At 1 atm, how much energy is required to heat 79.0 g H,O(s) at – 18.0 °C to H,O(g) at 157.0 °C? Use the heat transfer constants found in this table. q = kJ

10.00 g of Compound X with molecular formula C4H8 are burned in a constant-pressure calorimeter containing 50.00 kg of water at 25 °C. The temperature of the water is observed to rise by 2.151 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

Let's use our knowledge of constant volume (bomb) calorimetry to determine the heat energy in a given food sample, say a hamburger. A typical hamburger has a serving size of 105 g and consists of approximately 20% protein (21.0 g), 33% fat (34.7 g), and 47% carbohydrate (49.3 g). Assume that the heat capacity of the bomb calorimeter is 8.39 kJ K-¹, and the increase in water temperature was 13.2 K. Q5.38 Homework Unanswered How many Calories (Cal) are in the hamburger described above? Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105) Type your numeric answer and submit Unanswered • 4 attempts left Submit

A system does 516516 kJ of work and loses 236236 kJ of heat to the surroundings. What is the change in internal energy, Δ?Δ�, of the system? Note that internal energy is symbolized as Δ?Δ� in some sources.

An ideal gas sealed in a rigid 3.13-L cylinder, initially at pressure Pi=12.70 atm, is cooled until the pressure in the cylinder is Pf=1.18 atm. What is the enthalpy change for this process?What is the change in internal energy for this process?

If we measure the heat change (q) of everything in a system except the calorimeter, we can use the first law of thermodynamics (∆Euniverse = 0) to calculate the heat change of the calorimeter (qcal).  In this reaction, we combine 5.85 g of 63.7 ºC water with 6.63 g of 18.9 ºC water in a calorimeter.  Since some of the heat is absorbed by the calorimeter, the final temperature of the water is 28.8ºC.  Since the hot and cold water are combined, the final temp of the water is the final temp for the hot water and the cold water.  Calculate the heat change of the calorimeter in J. Remember that all of the heat changes must add up to zero so you can calculate the heat change of the hot water (qhotwater) and the heat change of the cold water (qcoldwater) using for each where Cs = 4.186 J/gºC.  The first law of thermodynamics tells us that all of these changes sum up to zero so   Enter your answer to one decimal place (tenths)

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A 25.0 mL portion of dilute HCl (aq) is combined with a 25.0 mL portion of dilute NaOH in a coffee-cup calorimeter. Both solutions are initially at a temperature of 23.3 ºC. The reaction produces enough heat to raise the final temperature of the 50.0 mL of liquid in the calorimeter to 25.3 ºC . What is qrxn in J? Assume the density of the reaction mixture is 1.0 g/mL and the specific heat of the solution is 4.184 J/g· ºC