**Using the Standard Enthalpies of Formation:****Problem Statement:**Using the standard enthalpies of formation, what is the standard enthalpy of reaction?**Chemical Reaction:**CO(g) + H₂O(g) ⟶ CO₂(g) + H₂(g)**Equation to Complete:**ΔH°ᵣₓₙ = [input box] kJ**Explanation:**This problem involves calculating the standard enthalpy change (ΔH°ᵣₓₙ) for the given reaction using the standard enthalpies of formation of the compounds involved.The standard enthalpy of reaction can be calculated using the formula:\[ \Delta H°ᵣₓₙ = \sum \Delta H°_f (\text{products}) - \sum \Delta H°_f (\text{reactants}) \]Each term in the formula represents the standard enthalpy of formation (ΔH°_f) of the substances, which are typically determined experimentally and provided in tables.To complete this calculation, the standard enthalpies of formation for CO(g), H₂O(g), CO₂(g), and H₂(g) must be obtained from a reference source. The values should then be substituted into the formula to calculate the ΔH°ᵣₓₙ, expressed in kilojoules (kJ).

Since, The standard enthalpy of the formation is defined as change of enthalpy of 1 mol of the…

Answered: Using the standard enthalpies of…

Using the standard enthalpies of formation, what is the standard enthalpy of reaction? CO(g) + H₂O(g) → CO₂(g) + H₂(g) AHixn = 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

A chemist carefully measures the amount of heat needed to raise the temperature of a 533.0 mg sample of CH,N from 53.8 °C to 68.3 °C. The experiment shows that 16.5 J of heat are needed. What can the chemist report for the molar heat capacity of CH,N? Round your answer to 3 significant digits. -1 - 1 J•mol • K x10
3. Hydrazine, N2H4, is a colorless liquid used as a rocket fuel. What is the enthalpy change for the process in which hydrazine is formed from its elements? N2(g) + 2H2(g) → N2H4(l) Use the following reactions, enthalpy changes, and Hess’s Law N2H4(l) + O2(g) → N2(g) + 2H2O(l); ΔrH° = −622.2 kJ H2(g) + ½O2(g) → H2O(l); ΔrH° = −285.8 kJ
Given that 2Al(s) + 3 2 O2(g) → Al2O3(s) Δ H o rxn = −1601 kJ/mol and 2Fe(s) + 3 2 O2(g) → Fe2O3(s) Δ H o rxn = −821 kJ/mol calculate the standard enthalpy change for the following reaction: 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s) Enter your answer in scientific notation. × 10 kJ
Consider the thermochemical equation for the combustion of acetone (C3H₂O), the main ingredient in nail polish remover: C3H6O (1) + 4 O₂ (g) → 3 CO₂ (g) + 3 H₂O (g) ΔΗ° rxn = 1790 kJ If a bottle of nail polish remover contains 222 mL of acetone, what is the magnitude (the value) of heat released by the complete combustion of the acetone in the bottle? The density of acetone is 0.788 g/mL. The molar mass of acetone is 58.08 g/mol. The units are kJ. Do not include units in your answer.
Consider the hypothetical thermochemical equation 3 A + B → 2 C for which AH = 63.1 kJ/mol. Which one of the following reactions would have an enthalpy change of -2×AH? Here, AH refers to the enthalpy change of the original reaction. А) С — 3/2 А + 1/2 В B) 6 A + 2 B –→ 4 C С) 3/2 А + 1/2 В — С D) 4 C → 6 A + 2 B
Given the following thermochemical equations, C2 (g) +5/2O2 (g) → 2CO2 (g) +H2O (l) ΔH = −1299.5kJ C (s) + O2 (g) → CO2 (g) ΔH = −393.5kJ H2 (g) +1/2O2 (g) → H2O (l) ΔH = −285.8kJ Calculate ΔH for the decomposition of one mole of acetylene, C2H2 (g), to its elements in their stable state at 25°C and 1 atm.
Consider these reactions, where M represents a generic metal. 2 M(s) + 6HCl(aq) →→→ 2 MC1₂(aq) + 3H₂(g) HCI(g) HCl(aq) H₂(g) + Cl₂(g) → 2 HCI(g) MCI, (s) → MCI, (aq) Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl₂(g) → 2 MC1₂ (s) 1. 2. 3. 4. ΔΗ = AH₁ = -694.0 kJ AH₂ = -74.8 kJ AH3= -1845.0 kJ AH4 = -375.0 kJ kJ
When pure sulfuric acid is dissolved in water, heat is evolved. 10.65 g of pure sulfuric acid at 20.00 °C was added to a calorimeter containing 300 g of water at 20.00 °C. The temperature of the solution increased to 26.35 °C. If the specific heat of the mixture is 4.184 Jg1°C1, the density of water is 1 g/mL, and the heat capacity of the calorimeter is ignored, what is the heat evolved per mole of sulfuric acid? a. -83.2 kJ O b. -73.6 kJ O C. -76.0 kJ d. -80.8 kJ e. -78.4 kJ
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?
The sugar arabinose, C5 H10 O5, is burned completely in oxygen in a calorimeter. C5 H10 O5 (8) + 502(g) → 5CO2(g) + 5H2 O(1) Burning a 0.541 g sample caused the temperature to rise from 20.00°C to 20.54°C. The heat capacity of the calorimeter and its contents is 15.2 kJ/°C. Calculate AH for the combustion reaction per mole of arabinose. ΔΗ+ kJ/mol
A piece of chromium metal with a mass of 24.50 g is heated in boiling water to 98.3 °C and then dropped into a coffee-cup calorimeter containing 82.3 g of water at 23.4 °C. When thermal equilibrium is reached, the final temperature is 25.7 °C. Calculate the specific heat capacity of chromium. (The specific heat capacity of liquid water is 4.184 J/g ⋅ K.)
A chemist carefully measures the amount of heat needed to raise the temperature of a 1.65kg sample of C9H10O2 from 25.9°C to 37.9°C. The experiment shows that 3.09 X 104J of heat are needed. What can the chemist report for the molar heat capacity of C9H10O2? Round your answer to 3 significant digits. = J * mol-1 * K-1