Calculate enthalpy changes for the following:a. 0.084 g of sulfur (rhombic) burns, formingSO2(g) (AfH forSO2(g) = 296.84 kJ/mol)==Enthalpy changeb. 0.23 mol ofd.c. 3.07 g ofHgO(s) decomposes toHg() andO2(g) (AfH forHgO -90.83 kJ/mol)Enthalpy change ==NH3(g) is formed fromN₂(g) and excessH₂(g) (AfH forNH3=-45.90 kJ/mol)Enthalpy change =kJkJkJ1.76 x 10-2 mol of carbon is oxidized toCO2(g) (AfH forCO2 = -393.509 kJ/mol)Enthalpy change[Review Topics]kJ

Answered: Image /qna-images/answer/a733f6ce-034f-446c-8f2a-7f360fa0f22c.jpg

Calculate enthalpy changes for the following: a. 0.084 g of sulfur (rhombic) burns, forming SO2(g) ( AfH for SO2(g) = 296.84 kJ/mol) - Enthalpy change = = b. 0.23 mol of HgO(s) decomposes to Hg(l) and O2(g) ( AfH for HgO = -90.83 kJ/mol) Enthalpy change = kJ kJ

Calculate enthalpy changes for the following: a. 0.084 g of sulfur (rhombic) burns, forming SO2(g) ( AfH for SO2(g) = 296.84 kJ/mol) - Enthalpy change = = b. 0.23 mol of HgO(s) decomposes to Hg(l) and O2(g) ( AfH for HgO = -90.83 kJ/mol) Enthalpy change = kJ kJ

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...

See similar textbooks

Similar questions

Using the reaction enthalpy data shown, determine the amount of heat released in each situation: 2 Ca (s) + O2 (g) ----> 2 CaO (s) ΔHrxn = -1,269.8 kJ a.) If excess calcium reacts with 3 moles of O2? b.) If 8 moles of calcium react with excess O2? c.) If calcium and oxygen react to form 1 mole of CaO?
The enthalpy of reaction is -11.7 kJ/mol for the following reaction: HCN(aq) + NaOH(aq) --> H2O(l) + NaCN(aq) If 0.541g of HCN react with excess NaOH in a coffee cup calorimeter, what amount will the temperature change by? Use 63.5 g as the total mass in the calorimeter and use 4.184 J/gC as the specific heat. Give your answer to 2 decimal places.
10. Calculate the standard enthalpy of formation of N₂O5 from the following data: kJ mol kJ 2NO(g) + O₂(g) →2NO₂(g) 4NO2(g) + O₂(g)→2N205(g) N₂(g) + O₂(g) →2NO(g) 4,H☺ = -114.1 = -110.2- 'mol kJ mol AH AH = + 180.5,
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300.g of water (see sketch at right). First, a 6.000g tablet of benzoic acid C6H5CO2H is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of /26.454kJg .) The temperature of the water is observed to rise from 14.00°C to 39.98°C over a time of 14.9 minutes. Next, 5.570g of acetylene C2H2 are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 14.00°C to 60.18°C . Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. →+2C2H2g 5O2g + 4CO2g 2H2Og Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students:…
Given the standard enthalpy changes for the following two reactions: ΔΗ° (1) N₂(g) + 2O2 (g) → 2NO2 (g) (2) 2N₂O(g) → 2N2(g) + O2(g) ΔΗ° = 66.4 kJ Standard enthalpy change : = - 164.2 kJ What is the standard enthalpy change for the following reaction? (3) 2N₂O(g) + 3O2 (g) → 4NO2 (g) AH° =? kJ
Find the enthapy change for the reaction below in kJ . 4NH3(g) + 5O2(g) --> 4NO(g) + 6H2O(g) ΔH= ? Given : (NH3(g)) = -46.1, (NO(g)) = + 90.3 kJ/mol and (H2O(g)) = -241.8 kJ/mol.
Consider the following two reactions and write down the balanced chemical equations. Reaction 1: Formic acid (CH202, ) reacts with oxygen to produce liquid water and carbon dioxide gas. The enthalpy change for this reaction is A,H= -255 kJ mol-1 (per mole of CH202). Reaction 2: The formation reaction for CO2(g). The enthalpy of formation for CO2(g) is A:H= -394 k) mol-1 Given the data above, what is the enthalpy of reaction for: C(gr) + H,O(1) +0,(g) → CH, O,(1) A,H = Number kJ mol-1 %3D
Calculate the standard enthalpy for the below reaction (in kJ) using the standard enthalpies of formation provided: Reaction: 5 A + 3 B ⟶⟶ 7 C + 3 D Standard enthalpies of formation, ΔH°f (in kJ/mol) are: A: ‑15.7 B: ‑86.4 C: ‑52.7 D: ‑71.6
Given the following two reactions:(1)Fe(s) + Cl2(g)->FeCl2(s) H(1) = -341.8 kJ(2)Hg(l) + Cl2(g)->HgCl2(s) H(2) = -224.3 kJcalculate the enthalpy change for the following reaction:(3) FeCl2(s) + Hg(l)-> Fe(s) + HgCl2(s) H(3) = kJ
How much heat is produced when 0.480 mol of methane is burned under standard conditions. Enthalpy of combustion of methane = -891 kJ/mol. - A) -891 kJ B 428 kJ -222 kJ -644 kJ -428 kJ
Please don't provide handwritten solution ....
20) The standard enthalpy change for the reaction below is -196.0 kJ. Use Table below to calculate the standard enthalpy of formation of H₂O (1). 2H₂O2 (1) ->>> 2H₂O (1) + O₂ (g) Substance H₂O2 (1) AH° (kj/mole) -187.8