7 salt packs data sheet

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.

q- mcAT Substance aJ kgK Substance cIJ kg"K Aluminium 900 Ice 2100 Iron/steel 450 Wood 1700 Copper 390 Nylon 1700 Brass 380 Rubber 1700 Zinc 380 Marble 880 Silver 230 Concrete 850 Mercury Tungsten 140 Granite 840 135 Sand 800 Platinum 130 Glass 670 Lead 130 Carbon 500 Hydrogen 14000 Ethanol 2400 Air 718 Paraffin 2100 Nitrogen 1040 Water 4186 Steam 2000 Sea water 3900 How much heat (J) must be added to a 50.0 g sample of zinc if the temperature increases from 20 C to 25 °C? a) b) If 500.0 J of heat must be added to a sample of carbon in order to increase the temperature by 10*C, what is the mass (kg) of the sample of carbon? c) If it takes 450.0 J of heat to raise the temperature of 0.05 kg of an unknown metal by 25°C, what is the specific heat of the metal (?

What is the change in enthalpy when 4.04 grams H₂ reacts with excess oxygen according to the following balanced chemical reaction: STARTING AMOUNT -572 mol H₂ ADD FACTOR X -572 g 0₂ X 1 kJ 2 H₂(g) + O₂(g) → 2 8.08 ΔΗ = -572 1144 g H₂O 32.0 kJ 2 = H₂O(l) ANSWER -1144 mol O₂ 18.02 mol H₂O RESET J 5 -286 4.04 9 +

Table 4. Enthalpy of solution of salts data and calculations NHẠNO3 MgSO4 [1] Mass of salt (g) 1.991 2.000 [2] Volume of DI water (mL) 49.9 49.8 Mass of DI water (g) [3] Temperature of DI water (°C) 25.0 24.4 [4] Temperature of mixture after dissolution (°C) 21.7 32.5 Temperature difference (°C) [5] Total mass in reaction (g) [6] Enthalpy of solution AHsolution (cal/mol)

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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

Sign in to your account 101 Chem101 b My Questions | bartleby x + app.101edu.co C Update : Question 32 of 37 Submit What amount of heat, in kJ, would be involved in condensing 19.1 g of CH;OH? (AHvap = 38.0 kJ/mol) 22.6 kJ 1 2 3 6 C 7 8 9. +/- x 100 + 4+

In lab, a student weighed out 3.569 g of an unknown salt. Her coffee cup calorimeter weighed 35.638 g. After adding water it weighed 81.73 g. Before the addition of salt, the temperature of the water in the coffee cup was 17.8d e g r e e s C. After all the salt dissolved the maximum temperature was 14.5d e g r e e s C. Calculate the enthalpy of solution for the salt, d e l t a H o f s o l u t i o n. Report your answer in J.

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CALORIMETRY DATA DETERMINATION OF THE ENTHALPY OF REACTION OF NITRIC ACID AND SODIUM HYDROXIDE Molarity of nitric acid, M 1.00 Volume of nitric acid, mL 10.00 Molarity of sodium hydroxide, M 1.00 Volume of sodium hydroxide, mL 5.00 Initial Temperature (°C) 26.7   Time (sec) Temperature of mixture (°C) 0 26.7 30 27.8 60 29.0 90 29.0 120 29.0 150 29.0 180 29.0 210 29.0   Solve for: Final Temperature (°C) ΔT (°C) ΔH (J/mol) ΔH (kJ/mol)

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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T STARTING AMOUNT X 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: -572 mol H₂ ADD FACTOR x( ) 458 g 0₂ 1 kJ 2 H₂(g) + O₂(g) →→ 2 H₂O(l) ΔΗ = -572 715 2 g H₂O 1.25 kJ ANSWER 18.02 mol O₂ -458 2.02 mol H₂O RESET J 5 -715 32.0 g H₂

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

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.

INTRODUCTION LABORATORY SIMULATION PHASE 3: Lab Data - X Calculate AHneutralization 37.2°C Complete the following steps: Concentration of hydrochloric acid (M) 2.09 Concentration of sodium hydroxide (M) 2.07 1 Calculate solution mass. Record in Lab Data Calorimeter constant (J/°C) 13.7 Volume of hydrochloric acid (mL) 2 Calculate moles of hydrogen ion (H*). 96.6 Record in Lab Data Temperature of hydrochloric acid (°C) 23.0 Volume of sodium hydroxide (mL) 3 Calculate moles of hydroxide ion (OH'). 98.1 Record in Lab Data Temperature of sodium hydroxide (°C) 23.0 Identify limiting reactant. Record in Lab Data 4 Final temperature after mixing (°C) Wash/Waste 37.2 Mass of mixed solution (g) Moles of H* (mol) 5 Calculate AHneutralization: Record in Lab Data Moles of OH- (mol) Limiting Reactant AHneutralization (kJ/mol) HCI Hydrochloric acid N2OH Sodium hydroxide How to calculate the enthalpy of neutralization oFF SPEED МЕТНODS RESET MY NOTES LAB DATA SHOW LABELS GO TO PHASE 4 PHASES

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

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