The standard enthalpy of formation (AH) is theenthalpy change that occurs when exactly 1 molof a compound is formed from its constituentelements under standard conditions. The standardconditions are 1 atm pressure, a temperature of25 °C, and all the species present at aconcentration of 1 M.A "standard enthalpies offormation table" containing AH values mightlook something like this:Part AWhat is the balanced chemical equation for the reaction used to calculate AH of BaCO, (s)?If fractional coefficients are required, enter them as a fraction (1.e. 1/3). Indicate the physical states using theabbreviation (s), (1), or (g) for solid, liquid, or gas, respectively without indicating allotrapes. Use (aq) foraqueous solution.SubstanceAHExpress your answer as a chemical equation.H(g)218 kJ/molView Available Hint(s)H2(g)O kJ/molBa(s)OkJ/molΑΣφBa2+ (aq) -538.4 kJ /molC(g)71 kJ/molC(s)O kJ/molDA chemical reaction does not occur for this question.N(g)473 kJ/molO2(g)O kJ/molSubmitO(g)249 kJ /molS2(g)129 kJ/molNext >Provide FeedbackPearsonchemistry.com/myct/itemView?assignmentProblemID=174388861

As we know enthalpy of formation of is defined as change in enthalpy associated with the formation…

The standard enthalpy of formation (AH) is the enthalpy change that occurs when exactly 1 mol of a compound is formed from its constituent elements under standard conditions. The standard conditions are 1 atm pressure, a temperature of 25 °C, and all the species present at a concentration of 1 M.A "standard enthalpies of formation table" containing AH values might look something like this: Part A What is the balanced chemical equation for the reaction used to calculate AH of BaCO3(s)? If fractional coefficients are required, enter them as a fraction (.e. 1/3). Indicate the physical states using te abbreviation (s), 1), or (g) for solid, liquid, or gas, respectively without indicating allotropes. Use (aq) for aqueous solution. Substance AH Express your answer as a chemical equation. H(g) 218 kJ/mol View Available Hint(s) H2(g) O kJ/mol Ba(s) O kJ/mol ΑΣΦ ? Ba2-(aq)-538.4 kJ /mol C(g) 71 kJ/mol C(s) O kJ/mol DA chemical reaction does not occur for this question. N(g) 473 kJ /mol O2(g) O kJ/mol Submit O(g) 249 kJ/mol S2(g) 129 kJ/mol Nex Provide Feedback P Pearson com/myct/itemView?assignmentProblemID=174388861

The standard enthalpy of formation (AH) is the enthalpy change that occurs when exactly 1 mol of a compound is formed from its constituent elements under standard conditions. The standard conditions are 1 atm pressure, a temperature of 25 °C, and all the species present at a concentration of 1 M.A "standard enthalpies of formation table" containing AH values might look something like this: Part A What is the balanced chemical equation for the reaction used to calculate AH of BaCO3(s)? If fractional coefficients are required, enter them as a fraction (.e. 1/3). Indicate the physical states using te abbreviation (s), 1), or (g) for solid, liquid, or gas, respectively without indicating allotropes. Use (aq) for aqueous solution. Substance AH Express your answer as a chemical equation. H(g) 218 kJ/mol View Available Hint(s) H2(g) O kJ/mol Ba(s) O kJ/mol ΑΣΦ ? Ba2-(aq)-538.4 kJ /mol C(g) 71 kJ/mol C(s) O kJ/mol DA chemical reaction does not occur for this question. N(g) 473 kJ /mol O2(g) O kJ/mol Submit O(g) 249 kJ/mol S2(g) 129 kJ/mol Nex Provide Feedback P Pearson com/myct/itemView?assignmentProblemID=174388861

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...

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After a few minutes on the hot plate some sodium bicarbonate (NaHCO3) begins to decompose into sodium carbonate, CO₂(g) and H₂O(g). Using standard enthalpies of formation, calculate the enthalpy change for this reaction. Use the following data. The standard enthalpy of formation for NaHCO3 is -997 KJ/Mol and sodium carbonate is -468 KJ/Mol.
nuraipy changes in chemical reactions Read through pages 18-20 in your laboratory manual for information on how to calculate the enthalpy change in a solution. Part A - Calculating ms In a calorimetry experiment 5.6 g of potassium hydroxide is dissolved in 400 mL water in a thermos flask. The temperature increase in the solution is 7 °C. The effective mass of the glass in the thermos flask (mcal) is 0.040 kg. The heat capacity of the solution (Cs) is 4.04 kJkg-¹K-1¹. The heat capacity of the calorimeter (Ccal) is 0.387 kJkg-¹K-1. Remember to enter your answer using the specified number of significant figures, but keep the entire number in your calculator for use in further calculations. Calculate the total mass of solution in kilograms (ms) Give your answer to four significant figures. ▾ View Available Hint(s) Hint 1. Calculating ms mg = mass water (kg) + mass solute (kg) —| ΑΣΦ Submit Request Answer ? kg < Pear 10
According to the following reaction, how many grams of hydrogen would be needed to produce 5.450 x 103 kJ of energy? Assume excess oxygen. Do not type units into your answer. H2(g) + 1/2 O2(g) ⟶⟶ H2O(l) Δ?=−285.83??ΔH=−285.83kJ
A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric acid. The temperature of the mixture rises 17.2 ° C. The density of the resulting solution is 1.00 g mL and has a specific heat capacity of 4.184 J g · ° C . The heat capacity of the calorimeter is 16.97 J ° C . Part 1: (a) Identify the limiting reagent for the reaction. Part 2: (b) Calculate the heat of reaction (in J). qrxn = × 10 JEnter your answer in scientific notation. Part 3 out of 3 (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization = ____ kj/mol
Measurements show that the enthalpy of a mixture of gaseous reactants increases by 214. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 62. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 significant digits. Is the reaction exothermic or endothermic? 0 kJ exothermic endothermic x10 X Ś U!! 00
I need help on part B
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What is the enthalpy change for the reaction MgO(s) + 2HCl(g) →MgCl2(s) + H2O(l)? Enthalpies of formation are −601.7 kJ/mole for MgO, −92.3 kJ/mole for HCl, −641.6 kJ/mole for MgCl2, and −285.8 kJ/mole for H2O(l).
22. Given that the enthalpy of neutralization for the reaction of HCl (a strong acid) and NaOH (a strong base) is always -55.90 kJ per mole of H2O formed, what is the concentration of a 65 mL sample of HCl if the enthalpy of neutralization for the reaction was found to be -5.38 kJ, assuming no heat is lost to the calorimeter? 0.96 M 1.48 M 1.60 M 0.38 M 4.63 M
Each year, residential homes in the United States use more than 1.05×1014 L of natural gas, which is primarily composed of methane. Calculate the total enthalpy change, Δ?methane, produced by the combustion of this volume of methane gas in kilojoules. Assume that the natural gas was stored at standard temperature and pressure. Standard enthalpy of formation values can be found in this table of thermodynamic properties. Name Formula ∆Hf ° kJ/mol Methane CH4(g) –74.6 Substance ∆Hf °kJ/mol ∆Gf°kJ/mol S°J/(mol·K) CH4(g) –74.6 –50.5 186.3
In an endothermic reaction the enthalpy of the reactants is greater than the enthalpy of the products. In an endothermic reaction, the energy required to break existing bonds is more than the energy released when new bonds form. In an exothermic reaction the energy required to break existing bonds is less than energy released when new bonds form. In an exothermic reaction the potential energy of the reactants is higher than the potential energy of the products and the energy term would be written on the product side of the equation.
26. Calculate the enthalpy change for the reaction below. NO(g) + O(g) →→→ NO₂(g) Given following data: NO(g) + O₂(g) →→ NO₂(g) + O₂(g) 03(g) → 1.50₂(g) 0₂(g) →20(g) AH-198.9 kJ AH = -142.3 kJ ΔΗ = 495.0 kJ