7 salt packs data sheet

I need help finding the enthalpy of MgSO4. Thanks

5. The enthalpy of solution for the dissolving of a KBr sample was determined following Part C of the Experimental Procedure in this experiment. Complete the following table for Trial 1 for determining the enthalpy of solution of KBr. 1. Mass of salt (g) 2. Moles of salt (mol) 5.00 3. Mass of water (g) 25.0 25.0 4. Initial temperature of water (°C) 5. Final temperature of water (°C) Calculations for Enthalpy (heat) of 18.1 Solution for the Dissolution of a Salt 1. Temperature change of solution, AT (°C) 2. Heat change by water (J) Show calculation. 3. Heat change of salt (J); specific heat capacity of KBr = 0.439 J/g.°C) 4. Total enthalpy change (J) Equation 25.11. Show calculation. 5. AH, (J/mol salt) Equation 25.12. Show calculation.

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+2 -3 a. solid calcium nitride plus heat Ca Na 3 Ca +2N b. solid lead (IV) carbonate plus heat рысозда 1→→ Pb 0₂ + 2003 c. solid chromium (III) sulfate hexahydrate plus heat d. sodium metal plus nitrogen gas

2. Use Hess's law and the following set of reactions: a) N2H4 (1) + 02 (1) b) H2(g) H2 (g) + O2 (g) → H2O (1) N2 (g) + 2H2O (1) AH=-622.2 kJ AH=-285.8 kJ AH=-187.8 kJ c) H2(g) + O2 (g) → H2O2 (1) to calculate the AH for the reaction N2H4 (1) + 2H2O2 (1) >N2 (g) + 4H2O (1) Solution:

.CO Aktiv Chemistry What is the change in enthalpy when 1.25 moles of O₂ are reacted with an excess H₂ of according to the following balanced chemical reaction: 2 H₂(g) + O₂(g) → 2 H₂O(l) ΔΗ = -572 kJ -572 mol H₂ ADD FACTOR x ( ) 458 g 0₂ 1 kJ Question 19 of 20 715 2 g H₂O 1.25 ANSWER 18.02 mol O₂ DELL -458 2.02 mol H₂O RESET J 2 -715 32.0 g H₂ TEL

Molar Masses A = 290.41 D = 250.53– 9 %3D E = 75.44 9 %3D mole mole %3D mole G = 117.05 X = 10.93 Z = 50.01 mole mole mole If 18.23 g A, according to the balanced thermochemical equation below, how much heat (in kJ) is absorbed? 5 A+6 D→ 5 Z +5G AH = 515 kJ Please input your answer to the second decimal place Type your answer...

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Experiment 4. Determining the specific enthalpy of fusion of water (latent heat) 32. Mass of calorimeter 6.616 57.202 g Mass of calorimeter and water 48.586 9 33. Mass of water 72.585g 34. Mass of calorimeter, water, and ice 35. Mass of ice added 5.383 g. 36. Initial temperature water 9.4 °C Initial temperature ice °C 1.9 37. Final calorimeter temperature °C 38. ATcalorimeter-water 255.64 K Ccalorimeter-water 39. ATice-water K qice-water J 40. qice (= AH°) 41. AHusion of ice J/g %-difference fusic 3.

NaOH(s) trial (A) NHẠNO3 (s) trial (B) Part 2: Enthalpy of dissolution a. Mass of substance dissolved (g) b. Mass of calorimeter (g) c. Mass of calorimeter + water (g) d. Mass of water (g) 0.8314 0.7985 2.114 2.179 11.9717 12.0731 e. Total mass of reactants (g) f. Initial temperature of water (°C) g. Final temperature of solution (°C) h. Change in the temperature, AT (°C) i. Moles of solid dissolved in water (mols) j. Heat lost or gained by the water, Aqm (J) k. Heat absorbed by the calorimeter, Aq. (J) I. Heat absorbed or released by the dissolving solute Aq: = Aqm+ Aqc (J) m. Enthalpy of solution, AHrxn (kJ/mol) n. Theoretical enthalpy, calculated AHrxn (kJ/mol) 18.0 18.2 30.0 13.6 o. Percent error

Mass of eat empty calorimeter 5.10g Mass of calorimeter and HCl solution 54.29g Calculated mass of HCl solutions/₂49.699 Initial temperature of HCI Solution Initial temperature of NaOH solution Final temperature of the solution Mass of the calorimeter and solution Calculated mass of NaOH solution AT For HCl solution AT for NaOH Solution Run 1 14,2°C 20.2°C 3. The number of moles of NaOH used. 24.0°C 104.959 50.16g 4.8°C 4. The number of moles of HCI used. Show Transcribed Text Part 4: Reaction 3 NaOH(aq) + HCl(aq)→ NaCl(aq) + H₂0(1) 1. The heat energy change of the calorimeter. 104.62g 50.43д 4,0°C 3,8°C hack mittarity of the calor 3.8°C Run 2 2. The heat energy change of the HCI solution, and the heat energy change of the NaOH solution, and the total heat energy change of both solutions. 5. The enthalpy of reaction. Also calculate the average enthalpy. 5.139 54.199 49.069 20.8°C 21.00C 24.8°C

A solution is made by mixing 287.0 mL287.0 mL of ethanol initially at 13.1 ∘C13.1⁢ ∘C with 287.0 mL287.0 mL of water initially at 22.0 ∘C22.0⁢ ∘C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL0.789 g/mL and the density of water is 1.00 g/mL1.00 g/mL. The specific heat of ethanol is 2.46 J/g·°C2.46 J/g·°C and the specific heat of water is 4.184 J/g·°C4.184 J/g·°C.

Solve for 6,7 and 8 please . Significant figures matter

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Question 6 Which of the following graph represents the change in the Potential Energy (PE) of the particles in the system when the substances undergoes the change corresponding to path I? PE с A D B Pressure (atm) A 10³ 10² 10¹ P 10-1 10-² 10-3 Т IV PE 20 ||| || 40 B C PE Т TREF 60 Temperature (K) 80 Т 100 PE D Т

Use the data table below, complete only Reaction B of the Post Lab Questions.

1edu.co ng Ce... R 4 F5 The heat liberated when 3 moles of methane (CH4) are burned in an excess amount of oxygen is kJ. 5 F6 CH4 (g) + 2 O2 (g) → CO₂ (g) + H₂O (1) AH = -890 kJ A) 1335 B) 2670 C) 1780 D) 890 F7 F8 Question 5 of 5 & Given the equation: 7 DELL F9 8 F10 ( F11 ) F12 PrtScr

You want to heat the air in your house with natural gas ( CH4 ). Assume your house has 275 m2 of floor area and the ceilings are 2.5 m from the floor.  Data for air: Cp (J/mol K) 29.1 Density (g/L) 1.22 Average molar mass (g/mol) 28.9   Calculate the mass of air (in grams) to be heated.  Calculate the amount of heat (in megajoules) required to increase the temperature of this mass of air from 15°C to 22°C.   If the energy density of CH4 is 55.5 MJ/kg, what is the mass of CH4 needed to heat your house?

على ملي OEt C مسلم A Ph 1. (Et)₂CuLi 2. 30* NaOEt EtOH H Ph heat CN-H [H"] 2. B 3. H3O, heat E D OEt H3O*, heat NaOEt EtOH heat

A coffee cup calorimeter with a heat capacity of 3.70 J/°C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL solution of 0.330 M AgNO3 was mixed with 50.0 mL of 0.190 M KI. After mixing, the temperature was observed to increase by 2.53 °C. Calculate the enthalpy of reaction, AHrxn, per mole of precipitate formed (AgI). Assume the specific heat of the product solution is 4.12 J/(g° C) and that the density of both the reactant solutions is 1.00 g/mL. 3 Calculate the theoretical moles of precipitate formed from AgNO3 and KI. theoretical moles of precipitate formed from AgNO3: theoretical moles of precipitate formed from KI: 0.0095 moles moles

uestion 12 of 23 The temperature of a sample of iron increased by 23.4 °C when 269 J of heat was applied. Substance Specific heat J/(g °C) lead 0.128 What is the mass of the sample? silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 m = g about us privacy policy terms of use contact us help careers home ort sc delete Dum backspace lock 8. enter pause B M 立

eM Gmail (16) Ayurveda | Anc. Bloated Belly After... rinding a [References] In a coffee-cup calorimeter, 140.0 mL of 1.4 M NAOH and 140.0 mL of 1.4 M HCl are mixed. Both solutions were originally at 23.7°C. After the reaction, the final temperature is 33.1°C. Assuming that all the solutions have a density of 1.0 g/cm and a specific heat capacity of 4.18 J/ C g, calculate the enthalpy change for the neutralization of HCI by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. AH= kJ/mol

Sign in to your account 101 Chem101 PLEASE HELP ASAP!! | bartleby x + app.101edu.co Update : Question 25.a of 37 Submit A 389.3 gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C. (heat capacity of solid = 2.96 J/g°C; heat capacity of liquid = 1.75 J/9•°C; AHfus = 8.04 kJ/mol; normal freezing point, Tf = 17.6 °C) How much energy (in kJ) is absorbed/released to heat the solid? kJ 1 2 3 6 C 7 8 9 +/- х 100 + 4+