7 salt packs data sheet

I need help finding the enthalpy of MgSO4. Thanks

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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+

Initial calorimeter mass, m, 13.366 g Calorimeter mass + water, m2 110.90 g Calorimeter mass + water + ice, mg 129.18 g Average initial water temperature, Tintal 27.4 °C Minimum water temperature, Tmnimum or Tmin 11.4 "C Change in water temperature, ATcool Tmin - Tinitital %3D "C Submit Request Answer

Calorimeter mass  162.2 g Mass of calorimeter + cold water 226.6 g Initial temperature of cold water 22°C Temperature of hot water before mixing 85°C Final temperature of the mixture 46°C Mass of calorimeter + mixture 302.7 g Specific heat of water = 1cal/ g °C10- ∆T H2O = ( Tm - T H2O cold) = ______________________________________11- ∆T H2O = ( Tm - T H2O hot) =___________________________________12- ∆T ° C = ∆T cold H2O:_________________________________________________13- Mass of cold water: = ( calorimeter mass + cold H2O - empty calorimeter mass):____14- Mass of hot water = ( mass of calorimeter + mixture) - ( mass of calorimeter + cold water) =.

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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:

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)

.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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is number 9 correct?

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

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

r STARTING AMOUNT X What is the change in enthalpy when 0.600 moles of H₂O are produced according to the following balanced chemical reacton: 27.67 ADD FACTOR x( ) 407 g B₂03 mol B,O B₂H₂(g) + 3 O₂(g) → B₂O₂(s) + 3 H₂O(g) 69.62 Question 35 of 35 32.00 g B₂H ΔΗ = -2035 -2035 -407 g 0₂ J kJ 1 ANSWER 1.22 x 10³ kJ mol B₂H 0.600 -1.22 x 10³ g H₂O 3 RESET 5 mol O₂ 18.02 mol H₂O Submit +

Part B. Enthalpy Change (HCI - MgO) Mass of beaker and MgO (g) Mass of empty beaker (g) Mass of magnesium oxide used (g) Mass of inner cup and solution (g) Mass of empty inner cup (g) Mass of solution (g) Initial temperature of solution (°C) Temperature (°C) after 30 seconds 60 seconds 90 seconds 120 seconds 150 seconds 180 seconds Final temperature of solution (°C) Molar enthalpy of reaction (kJ mol¹) Average AH (kJ mol¹) Experimental AH for the reverse reaction A Trial 1 3.210 52.456 4.623 21.4 26.4 27.1 28.2 28.2 28.1 28.0 Trial 2 3.010 52.050 4.623 21.0 25.7 26.4 27.7 28.5 28.5 28.5 Trial 3 2.890 53.000 4.500 20.0 24.8 24.8 24.9 24.6 24.5 24.4 Trial 4 2.910 53.000 4.500 20.0 23.7 23.8 24.0 24.2 24.4 24.6 Heat capacity of calorimeter (J/oC) Specific heat of solution (J/goC) Activate Windows 2.1 4.17

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

The heat evolved from the combustion of 0.94g ethanol raises the temperature of 250 cm3 water contained in a copper beaker by 20.0 °C. [Specific heat capacity of solution = 4.18 Jg-1 °C-1; density of solution = 1.0 g cm-3] i) What is the enthalpy of combustion per mol of ethanol?ii) Calculate the temperature rise when 1.50 g ethanol is used to heat 500 cm3 water in the same copper beaker.

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D (35) W X O PRINC x C Men's x B CHEM X 101 Chem X C An Exo X C An Enc x If 801 A How d X S If reac X C A Bom A app.101edu.co Question 27 of 27 How many grams of CHe liquid must decompose according to the following chemical equation to transfer 430 kJ of heat? CH6(1) - C,H2(g) AH = 630 kJ STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 1 630 78.12 2.15 x 107 3 0.001 53.3 430 1000 17.8 6.022 x 1023 160 26.04 mol CH2 g CHe mol CeHe kJ g C,H2 J

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

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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

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