Sample 1 Sample 2 [1] Volume of HCI (mL) 50.2 50.2 [2] Temperature of HCI (mL) 24.8 24.3 [3] Volume of NaOH (mL) 49.8 49.9 [4] Temperature of mixture after reaction ("C) 31.8 31.0 Temperature difference ("C) [5] Number calories evolved (cal) enter a positive value [6] Moles of H* that were neutralized (mol) [7] Calories evolved per mole of H* (cal/mol) Average of the two trials of calories evolved per mole of H*
Q: hydrochloric acid + calcium carbonate carbonic acid + calcium chloride --> CO2(g) + H2O(1) + Calcium…
A: Answer: Balanced equation: CaCO3(s) + 2HCl(aq) ---> CaCl2(aq) +…
Q: Given the data below, H°rxn for the reaction 3Cl2 (g) + PH3 (g) → PCl3 (g) + 3HCl (g) is…
A: Hess's law states that the amount of heat evolved or absorbed in a process is independent of the…
Q: If AG for a reaction is -3.8 kcal/mol, and Q is 1.3 x10°, what is the value of Keg for this reaction…
A:
Q: Кон, heat G) () name of reaction 1. CH,CH2CH,M9CI (k) (k) 2. H+ name of reaction
A:
Q: NaOH + HeSO4 NO visiable Change yes 7. test tube 90t warm 8 NoOH t K2COS NO Changes NO 13 8. NaOH+…
A: 7. For NaOH and H2SO4 : The molecular reaction : 2NaOH(aq.) + H2SO4(aq.) → Na2SO4(aq.) +…
Q: Given the following equation, C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) ΔG°rxn = -2074 kJ Calculate…
A: The desired equation is, 5C3H8(g) +25O2(g) →15CO2(g) +20H2O(g) ;∆G°=? The given…
Q: Using only following ArxnH° values: kJ 4 NH3 (g) + 5 O2 (g) → 4 NO (g)+ 6 H2O (£) ArxnH° = -1170 mol…
A: Our desired equation is: NH3(g) + 2O2(g) ----> HNO3(l) + H2O(l) We have to arrange the given…
Q: Based on the following reaction and enthalpy data: HBF2 + Bel2 → BeF2 + Hgl2 Q R S P Data: H8F2 =…
A:
Q: n Completion Status: Moving to another question will save this response. n 2 new element (Rr) has…
A:
Q: In a calorimeter, 460 mL of sulfuric acid reacts with 0.970 L of NaOH. Temperature final is 24.49 °…
A: Volume of sulfuric acid = 460 ml So mass of sulfuric acid = 460 g Volume of NaOH = 0.970 L = 970 ml…
Q: How many moles are contained in each number of grams of fructose (C6H1206, molar mass 180.2 g/mol),…
A: 1 mole = 6.022×1023 [Avogadro's number] The mass of 1 mole of molecules of any substance is known…
Q: Questions 1. Complete the following reactions: a. heat NH, C,H,NO, b. heat NH OH/H,0 C,H,O, +] then…
A: In this problem, we will perform the following reactions: phthalic anhydride with ammonia. Which…
Q: CS2 and 10.0 g Cl2 reacts by the followi CS2(g) + 3Cl2 (g) AH = -230. kJ
A: Given, Mass of Cl2 = 10 g Mass of CS2 = 10 g Molar mass of CS2 = 76 g/mol Molar mass of Cl2 = 71 g…
Q: D=delta symbol. Component DHf (kJ/mole) Component DHf (kJ/mole) C7H12 (l) -187.9 C7H12…
A:
Q: Consider the followin thermochemical equation: 2NH3 (g) + 6H2O (g) -> 1/2 N2 (g) + 9H2 + 5/2 O2…
A: Reversing the equation-2:2NH3 (g) -> N2 (g) + 3H2 (g) ΔH° =+22.10 kcalReversing the equation-3…
Q: Calculate the ΔH for the reaction: CS2 (l) + 2 O2 (g) —> CO2 (g) + 2 SO2 (g) Given: ΔHf o CO2 (g) =…
A: To find out enthalpy change for a reaction we will use the formula " Enthalpy change for a reaction…
Q: Use the following reactions to find AH when 1 mole of HCI gas forms from its elements: N2 (g) + 3 H2…
A:
Q: General Chemistry student performed the “Thermochemistry” lab and obtained the following results:…
A: The balanced reaction is: HCl+NaOH→NaCl+H2O Calculation of no. of mol of HCl: n=Molarity×Volume=2.15…
Q: This is an endothermic reaction O A. True O B. False
A: The reaction which release heat during the course of the reaction are called exothermic reactions.…
Q: RUN 1 RUN 2 Mass Mg (mg): Mass Mg (mg): Moles Mg (mol): Moles Mg (mol): AT (°C): AT (°C): Heat…
A: Experiment Mass of Mg (mg) Initial temperature ( oC) Final temperature ( oC) 1 19.8 19.1 32.9 2…
Q: Consider the reaction: ICl(g) + Cl₂(g) → ICl₃(s). The ∆G(f)° of ICl(g) is -5.5 kJ/mol and the ∆G(f)°…
A: For the given reaction: ICl(g) + Cl₂(g) → ICl₃(s) ∆G(f)° [ ICl(g)] =-5.5 kJ/mol ∆G(f)° [ Cl₂(g) ] =0…
Q: Part B: Heat of Solution Name A) For NaOH Volume of H2O used Note: density of water, dH20 = 0.997…
A: Concept ∆Hsoln=qnwhere q= heat of the solutionn= moles of solute
Q: Using values from Appendix C of your textbook, calculate the value of Ho for each of the following…
A:
Q: Given the data below, H°rxn for the reaction 2502 (g) + O2 (g) → 2SO3 (g) is kJ. AH°; (SO2 (g)) =…
A: Given Reaction 2SO2(g) + O2(g) → 2SO3(g) ∆H°f ( SO3(g) ) = - 396 KJ/mol ∆H°f ( SO2(g) )…
Q: Calculate ΔHorxn for SiO2(s) + 4 HF(g) --> SiF4(g) + 2 H2O(l) ΔHof [SiO2 (s)] = = −910.9 kJ/mol…
A: Given ΔHof [SiO2 (s)] = = −910.9 kJ/mol ΔHof [HF (g)] = −273 kJ/mol ΔHof [SiF4 (g)] = −1,614.9…
Q: Table 3. Heat of neutralization data and calculations Sample 1 Sample 2 [1] Volume of HCI (mL) 50.0…
A:
Q: Taro Peed Sarving Part C: Energy in Changes of State: C1. Mass of empty calorimeter cup with lid 6.…
A: We will use the formula q = mcΔT here where q = heat absorbed or released. m = mass of the…
Q: Find the heat change of the reaction. SO3 (g) + BaO (s) à BaSO4 (s) Substance AHf° (kJ/mol) SO3 (g)…
A:
Q: After performing the experiment related with calorimeter, we observed Temperature of hot water is 49…
A: The water equivalent of a calorimeter is defined as the mass of water that will absorb or lose as…
Q: Using values from Appendix C of your textbook, calculate the value of Ho for each of the following…
A: Given - (a) 4HCl(g) + O2(g) ----> 2 Cl2(g) + 2 H2O(g)Ho = kJ(b) 2 NO(g) ----> N2(g) +…
Q: 2NaOH + H₂SO4 → 2H₂O + Na2SO4 ΔΗ = -112 kJ 50.0 mL of 0.50 M H2SO4 is added to 60.0 mL of 0.80 M…
A:
Q: NO + O O NOle) Given the following information: As part of your answer, show how the equations can…
A: NO(g) + O(g) ---> NO2(g)
Q: Find the heat change of the reaction. CH4 (g) + 2 Cl2 (g) à CCI4 (g) + 2 H2 (g) Substance AHf…
A:
Q: The electron affinity of oxygen is -141kj/mol, corresponding to the reaction O(g)+e-—>O-(g) The…
A: The reaction takes place according to the following steps
Q: AH: (kJ/mole) AH: (kJ/mole) Component Component C3H12 (g) -143.8 -173.2 C5H12 () H2O (g) -241.8 H2O…
A: Given a reaction:- C5H12(l) + 8O2(g) → 5CO2(g) + 6H2O(g) From the table, ∆Hf of C5H12(l) = -173.2…
Q: Molar Masses A = 290.41- D = 250.53- mole E = 75.44e mole G = 117.05 X = 10.93le Z = 50.01 mole mole…
A:
Q: number of kcal
A:
Q: Part C: energy in changes of state C1. Mass of empty calorimeter cup with lid 6.835 g 107.15g 1 °C…
A: ***As per Bartleby guidelines I can solve only the first three subparts of the question. You can…
Q: When 3.50 g of CH3OCH3 is burned at constant Pressure, 110.6 kJ of heat is given off. What is AH for…
A:
Q: 5. Potassium chlorate, an ingredient in matches, reacts with sugar (sucrose) in an exothermic…
A:
Q: HBr (1 mole) CH3OC(CH,), heat
A: Protonation of etheral oxygen Formation of carbocation intermediate. Attack of nucleophile to…
Q: 1. PhMgBr, THF 2. PCC, CH2CI2 3. Os04, TBHP THF/H2O 4. Теон, PhН, heat
A: Ans
Q: Consider the reaction A→B with AH° = -71.25 kJ/molxn- What should be the AH° in kJ/molm for the…
A: Given that enthalpy of reaction A → B, is -71.25 kJ/mol We are asked to find the enthalpy of…
Q: What is the AH of the following hypothetical reaction? 2A(s) + B2(g) → 2AB(g) Given: A(s) + B2(g) →…
A:
Q: What is the missing value in the table below? Reaction ΔΗ (kJ/mol) A - B -10 B - C A - C ? kJ/mol LO
A: On adding equation 1 and equation 2, equation 3 can be obtained. A→B ...... 1B→C...... 2A→C…
Q: Reaction A (Mg + HCI) Trial 1 Trial 2 Mass of Calorimeter (g) 2.384 2.431 Mass of Calorimeter + HCI…
A: We would use given data values to calculate these values as : 1.) Mass of HCl = ( mass of…
Q: Consider the reaction of ammonia gas with O2(g) according to the thermochemical equation given…
A: ∆H is an extensive property. It depends on quantity of the substance and Stoichiometry of chemical…
Q: Use the data below to calculate the ΔG° for the reaction: 6C(s) + 3H2(g) C6H6(l) Data: 2C6H6(l)…
A:
Q: Titanium(IV) oxide is commonly used as a white paint pigment. The compound is produced by the…
A: For a chemical reaction, the enthalpy of the reaction is the difference between products and the…
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
- Table 2. Gibbs Free Energies of formation (kJ), ∆G°f, for Ions in 1M Solution and Ionic Solids Cations Cl--131.228 I--51.57 NO3--108.74 SO4-2-744.53 Ca2+-553.58 -748.1 -528.9 -743.07 -1797.28 W2 ∆G°f of water = -237.129 kJ/mol Calculated values of ∆G°rxn and the ∆Grxn of each box, Predicted results (ppt or no ppt).Observations (Rxn or No Rxn). S or support and R for Refute Cations Cl- I- NO3- SO4-2 Ca+2 helpA student investigates the enthalpy of solution, ΔHsoln, for two alkali metal halides, KCl and RbCl. Inaddition to the salts, the students has access to a calorimeter, a balance with a precision of ±0.1 g,and a thermometer with a precision of ±0.1°C.a. To measure ΔHsoln for KCl, the student adds 100.0 g of water initially at 25.0°C to acalorimeter and adds 20.0 g of KCl(s), stirring to dissolve. After the KCl dissolvescompletely, the maximum temperature reached by the solution is 55.4°C. Question : Determine the value of ΔHsoln for KCl in kJ/molrxnA student investigates the enthalpy of solution, ΔHsoln, for two alkali metal halides, KCl and RbCl. Inaddition to the salts, the students has access to a calorimeter, a balance with a precision of ±0.1 g,and a thermometer with a precision of ±0.1°C.a. To measure ΔHsoln for KCl, the student adds 100.0 g of water initially at 25.0°C to acalorimeter and adds 20.0 g of KCl(s), stirring to dissolve. After the KCl dissolvescompletely, the maximum temperature reached by the solution is 55.4°C.i. Calculate the magnitude of the heat absorbed by the solution during the dissolutionprocess, assuming that the specific heat capacity of the solution is 4.18 J/(g*°C).Include units with your answer.
- When 3.00 g of sodium hydroxide (NaOH) was dissolved in 100.00 g of water a value of 11.00oC was obtained for ΔT. 1. Calculate the molarity of the sodium hydroxide solution? _____ 2. Calculate the value (calories) for the heat of solution of 3.00 g of NaOH? ______ 3. Calculate the number of calories that would be produced if one mole of sodium hydroxide was dissolved. (ΔHsolnNaOH)? ______What is the enthalpy change when 42.0 mL of 0.350 M sulfuric acid reacts with 16.0 mL of 0.100 M potassium hydroxide? H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l) ΔH° = -111.6 kJ/mol -112 kJ -0.0893 kJ -1.82 kJ -1.64 kJ -0.179 kJIn a coffee-cup calorimeter, 1.60 g of NH4NO3 is mixed with 75.0 g of water at an initial temperature of 25.00°C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34°C. (molar mass of NH4NO3 = 80.043 g/mol) (Density of water = 1.00 g/mL) Was the dissolution process exothermic or endothermic? Assuming the solution has a heat capacity of 4.18 J/°C-g and assuming no heat loss to the calorimeter, calculate the enthalpy change (ΔHsoln) for the dissolution of NH4NO3 (remember the appropriate units forΔHsoln and pay attention to your signs)
- How does the heat or enthalpy of the reaction (ΔHrxn) change when the concentration of a Strong acid (HCl) is increasing and the concentration of strong base (NaOH) is kept constant in a solution mixture? plz answer showing the steps to solve quantatiavely using hess's law. ive also attached images of my lab data for reference8.82*10^-2 of potassium bromide has an enthalpy change of 1620J when it dissolves in water. What is the molar enthalpy of potassium bromide dissolving in water 0.018 kJ/mol 5.4*10^-5 kJ/mol 4.18 kJ/mol 18 kJ/molBased on the data given of all 3 trials given in the screenshots (if you cant see it properly click on it and download) answer these questions with step by step solution: Show the enthalpy diagram for each chemical salt when they dissolve in water. What two variables were kept constant throughout the trials and give a reason for this Thank you!
- Use Table B.11 to determine the specific enthalpy (kJ/mol HCl) of hydrochloric acid containing 1 mol HCl/5 mol H 2O at 25°C relative to:(a) HCl(g) and H 2O(l) at 25°C(b) H 2O (l) and an infinitely dilute HCl solution at 25°C.a. Calculate the amount of energy involved when 300. mL of 2.00 M NaOH is mixedwith 400. mL of 1.00 M H2SO4.(∆H°f values: NaOH(aq) = -470.114 kJ/mol, H2SO4 (aq) = - 909.27 kJ/mol,Na2SO4 (aq) = - 1390 kJ/mol, H2O (l) = - 285.83 kJ/mol)b. If both of the original solutions start at 25°C, what is the final temperature of thesolutions after the reaction? Assume no heat is lost to the surroundings, and assumethe heat capacity of the final solution is 4.2 J/g°C and that it has a density of 1.05g/mL.c. How many moles of NaOH and H2SO4 would be needed to give off 100. kJ ofenergy? Answer: a. - 33.6 kJb. 36 °Cc. 1.79 mol NaOH, 0.893 mol H2SO41. A student conducted an experiment in a Styrofoam cup calorimeter that contained 100.0 g of water at 25°C. The temperature was recorded over 2 minutes before adding 6.00 g of urea, H2NC(O)NH2(s) to the water. The temperature was recorded for another three minutes, after adding urea, with a final temperature of 21.8°C. a. Determine the change in temperature of the solution that results from the dissolution of the urea. b. According to the data, is the dissolution of urea in water an endothermic process or an exothermic process? Explain. c. Calculate the enthalpy change for the dissolution of the urea in kJ/mol. Assume that the specific heat capacity of the calorimeter is negligible and that the specific heat capacity of the solution of urea and water is 4.2 J g−1 °C−1 throughout the experiment. d. Calculate ∆H°reaction using standard enthalpies of formation. e. Compare your theoretical and experimental value