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, 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:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s) + 2HCl(aq) → ZnCl₂ (aq) + H₂(g) When 0.123 g of Zn(s) is combined with enough HCl to make 52.6 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.4 °C to 24.6 °C. Part A Find AHIxn for this reaction as written. (Use 1.00 g/mL for the density of the solution and 4.18 J/(g · °C) as the specific heat capacity.) Express your answer in kilojoules per mole to two significant figures. ► View Available Hint(s) AHrxn = VE ΑΣΦ ? kJ/mol
The addition of 1.250 g of zinc metal (65.38 g/mol) to 0.100 L of 0.1912 M HCl in a coffee-cup calorimeter causes the temperature to increase from 15.00°C to 21.95°C. What is the value of ΔHrxn for the following reaction? (Hint: Look at the reaction stoichiometry and decide which reactant is the limiting reactant.) Zn(s)+2HCl(aq)-->ZnCl2(aq)+H2(g) Assume the density and specific heat of the solution are 1.00 g/mL and 4.18 J/g·°C, respectively._____ kJ/mol reaction
Suppose 23.00 g ammonium chloride (53.491 g/mol) dissolves in water in a calorimeter to form 100.00 g of solution. The temperature decreases by 10.75°C. Calculate the ΔH of the solution of NH4Cl in kJ/mol. Assume the specific heats of the solution and the empty calorimeter are 4.18 J/(g·°C) and 0.170 kJ/°C, respectively.
A 21.3 ml sample of 0.997 M NaOH solution is mixed with 29.5 ml of highly concentrated HCI in a coffee-cup calorimeter. The reaction that occurs is: NAOH(aq) + HCI(aq) → NaCl(aq) + H;O(1), AH =-55.8 kJ Both solutions started at 19.6 °C prior to mixing and reacting. What is the final temperature of the reaction mixture? Assumptions to make: 1. No heat is lost from the calorimeter. 2. The density of all solutions is 1.00 g/mL. 3. Volumes are additive. 4. The C, of the solution is the same as water 4.18 J-g1.°C 1. O 25.2 °C O 20.2 °C O 19.6 °C O 19.9 °C
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
AB both
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?
Methanol is an organic solvent that can be used as a fuel in some automobiles. 2 CH3OH() + 3 02(g) → 2 CO2(g) +4 H20 (/) AH = -1452.8 kJ/mol How much heat (kJ) is evolved when 35 mL of methanol (CH3OH) with a density of 0.792 g/mL heated in the presence of excess oxygen gas?
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: