* Given the Changes forthe following twoStandard enthalpytwo reactions:1) 4C (s) + 6H₂ (g) → Cn H₁0 (9) A°= -125600tallins*2AH° = -52.3k5COM2) **C₂ H₂ (g) → 2C(s) + 2 H₂ (9)14*what is the stadard enthalpy change for thereaction :C3) 20₂ H₁₂ (9) + H₂ (9) -> (4 H10 (9) AH`= ?KJ*

-> When reaction is multiplied with any constant then enthalpy also multiplied. ->When…

* Given the Standard enthalpy changes for the following two reactions: 1) 4C (s) + 6H₂ (g) → C₂ H₁0 (9) AH = -12565 2) **C₂ H₂ (g) → 2C(s) + 2 H₂ (9) EN JA *what is the stadard enthalpy change for the reaction: I *2 AH = -52.345 3) 20₂ H₁4 (9) + H₂ (9) -> (4 H₁0 (9) AH` = ? C KJ *

* Given the Standard enthalpy changes for the following two reactions: 1) 4C (s) + 6H₂ (g) → C₂ H₁0 (9) AH = -12565 2) **C₂ H₂ (g) → 2C(s) + 2 H₂ (9) EN JA what is the stadard enthalpy change for the reaction: I 2 AH = -52.345 3) 20₂ H₁4 (9) + H₂ (9) -> (4 H₁0 (9) AH` = ? C 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

Hydrogen peroxide, H2 O2, is a colorless liquid whose solutions are used as a bleach and an antiseptic. H2 O2 can be prepared in a process whose overall change is H2 (g) + O2 (g) –→ H2O2 (1) Calculate the enthalpy change using the following data: 2H2О2(1) — 2H,0() + О-(9); дн: -196.0 kJ На (9) + 3 О2(9) > H20(1); дН — — 285.8 kJ = - ΔΗ - kJ
just need the final answer
Use only 1 decimal for the Final answers. From the following enthalpies of reaction: 4 HCl(g) + O2(g) → 2 H2O(l) + 2 Cl2(g) ΔH = -202.4 kJ/mol 1/2 H2(g) + 1/2 F2(g) → HF(l) ΔH = -600.0 kJ/mol H2(g) + 1/2 O2(g) → H2O(l) ΔH = -285.8 kJ/mol The ΔHrxn for: 2 HCl(g) + F2(g) → 2 HF(l) + Cl2(g) is: From the following enthalpies of reaction: 2 H2(g) + O2(g) → 2 H2O(l) ΔH = -571.6 kJ/mol C3H4(g) + 4 O2(g) → 3 CO2(g) + 2 H2O(l) ΔH = -1937 kJ/mol C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) ΔH = -2220 kJ/mol Determine the heat of the hydrogenation reaction: C3H4(g) + 2 H2(g) → C3H8(g)
Using the standard enthalpies of formation Hf0 given, determine the enthalpy of this reaction. AX2 (g) + 2Y2 (g) → AX2Y4 (g) Hf0 values AX2 (g) = - 267.4 kJ/mol Y2 (g) = 126.2 kJ/mol AX2Y2 = 324.5 kJ/mol For full credit: Round your answer to the tenths place so that there are no decimals. (EX: 12.3 = 12) Include the correct unit.
Q2 (a) Given that the enthalpy values for the following reactions are: AH = -1049.0 kJ 2 Al (5) + 6HCI (ад) — 2 ALCI3 (аg) + 3 Н2 (9) AH = -74.8 kJ HCl (g) → HCl (aq) + Cl2 (g) → 2HCI AH = -185.0 kJ H2 (9) + AlCl3 (s) → AlCl3 (aq) (g) AH = -323.0 kJ ΔΗ Manipulate the reactions above to determine AH for: 2 Al(s) + 3 Cl2 (9) → 2 AlCl3 (s) In one experiment, a 25 g sample of an alloy was heated to a certain temperature. (b) The heated alloy was then dropped into a beaker containing 90 g of water at 25.32 °C. The temperature of the water rose to a final value of 27.18 °C. Predict the final temperature that the alloy is being heated at the beginning of the experiment. Given that the heat capacity of water and alloy are 4.184 Jgl°C-' and 0.3847 Jg l°C' respectively.
< Question 21 of 29 O Attempt 2 When 0.376 g of sodium metal is added to an excess of hydrochloric acid, 3910 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HCI(aq) 2 NaCl(aq) + H2(g) Enthalpy of reaction: 478.35 kJ Incorrect
18. From the following data, AH = -393.5 kJ/mol C(graphite) + O₂(g) → CO₂(g) 1 H₂ (g) + O₂(g) → H₂O(l) AH = -285.8 kJ/mol 2C₂H6 (g) +70₂(g) → 6H₂O(l) + 4CO₂(g) AH = -3119.06 kJ/mol calculate the enthalpy change for the reaction: 2C (graphite) (1) + 3H₂(g) → 2C₂H6 (g)
Consider the two reactions. 2NH3(g)+3N2O(g)⟶4N2(g)+3H2O(l) Δ?∘=−1010 kJ 4NH3(g)+3O2(g)⟶2N2(g)+6H2O(l) Δ?∘=1531 kJ Using these two reactions, calculate and enter the enthalpy change for the reaction below. N2(g)+1/2 O2(g)⟶N2O(g) Δ?∘=_____________kJ
Use Hess’s law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) —> W(s) +3H2O(g) from the following data: 2W(s) + 3O2(g) —> 2 WO3(s) H=-1685.4 2H2(g) + O2(g) —> 2H2O(g) H=-477.84
Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the reaction 2 SO2(g) + O2(g) → 2 SO3(g) The standard enthalpies of formation for SO2(g) and SO3(g) are AH; [SO2(g)] = -296.8 kJ/mol AH; [SO3(g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 2.25 L of SO2(g) is converted to 2.25 L gas behavior. of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal AH= kJ
Methane (CH4) burns in oxygen via the following reaction:CHa(g) + 202(g) > CO2(g) + 2H20(g) ; AH= -890 kJWhat is the enthalpy change for the combustion of 148.2 grams of methane ?
The enthalpy changes, AH, for three reactions are given. H, (g) + H, O(1) AH= -286 kJ/mol Ca(s) + 2 H*(aq) Ca2+(aq) + H, (g) Ca+(aq) + H, O(1) AH = -544 kJ/mol CaO(s) + 2 H*(aq) AH = -193 kJ/mol Using Hess's law, calculate the heat of formation for CaO(s) using the reaction shown. Ca(s) + O,(g) CaO(s) AH kJ/mol