Calculate the standard enthalpy change, ΔH°rxn, in kJ for the following chemical equation, using only the...

Question

Question

Calculate the standard enthalpy change, ΔH°rxn, in kJ for the following chemical equation, using only the...

Calculate the standard enthalpy change, ΔH°rxn, in kJ for the following chemical equation, using only the thermochemical equations below:

2COBr₂(g) + 4NO(g) → 4NOBr(g) + 2CO(g)

Report your answer to three significant figures in scientific notation.

Equations:		ΔH°_rxn (kJ)
CO(g) + Br₂(g) → COBr₂(g)		-3
1/2N₂(g) + 1/2O₂(g) → NO(g)		90.4
1/2N₂(g) + 1/2O₂(g) + 1/2Br₂(g) → NOBr(g)		82.1

science chemistry

Add a comment Improve this question Transcribed image text

Answer 1

Answer #1

Add a comment

Answer 2

Similar Homework Help Questions

Calculate the standard enthalpy change, ΔH°rxn, in kJ for the following chemical equation, using only the...

Calculate the standard enthalpy change, ΔH°rxn, in kJ for the following chemical equation, using only the thermochemical equations below: CaCO3(s) → CaO(s) + CO2(g) Report your answer to three significant figures in scientific notation. Equations: ΔH°rxn (kJ) Ca(s) + CO2(g) + 1/2O2(g) → CaCO3(s) -812.5 2Ca(s) + O2(g) → 2CaO(s) -1270.3
Calculate the standard enthalpy change, ΔΗ0rn, în k] for the following chemical equation, using o...

Calculate the standard enthalpy change, ΔΗ0rn, în k] for the following chemical equation, using only the thermochemical equations below. Please Go Over This Question In etail 12NH3(aq) 1502(9)12NOg)18H200) Report your answer to three significant figures in scientific notation. Equations: 1/2N2(g) 1/202(g) NO(g) 1/2N2(g) O2(9) NO2(9) 4NH3(g) + 7O2(g) → 4NO2(g) + 6H20(1) 90.4 33.8 -1326.2 Submit Answer Incorrect. . Tries 2/99 Previous Tries Submissions to practice problems are not permanently recorded Calculate the standard enthalpy change, ΔΗ0rn, în k] for...
1. For a given chemical process, the system releases 226 kJ of heat and the surroundings...

1. For a given chemical process, the system releases 226 kJ of heat and the surroundings perform 233 kJ of work on the system. What is the value of ΔU (in kJ) for the process? Report your answer to three significant figures. 2. Calculate the standard enthalpy change, ΔH°rxn, in kJ for the following chemical equation, using only the thermochemical equations below: 2CaO(s) + 2CO2(g) → 2CaCO3(s). Report your answer to three significant figures in scientific notation. Equations: ΔH°rxn (kJ)...

The standard enthalpy of formation of CO(g) is −111 kJ/mol [refer to this equation C(s) +...

The standard enthalpy of formation of CO(g) is −111 kJ/mol [refer to this equation C(s) + 1/2O2(g) ⟶ CO(g)] What is the ΔHorxn of this reaction? (What is the standard enthalpy change of this reaction?) 2C(s) + O2(g) ⟶ 2CO(g) -253 kJ/mol - 222 kJ/mol -97.1 kJ/mol 534 kJ/mol 124.9 kJ/mol -50.5 kJ/mol 5 points QUESTION 2 (assume A, B, C, and D and E are chemicals) Look at these equations A + B à C ΔH° = -9 kJ/mol rxn...
Consider the exothermic reaction CH4(g)+2O2(g)→CO2(g)+2H2O(g) Calculate the standard heat of reaction, or ΔH∘rxn, for this reaction...

Consider the exothermic reaction CH4(g)+2O2(g)→CO2(g)+2H2O(g) Calculate the standard heat of reaction, or ΔH∘rxn, for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure form is considered to be zero. Reactant or product ΔH∘f (kJ/mol) CH4(g) -201 CO2(g) -393.5 H2O(g) -241.8 Express your answer to four significant figures and include the appropriate units.
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of...

The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...

Using the standard heats of formation that follow, calculate the standard enthalpy change for the following...

Using the standard heats of formation that follow, calculate the standard enthalpy change for the following reaction. S(s,rhombic) + 2CO(g)— SO2(g) + 2C(s,graphite) AH°rxn- KJ Species AH®(kJ/mol CO(g) -110.5 SO2(g) -296.8 Check & Submit Answer Show Approach
PART A. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: C2H5OH(l)+3O2(g)→2CO2(g)+3...

PART A. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g) Express your answer using four significant figures. PART B. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: CH4(g)+2O2(g)→CO2(g)+2H2O(g) Express your answer using three significant figures. PART C. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: C(s)+O2(g)→CO2(g) Express your answer using four significant figures. PART D. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction:...
The enthalpy of combustion (ΔH°c) of 1,1,2,2,-tetramethylcyclopropane (C7H14) is -4635.62 kJ/mol. a-Using the appropriate information given...

The enthalpy of combustion (ΔH°c) of 1,1,2,2,-tetramethylcyclopropane (C7H14) is -4635.62 kJ/mol. a-Using the appropriate information given below, calculate the enthalpy of formation (ΔH°f), in kJ/mol, for 1,1,2,2,-tetramethylcyclopropane. Report your answer to two decimal places. ΔH°f (CO2 (g)) = -393.51 kJ/mol ΔH°f (H2O (l)) = -285.83 b- Determine the mass (in g) of 1,1,2,2,-tetramethylcyclopropane produced, if ΔH° was determined to be -35.93 kJ during an experiment in which 1,1,2,2,-tetramethylcyclopropane was formed. Report your answer to three significant figures.

Using the enthalpy changes given below, calculate the enthalpy change for the following equation: N2(g) +...

Using the enthalpy changes given below, calculate the enthalpy change for the following equation: N2(g) + 2O2(g) -----> 2 NO2 using the following equations: 2NO -----> N2 + O2 delta H + -180.0 kJ NO2 -----> NO + 1/2 O2 delta H= 112.0 kJ

Calculate the standard enthalpy change, ΔH°rxn, in kJ for the following chemical equation, using only the...

Homework Answers