When 6.50g of NaOH(s) dissolves in 100g of H2O(l) in a constant pressure calorimeter, the temperature rises from 21.6 degrees Celsius to 37.8 degrees Celsius. Assuming that the specific heat of the solution is 4.18 J/g * degrees C, determine delta H for the dissolution of sodium hydroxide.

In a coffee-cup calorimeter, 0.800 g of ammonium nitrate is mixed with 37.5g of water at an initial temperature of 31.0 ^oC The ΔH for the solution of ammonium nitrate is 26.6 KJ/mol NH4NO3.  Calculate the final temperature of the calorimeter in celsius after the salt has dissolved.

A student dissolves 11.0 g of sodium hydroxide (NaOH)in 300. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 21.0°C to 31.1 °C over the course of 6.5 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) Na (aq) + OH (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 3 significant digits. - Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy A/, per mole of NaOH. O exothermic O…

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)

When 3.50 g of sodium hydroxide (NaOH) was dissolved in 50.00 g of water a value of 9.50oC was obtained for ΔT. Calculate the value (calories) for the heat of solution of 3.50 g of NaOH. Calculate the number of calories that would be produced if one mole of sodium hydroxide was dissolved. (ΔHsolnNaOH)

A student dissolves 11.0 g of potassium hydroxide (KOH) in 200. g of water in a well-insulated open cup. He then observes the temperature of the water rise from 22.0 °C to 33.7 °C over the course of 8.5 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: КОН(:) K*(aq) + OH (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. I kJ Calculate…

Calculate the change in internal energy (ΔE) for a system that is giving off 3.0 kcal of heat and is changing from 1.00 L to 8.00 L in volume at a pressure of 2.00 atm. (Remember that 101.3 J = 1 L∙atm; 1 cal = 4.18 J)

The ΔHo reaction for the oxidation of ammonia4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g) is -905.2 kJ.Calculate ΔH̊ for ammonia. The standard enthalpies of formation are:NO(g) = +90.3 kJ/molH₂O(g) = -241.8 kJ/mol.

A calorimeter contains 16.0 mLmL of water at 12.5 ∘C∘C . When 1.40 gg of XX (a substance with a molar mass of 75.0 g/molg/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq)X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.0 ∘C∘C . Calculate the enthalpy change, ΔHΔ�, for this reaction per mole of XX. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)J/(g⋅∘C)],  that density of water is 1.00 g/mLg/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures.