The combustion of butane is shown by the following equation: 2C,H10(1) + 130½(g) → 8CO2(g) + 10H;0(g) Use the following data to find the heat of reaction for the above equation. C(s) + O2(g) –→ CO2(g) + 393 kJ H2(g) + ½O2(g) → H,O(g) + 242 kJ 4C(s) + 5H2(g) → C,H10(1) + 126 kJ

The combustion of butane is shown by the following equation: 2C,H10(1) + 130½(g) → 8CO2(g) + 10H;0(g) Use the following data to find the heat of reaction for the above equation. C(s) + O2(g) –→ CO2(g) + 393 kJ H2(g) + ½O2(g) → H,O(g) + 242 kJ 4C(s) + 5H2(g) → C,H10(1) + 126 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

When 2.232 g of AX (s) dissolves in 147.5 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 34.8 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX (s) → A*(aq) + X¯ (aq) Assumptions for this calculation: · The specific heat of the solution is the same as that of pure water (4.18 J/gK) • The density of water = 1.000 g/mL · The liquid's final volume is not changed by adding the solid · The calorimeter loses only a negligible quantity of heat. The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change. Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCI(aq) 2 MCI, (aq) + 3 H, (g) ΔΗ = -550.0 kJ 2. HCl(g) HCI(aq) AH2 = -74.8 kJ > 3. H, (g) + Cl, (g) → 2 HCl(g) AH3 = -1845.0 kJ 4. MCl, (s) → MCI, (aq) AH4 = -291.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) → 2 MCI, (s) ΔΗ kJ
When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
2. Slaked lime (Ca(OH)2(s)) is produced when lime (calcium oxide, Cao (s)) reacts with liquid water. 65.2 kJ of heat is released for each mol of Ca(OH)2 that is produced. (a) Write a thermochemical equation for the reaction. (b) What is the enthalpy change when 523.3 kg of lime reacts with excess water?
Determine the amount of heat released when 180.00 g AsBr5(g) reacts according to the following equation: As4O10(g) + 6 AsBr5(g) → 10 Br3AsO(g) Additional equations that may be useful: 1/4 As4(s) + 3/2 Br2(g) → AsBr3(g) ΔH = -336.4 kJ/mol As4(s) + 5 O2(g) → As4O10(g) ΔH = -2967.3 kJ/mol AsBr3(g) + Br2(g) → AsBr5(g) ΔH = -84.2 kJ/mol AsBr3(g) + 1/2 O2(g) → Br3AsO(g) ΔH = -295.7 kJ/mol
4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).
Use the following information to calculate the amount of heat involved in the complete reaction of 7.20 g of carbon to form PbCO3(s) in reaction 4. Be sure to give the proper sign (positive or negative) with your answer. Reaction 1 Pb(s) + O₂(g) PbO(s) Reaction 2 C(s,graphite) + O₂(g) →→→ CO₂(g) Reaction 3 PbCO3(s). PbO(s) + CO₂(g) Reaction 4 Pb(s) + C(s,graphite) + O₂(g) →→→ PbCO3(s) 1st attempt AH rxn4° = ? kJ AH rxnl AHO rxn2 AHO rxn3 AHXn4 = -219 kJ = - 394 kJ = 86 kJ = ? See Periodic Table See Hint
Consider the following reaction: 2Mg(s)+O2(g)⟶2MgO(s)ΔH∘=−1203kJ What mass of magnesium must be combusted in order to generate 174.0 kJ of heat?
The flame in a torch used to cut metal is produced by burning acetylene (C2H2)(26.04 g/mol) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 22.5 × 104 kJ of heat? 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) ΔH = –2502 kJ
*ONLY THE SECOND PART*
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?