of the product at -6 ° C when 80% of the water is frozen. The specific heat of the dry product is 2 kJ / (kg ° C). it is assumed that the specific heat of water at -10 ° C is the same as the specific heat of water at 0 ° C, and the specific heat of ice follows the function Cp ice = 0.0062 Freezing point + 2.0649. Cp of frozen product = .... kJ / kg ° C.

A blacksmith cools a chunk of iron initially at 650 degrees celsius by trickling water from a jug over it. The water in the jug has a temperature of 15 degrees celsius. All of the water boils away and the iron chunk cools down 120 degrees celsius. If, in total, he poured 0.90 kg of water over the iron, what is the mass of this chunk of iron?

What is the ratio of the energy required to warm 125 g of Ice (0.0 \deg C) to body temperature (37 \deg C) to warming the same amount of water through the same temperature change? Answer format is the number Eice/Ewater = (2 significant figures) Latent Heat of Fusion of Water: 335, 000 J/kg Specific Heat Capacity of Water: 4186 J/kg/\deg C

A chunk of metal with a mass of 85.0 grams and a specific heat of 759 joules per kilogram·kelvin is heated to 78.9 degrees Celsius and placed in 122 milliliters of water (c = 4186 J/kg·K) at 18.6 degrees Celsius. What is the final temperature of the metal and water? Hint: The heat lost by the metal is gained by the water, so the sum of the heats is zero.

An ice block of mass 1.2000000000000002 kg at an initial temperature of –11 ∘C is put into a copper pot of mass 2.5 kg containing 4.3 L of water at 21 ∘C. If you heat up the pot, what is the amount of energy (in J) you need to convert all the ice and the water into steam? (Assume that no energy is lost from the system.)   You may need some or all of the following constants: The specific heat of ice is 2200 J/kg ∘C, the specific heat of copper is 386 J/kg ∘C and the specific heat of water is 4186 J/kg ∘C. The latent heat of fusion of ice is 334000 J/kg and the heat of vaporization for water is 2256000 J/kg .

A 200 g iceball can be launched from a custom launcher at 250 m/s. The iceball is initially at -5oC when it is shot vertically upwards, and by the time the iceball starts to fall down again 10 g of the ice has melted away. What is the maximum height of the iceball? The specific heat of ice is 2100 J/(kg oC) and the latent heat of fusion for ice is 334,000 J/kg.