What mass of this substance must evaporate to freeze 210 g of water initially at 24 ∘C? (The heat of fusion of water is 334 J/g; the specific heat of water is 4.18 J/(g⋅K).)
What mass of this substance must evaporate to freeze 210 g of water initially at 24...
Compounds like CCl2F2 are known as chlorofluorocarbons, or CFCs. These compounds were once widely used as refrigerants but are now being replaced by compounds that are believed to be less harmful to the environment. The heat of vaporization of CCl2F2 is 289 J/g. What mass of this substance (in grams) must evaporate in order to freeze 250 g of water initially at 15 ?C? (The heat of fusion of water is 334 J/g; the specific heat of water is 4.18...
32. An icemaker uses the heat change from evaporation of a refrigerant to freeze water. How many moles of the refrigerant CCI,F2 must be evaporated to freeze 209 g of water initially at 0°C to make ice at 0 °C? The heat of vaporization of CCI,F2 is 289 J/g. The heat of fusion of water is 334 J/g. A. 0.00 moles B. 1.00 moles C. 2.00 moles D. 3.00 moles E. 4.00 moles
What will take the most energy? (Constants: Heat of fusion of water: 334 J/g Heat of vaporization of water: 2260 J/g Specific heat capacity of copper: 0.385 J/g*C Specific heat capacity of gold: 0.129 J/g*C Specific heat capacity of water: 4.18 J/g*C) a. Increase the temperature of 10 grams of solid gold by 15 degrees b. Increase the temperature of 10 grams of solid water (ice) by 12 degrees c. Evaporate 10 grams of water d. Increase the temperature of...
1. A 110.4 g110.4 g sample of a substance is initially at 20.1 °C20.1 °C . After absorbing 335 cal335 cal of heat, the temperature of the substance increases to 67.6 °C67.6 °C . What is the specific heat (SH)(SH) of the substance? 2. When 165.0165.0 J of heat are added to a 15.015.0 g sample of mercury the final temperature of the mercury is recorded as 63.063.0 °C. The metal has a specific heat of 0.13950.1395 J/(g·°C). 3. A...
20.45g of a substance, initially at 97.20C was poured into 10.08 g of water in a calorimeter. The initial temperature of the water and the calorimeter was 21.37C. The calorimeter has a heat capacity of 9.76 J/K. The temperature after mixing, Tf, was determined to be 32.66C. Calculate the specific heat capacity of the substance.
A 20-g ice cube floats in 210 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 92°C is dropped into the cup, and the final equilibrium temperature is 12°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 105 J/kg and 4,186 J/kg · °C, respectively. The specific heat of lead and copper are 128 and 387 J/kg · °C,...
mass of water is 0.3kg
An insulated beaker with negligible mass contains a mass of 0.300 kg of water at a temperature of 84.1 °C. - Part A How many kilograms of ice at a temperature of – 10.3 °C must be dropped in the water to make the final temperature of the system 29.9 °C? Take the specific heat for water to be 4190 J/(kg · K), the specific heat for ice to be 2100 J/(kg · K), and...
//
Chemical potential/phases A substance has three phases: gas, liquid, and solid. The chemical potentials of various phases are illustrated below. T (K) 1) For a given temperature, which of the states represents an equilibrium condition? Submit 2) If the substance starts out in state Q and is held at constant temperature, what happens if it is allowed to reach equilibrium? The substance will freeze. The substance will evaporate The substance will melt and evaporate. The substance will sublime. Nothing...
How much heat must be removed to completely freeze 15 kg of water initially at 95°F? For water : Cice = 2100 J kg.K Cwater = 4186 kg K Lf=3 J . 34 x 10° ke, L, = 2. 26 x 100 kg