Use and modify some/all the reactions provided to form the indicated overall reaction according to Hess' Law. • If a reaction is not used in your Hess' Law process, include that indication by multiplying the reaction by "0" • If no modification is needed and the reaction is applied as written below, include that indication by multiplying the reaction by "1" • Use whole numbers and simple fractions (such as "2" or "1/2", not 0.5) and negative signs (such as "-2") where needed Then calculate and report the enthalpy change (in kJ) for the overall reaction in the indicated blank, including units with your written value and rounded to 1 decimal place. Overall Reaction: CS2(1) + 302(g) → CO2(g) +2SO2(g) Rxn # Reaction ΔΗ° (kJ) 1 C(s) → C(g) 716.67 2 C(s) + O2(g) → CO2(g) -393.5 3 3Fe(s) +202(g) → Fe3O4(s) -1118 4 C(s) + 2S (s) → CS2(1) 87.9 5 CH4(g) + O2(g) → CO2(g) + H₂O(g) -882.0 S(s) + O2(g) → SO2(g) -296.8 N2(g) + 4H2(g) + Cl2(g) → 2NH4Cl(g) -629.1 6 7

Use and modify some/all the reactions provided to form the indicated overall reaction according to Hess' Law. • If a reaction is not used in your Hess' Law process, include that indication by multiplying the reaction by "0" • If no modification is needed and the reaction is applied as written below, include that indication by multiplying the reaction by "1" • Use whole numbers and simple fractions (such as "2" or "1/2", not 0.5) and negative signs (such as "-2") where needed Then calculate and report the enthalpy change (in kJ) for the overall reaction in the indicated blank, including units with your written value and rounded to 1 decimal place. Overall Reaction: CS2(1) + 302(g) → CO2(g) +2SO2(g) Rxn # Reaction ΔΗ° (kJ) 1 C(s) → C(g) 716.67 2 C(s) + O2(g) → CO2(g) -393.5 3 3Fe(s) +202(g) → Fe3O4(s) -1118 4 C(s) + 2S (s) → CS2(1) 87.9 5 CH4(g) + O2(g) → CO2(g) + H₂O(g) -882.0 S(s) + O2(g) → SO2(g) -296.8 N2(g) + 4H2(g) + Cl2(g) → 2NH4Cl(g) -629.1 6 7

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

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.70 kg of water at 37.5C. During the reaction 92.8kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. Heat capacity of water is 4.18J.g-1.K-1. Round your answer to 3
4.0g of Colorado oil shale is burned in a bomb calorimetre. The combustion of the soil shale causes the temperature of the calorimetre to increase by 5.0 degrees. The calorimetre contains 1.00 kg of water and the heat capacity of the empty calorimetre is 100J/degrees. How much heat is released per gram of oil shale when it is burned? Please write in simple form and break down with equations.
please don't provide hand written solution....
The G.R.A.S.P. method
3. During the experiment, when calculating AH using the formula AH=C x AT, can we calculate the AH without measuring the amount of water that we put inside the calorimeter? Explain why or why not. (max of 5 sentences) 4. You accidentally forgot to measure the mass of the octane that you transferred in the crucible. You already started the calorimeter and it is too late to stop the equipment. Is it still possible to calculate the energy (in Joules) of octane? Explain.(max of 2 sentences)
1. What is the final overall reaction for these three reactions below? Reaction 1: C3 Hs (g) + 5 O2 (g) → 3 CO2 (g) +4 H2O (g), AH1 = -2043 kJ Reaction 2: C (s) + O2 (g) Reaction 3: 2 H2 (g) + O2 (g) + CO2 (g), AH2 = -393.5 kJ 2 H2O (g), AH3 -483.6 kJ Hint. Reverse Reaction 1 then simplify by cancelling compounds in opposite sides of the arrow.
An increase in temperature drives an endothermic reaction toward the reactants. True False
One proposed source of clean energy is the combustion of hydrogen in the presence of oxygen. This reaction releases a significant amount of energy, and the only product of the reaction is water. The balanced chemical equation is shown here: 2H₂(g) + O₂(g) →→→ 2H₂O(g) + energy
Use these three reactionsCH4(g) + 2 O2(g) −→ CO2(g) + 2 H2O(g)∆H◦ = −802 kJCH4(g) + CO2(g) −→ 2 CO(g) + 2 H2(g)∆H◦ = 247 kJCH4(g) + H2O(g) −→ CO(g) + 3 H2(g)∆H◦ = 206 kJto determine the appropriate enthalpy change ofCH4(g) + 3/2O2(g) −→ CO(g) + 2 H2O(g). Choose the correct answer: 1. −200 kJ 2. −330 kJ 3. −520 kJ 4. −600 kJ 5. −810 kJ 6. −843 kJ 7. −349 kJ 8. −450 kJ 9. −761 kJ
Metal carbonates react with acids to form the salt of the metal and two other products, a gas and a liquid. Complete the balanced reaction of hydrochloric acid with an unknown carbonate below.
The nutrition label tells us that 13 g of a serving of gummy bears (i.e. 10 gummy bears) is made of sugars. Let's assume that all of the sugar is sucrose. The unbalanced reaction for the combustion of sucrose is given below. How much heat is released from the combustion of the sucrose in a single gummy bear? 2C12H22O11+24O2→24CO2+22H2OΔHrxn=−11,286kJ Heat in kJ:
How much heat will be given off when 18.5 g of C,H, is bumed in oxygen to form CO2ig) and H,O(g)? For the reaction: C2Hal@) + 3 O2ig) + 2 CO2(9) + 2 H2Oa) + 316 kcal