You can create ice by adding liquid nitrogen to a container of water. If you want to produce 200g of ice from 450g of water at 10°C, how many grams of liquid nitrogen (at its boiling point) would need to be added to the water? Assume that the liquid nitrogen leaves the container of water as soon as it turns to gas. Assume the water values are given to the nearest gram. The boiling point of liquid nitrogen is 77.3K. Given: Latent heat of vaporisati on of nitrogen: L, = 201.0 Latent heat of fusion of water: Le = 333.02; heat capacity of water. C, = 4.186 T(K) = T(°C) + 273.15 Qr = mC,AT; Qv or f = mLv or f

You read in a popular diet blog that the author claims you can lose up to half a pound of body fat per week if, instead of drinking 1.9 liters (i.e., 1.9 kilograms) of water every day, you can eat the same amount of water in the form of ice. The reasoning is that your body must first melt the ice and then bring the ice water up to the body temperature of 37°C, which is a process that requires a significant amount of energy at the expense of “burned” body fat. Thankfully, you just finished discussing heat and phase changes in your physics class, so you can calculate exactly how much energy is expended. The specific heat and latent heat of fusion for water are 4.186 × 103 J/(kg⋅°C) and 3.34×105 J/kg, respectively a)  How many kilocalories do you expend when you eat 1.9 kg of ice at 0°C? Note that 1 kcal = 4186 J.  b) Assuming the metabolism of one pound of body fat produces 3500 kcal of energy, how many pounds of body fat could you lose in a week just by eating 1.9 kilograms of ice every…

What is the ΔS° for the reaction? Given are the S°, in J K-1 mol-1, of each substance in parentheses. SiCl4 (g, 330.73) + 2 Mg (s, 32.68) → 2 MgCl2 (s, 89.62) + Si (s, 18.83)     -198.02 J/K     198.02 J/K     -254.96 J/K     254.96 J/K

One mole of oxygen gas is at a pressure of 5.45 atm and a temperature of 27.5°C. (a) If the gas is heated at constant volume until the pressure triples, what is the final temperature? °C (b) If the gas is heated so that both the pressure and volume are doubled, what is the final temperature? °C Submit Answer

A volumetric flask made of Pyrex is calibrated at 20.0°C. It is filled to the 235-mL mark with 37.0°C glycerin. After the flask is filled, the glycerin cools and the flask warms so that the combination of glycerin and flask reaches a uniform temperature of 32.0°C. The combination is then cooled back to 20.0°C. (The average volume expansion coefficient of glycerin is 4.85  10-4(°C)−1.) (a) What is the volume of the glycerin when it cools to 20.0°C?