Given the following reactionsReactionsEnthalpies of ReactionNa(s) +-2Cl2(g) Na(g) + CI(g)AH = 269 kJNa(g) + Cl(g) Na*(g) + CI(g)AH = 182 k)Na(s) +Cl2(g)NaCl(s)AH = -445 k)%3DUse Hess' Law to determine the AH for the following reaction: (watch your states and chargesNa*(g) + Cl(g)→NaC(s)kJShow your work:Graph to add drawings to:

Determine the ∆H for the reaction, Na+(g) + Cl-(g) -----> NaCl(s) ∆H = ?

Given the following reactions Reactions Enthalpies of Reaction Na(s) + Cl2(8) Na(g) + Cl(g) AH = 269 kJ Na(g) + Cl(g) Na*(g) + Cl(g) AH = 182 k) Na(s) + 1 Cl2(8) NaCl(s) 445 k) AH = Use Hess' Law to determine the AH for the following reaction: (watch your states and charge Na*(g) + Cl'(g) → NaC(s) kJ Show your work: Graph to add drawings to:

Given the following reactions Reactions Enthalpies of Reaction Na(s) + Cl2(8) Na(g) + Cl(g) AH = 269 kJ Na(g) + Cl(g) Na(g) + Cl(g) AH = 182 k) Na(s) + 1 Cl2(8) NaCl(s) 445 k) AH = Use Hess' Law to determine the AH for the following reaction: (watch your states and charge Na(g) + Cl'(g) → NaC(s) kJ Show your work: Graph to add drawings to:

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

Below are the equations of interest in this laboratory exercise. As you know from reading the laboratory handout, your goal is to determine the enthalpy change for reaction 1. (1) Mg(s) + 1/2O2(g) → MgO(s) ∆H1 = ∆Hf(MgO) = ? (2) Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g) ∆H2 (measured) (3) MgO(s) + 2H+(aq) → Mg2+(aq) + H2O(I) ∆H3 (measured) (4) 1/2O2(g) + H2(g) → H2O(l) ∆H4 = -286.0 kJ/mol To arrive at equation (1) from the others equation (2) needs to be (pick one) Select one: a. kept the same b. multiplied by 2 c. reversed d. reversed and multiplied by 2
just need the final answer
Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2NH3(g) + 3N₂O(g) → 4N2(g) + 3H₂O(g) AH (NH3 (9))=-46.1 kJ/mol AH (N₂O(g)) 82.1 kJ/mol AH (N₂(9))= 0.0 kJ/mol AH (H₂O(g))=-241.8 kJ/mol AH rxn kj
Use the following information to determine the enthalpy for the reaction shown below. CS2() + 302(g) → CO2(g) + 2SO2(g) C(graphite) + O2(g) CO2(g) S(s) + O2(g) SO2(g) C(graphite) + 2S(s) CS2() AH = -393.5 kJ AH =-296.8 kJ AH = 87.9 kJ Select one: a. -899.2 kJ b. +1075.0 kJ C. -778.2 kJ d. -1075.0 kJ e. +778.2 kJ
Below are the equations of interest in this laboratory exercise. As you know from reading the laboratory handout, your goal is to determine the enthalpy change for reaction 1. (1) Mg(s) + 1/2O2(g) → MgO(s) ∆H1 = ∆Hf(MgO) = ? (2) Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g) ∆H2 (measured) (3) MgO(s) + 2H+(aq) → Mg2+(aq) + H2O(I) ∆H3 (measured) (4) 1/2O2(g) + H2(g) → H2O(l) ∆H4 = -286.0 kJ/mol To arrive at equation (1) from the others equation (3) needs to be (pick one) Select one: a. kept the same b. multiplied by 2 c. reversed d. reversed and multiplied by 2
Ba(OH)2 8H20(s) + 2NH4NO3(aq) → Ba(NO3)2(aq) + 2NH3(aq) + 10H20(1). 0.25 g of Ba(OH)2 8H20 is added to a coffee cup calorimeter containing 200.0 mL of 0.01 M NH4NO3, changing the temperature from 25.00°C to 24.84°C. If the density of the solution is the same as water and its specific heat is 4.184 J/g°C, what is the enthalpy of the reaction (kJ/mol)? Assume the volume of the solution does not change.
Look at the image.
A chemist measures the enthalpy change AH during the following reaction: P4(s) + 6 Cl,(g)→4 PCI3(g) AH=-1148. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ 2 1 -P -PCl, (g) s) + Cl, (g) kJ 3 4PCI, (g) - P, (s) + 6Cl, (g) | kJ 1 3 (s) + 4 Cl, (g) PCI, (g) kJ
Using Hess's Law to calculate net reaction enthalpy Nitric oxide (NO) can be formed from nitrogen, hydrogen and oxygen in two steps. In the first step, nitrogen and hydrogen react to form ammonia: N2(9) + 3 H,(9) → 2 NH3(g) AH=-92. kJ In the second step, ammonia and oxygen react to form nitric oxide and water; 4 NH,(g) + 50,(g) → 4NO(g) + 6 H,O(g) AH=-905. kJ Calculate the net change in enthalpy for the formation of one mole of nitric oxide from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ.
calculate the standard enthalpy change (in kJ/mol) for each of the following reactions. (a) 2 Na(s) + I2(g) → 2 NaI(s) _______________kJ/mol (b) Cr2O3(s) + 3 H2(g) → 2 Cr(s) + 3 H2O(l) ___________kJ/mol (c) 2 KOH(s) + CO2(g) → K2CO3(s) + H2O(g) _________________ kJ/mol (d) Na(s) + O2(g) → NaO2(s) _____________kJ/mol
4 CH3NH2 (g) + 2 H2O (l) ➝ CO2 (g) + 3 CH4 (g) + 4 NH3 (g) ΔHº = –138.96 kJ• Calculate the overall change in enthalpy when 30.00 grams of CH3NH2 (g) reacts with excess H2O (l). [Be sure to include the correct sign.]
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K kJ HopHelpCh5N1