In a coffee-cup calorimeter, 100 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both solutions were originally at (2.22x10^1) °C. After the reaction, the temperature is (2.9200x10^1) °C. Assuming all solutions have a density of 1.00 g/mL and a heat capacity of 4.18 J/°C.g, what is the enthalpy change for the neutralization of HCI by NaOH? Assume that no heat is lost to the surroundings or the calorimeter. Enter your answer in kJ. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: Answer x10 units

A 5.71 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. What is the total mass inside the calorimeter in grams?

You are performing an important biological experiment which requires that you set up a water bath at 37.0 oC (physiological temperature). You add cold tap water at 20.0 oC, and hot tap water at 55.0 oC. You start with 85.0 g cold water, what mass of hot water must be added to get to 37.0 oC? (Specific heat capacity of water is 4.184 J/g.K)

100.0 ml of 0.115 m potassium hydroxide solution is mixed with 75.0 ml of 0.245 M nitric acid solution in a coffee cup calorimeter. Before mixing, both solutions are initially at 23.85 C;after mixing, the temperature of the mixture in the coffee cup calorimeter increases to 26.30 C. Determine the enthalpy change(delta h) of reaction in kJ/mol for the reaction as written below. KOH(aq) + HNO3(aq) ⮕ KNO3(aq) + H2O(aq) Assume the  resulting  solution density is 1.03 g/mL. Specific heat of solution=4.20 J/g C