In a coffee cup calorimeter, 3.00 g of NaOH (molar mass 40.00g/mol) was mixed with 75.0 mL of 1.00M HNO3. If the initial temperature of the HNO3 was 31.3°C and the final temperature of the solution was 22.3°C, determine AH for the reaction in kJ/mol. NaOH(s) + HNO3(aq) ===> NaNO3(aq) + H2O) The density and the specific heat capacity of the resulting solution are 1.00 g/ml and 4.18 J/°C.g, respectively. Units do not need to be typed, simply enter the correct number. If the sign of AH is negative put a negative sign (-) in the answer. Answer:

In a coffee cup calorimeter, 50.0 mL of 0.106 M AgNO3 and 50.0 mL of 0.106 M HI are mixed. The following reaction occurs. Ag+ (aq) + I¯(aq) → AgI(s) If the two solutions are initially at 21.80°C, and if the final temperature is 23.22°C, calculate AH for the reaction in kJ/mol of AgI formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J °C-¹ g-¹. X kJ/mol

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A 1.110-g sample of benzoic acid (HC7H5O2; molar mass = 122.12 g/mol) is burned in an excess of O2(g) in a bomb calorimeter, which is immersed in water. The reaction produces heat that causes the temperature of the water and bomb to increase from 21.90 to 26.15oC. (a) If the heat capacity of the calorimeter is 6.90 kJ/oC, calculate the amount of heat (in kJ) absorbed by the calorimeter. (b) How much heat (in kJ) is produced if 1.00 g of benzoic acid is completely combusted? (c) Calculate the molar enthalpy of combustion of benzoic acid.

A student dissolves 14.1 g of sodium hydroxide (NaOH)in 250. g of water in a well-insulated open cup. He then observes the temperature of the water rise from 22.0 °C to 35.5 °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 AHxn per mole of NaOH. exothermic O…

10. The enthalpy change for the reaction: H+(aq) + OH-(aq) → H2O (l) ΔH rxn =-57.6 kJ/mol. If 161.4 mL of 0.52 M H3PO4 at 24.17°C is mixed with 169.1 mL of 0.56 M Ba(OH)2 at 24.17°C, what is the maximum temperature reached by the resulting solution if the heat capacity of the calorimeter is 435.6 J/K?

66.667 ml of 3.000 M H2SO4 (aq) solution was neutralized by the stoichiometric amount of 4.000 M Al(OH)3 solution in a coffee cup calorimeter. The initial temperature of the solutions was 22.3 ºC and after mixing the temperature raised to 24.7 ºC. If the heat capacity of coffee cup is 1.10 J/g ºC, calculate the DHreaction in J/mol Al2(SO4)3.

Zinc metal reacts with HCl according to the following balanced equation: Zn(s) + 2HCI(aq) --> ZnCl2(aq) + H2(g) When 0.140 grams of Zn(s) is combined with an excess amount of HCI to make 50.0 mL of solution in a coffee-cup calorimeter, all the zinc reacts, raising the temperature of the solution from 21.60°C to 24.60°C. Find AH for this reaction in kJ/mol. Assume the density of the solution is 1.00 g/mL and the specific heat capacity of the solution is 4.184 J/g°C. Use an atomic weight of 65.38 g/mol for Zn Hints: -q(reaction) = q(solution) %3D AH = q/mol of limiting reagent %3D Do not type units with your answer. Type your answer to three significant figures. the proper If this question is on an exam on your scrap paper report your answer number of significant figures but still type three significant figures online. Your Answer:

In a coffee cup calorimeter, 50.0 mL of 0.139 M AgNO3 and 50.0 mL of 0.139 M HI are mixed. The following reaction occurs. Ag+ (aq) + I (aq) → Agi(s) If the two solutions are initially at 21.74°C, and if the final temperature is 23.60°C, calculate AH for the reaction in kJ/mol of AgI formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J °C-1g-¹. kJ/mol Need Help? Read It Supporting Materials Periodic Table Watch It Constants & Factors. Supplemental Data

In a coffee cup calorimeter, 50.0 mL of 0.130 M AGNO, and 50.0 mL of 0.130M HBr are mixed. The following reaction occurs. Ag*(aq) + Br¯(aq) → AgBr(s) If the two solutions are initially at 23.51°C, and if the final temperature is 24.82°C, calculate AH for the reaction in kJ/mol of AgBr formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J°C¯1g=1. 84.2 X kJ/mol