Homework Answers
Use bond energy values given
in your book it it says incorrect answer..because method is
accurate
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Part C Use bond energies to calculate ΔHrxn for the following reaction: N2 (g) + 3H2...
Use bond energies to calculate ?Hrxn for the reaction. 2H2(g)+O2(g)?2H2O(g) Note: The answer is NOT 442...
Use bond energies to calculate ?Hrxn for the
reaction.
2H2(g)+O2(g)?2H2O(g)
Note: The answer is NOT 442 kJ or 442kJ/mol
It gave me this hint when I got the answer wrong: The bond
energies of H?H, O=O, and H?O are provided in the introduction. To
determine the enthalpy of this reaction, sum all of the bond
energies for the reactants (accounting for stoichiometric ratios as
is), and subtract the bond energies for the product. Note how many
bonds are in each...
Calculate the heat of reaction AH for the following reaction: 2 NH3(9)-N2(g) + 3H2(g) You can...
Calculate the heat of reaction AH for the following reaction: 2 NH3(9)-N2(g) + 3H2(g) You can find a table of bond energies by using the Data button on the ALEKS toolbar. Round your answer to the nearest kJ/mol. kJ X 5 ? mol
The value of the equilibrium constant Kc for the reaction N2(g)+3H2(g)⇌2NH3(g) changes in the following manner...
The value of the equilibrium constant Kc for the reaction N2(g)+3H2(g)⇌2NH3(g) changes in the following manner as a function of temperature Temperature (∘C) Kc 300 9.6 400 0.50 500 0.058 Part A Use the standard enthalpies of formation given in Appendix C to determine the ΔH for this reaction at standard conditions. Express your answer in kilojoules to two decimal places. Part B If 0.027 mole of gaseous NH3 is added to a 1.00 L container and heated to 500 ∘C,...
Use average bond energies to calculate ΔHrxn for the following hydrogenation reaction: H2C=CH2(g)+H2(g)→H3C−CH3(g)
Use average bond energies to calculate ΔHrxn for the following hydrogenation reaction: H2C=CH2(g)+H2(g)→H3C−CH3(g)
23 A) For the reaction 2CH4(g)⇌C2H2(g)+3H2(g) Kc = 0.130 at 1651 ∘C . What is Kp...
23 A) For the reaction 2CH4(g)⇌C2H2(g)+3H2(g) Kc = 0.130 at 1651
∘C . What is Kp for the reaction at this temperature?
23 B) For the reaction N2(g)+3H2(g)⇌2NH3(g) Kp= 3.40×10−3 at 292
∘C. What is Kc for the reaction at this temperature?
Part A For the reaction 2CH (g) = C2H2(g) + 3H2(g) Kc = 0.130 at 1651 °C. What is K, for the reaction at this temperature? Express your answer numerically. View Available Hint(s) V AC ? K Kp...
For the reaction 2CH4(g)⇌C2H2(g)+3H2(g)2CH4(g)⇌C2H2(g)+3H2(g) KcKcK_c = 0.165 at 1642 ∘C∘C . What is KpKpK_p for the...
For the reaction 2CH4(g)⇌C2H2(g)+3H2(g)2CH4(g)⇌C2H2(g)+3H2(g) KcKcK_c = 0.165 at 1642 ∘C∘C . What is KpKpK_p for the reaction at this temperature? Express your answer numerically. For the reaction N2(g)+3H2(g)⇌2NH3(g)N2(g)+3H2(g)⇌2NH3(g) KpKpK_p = 5.65×10−3 at 350. ∘C∘C . What is KcKc for the reaction at this temperature? Enter your answer numerically.
Given the following data for heats of reaction N2(g) + 3H2(g) ----> 2NH3(g) H = -91.8 kJ...
Given the following data for heats of reaction
N2(g) + 3H2(g) ---->
2NH3(g) H
= -91.8 kJ
C(graphite) + 2H2(g) ------->
CH4(g)H
= -74.9kJ
H2(g) + 2C(graphite) + N2(g)
--------> 2HCN(g) H
= 270.3 kJ
Calculate
H for the reaction used to make HCN
CH4(g) + NH3(g) --------> HCN(g) +
3H2(g)
Ethanol is a possible fuel.Use average bond energies to calculate ΔHrxn for the combustion of ethanol. CH3CH2OH (g) +...
Ethanol is a possible fuel.Use average bond energies to calculate ΔHrxn for the combustion of ethanol. CH3CH2OH (g) + 3O2(g) ------> 2CO2 (g) +3H2O(g) ΔHrxn= ______ kJ/mol
What is the ΔSuniv for the following reaction at 25°C? N2(g) + 3H2(g) ⇌ 2NH3(g) ΔSsys...
What is the ΔSuniv for the following reaction at 25°C? N2(g) + 3H2(g) ⇌ 2NH3(g) ΔSsys = -197 J/K; ΔHsys = -91.8 kJ PLEASE SHOW WORK
For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) Kc is 0.595 at 461°C. Calculate KP for...
For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) Kc is 0.595 at 461°C. Calculate KP for the reaction at this temperature.
Use bond energies to calculate ?Hrxn for the
reaction.
2H2(g)+O2(g)?2H2O(g)
Note: The answer is NOT 442 kJ or 442kJ/mol
It gave me this hint when I got the answer wrong: The bond
energies of H?H, O=O, and H?O are provided in the introduction. To
determine the enthalpy of this reaction, sum all of the bond
energies for the reactants (accounting for stoichiometric ratios as
is), and subtract the bond energies for the product. Note how many
bonds are in each...
Calculate the heat of reaction AH for the following reaction: 2 NH3(9)-N2(g) + 3H2(g) You can find a table of bond energies by using the Data button on the ALEKS toolbar. Round your answer to the nearest kJ/mol. kJ X 5 ? mol
23 A) For the reaction 2CH4(g)⇌C2H2(g)+3H2(g) Kc = 0.130 at 1651
∘C . What is Kp for the reaction at this temperature?
23 B) For the reaction N2(g)+3H2(g)⇌2NH3(g) Kp= 3.40×10−3 at 292
∘C. What is Kc for the reaction at this temperature?
Part A For the reaction 2CH (g) = C2H2(g) + 3H2(g) Kc = 0.130 at 1651 °C. What is K, for the reaction at this temperature? Express your answer numerically. View Available Hint(s) V AC ? K Kp...
Given the following data for heats of reaction
N2(g) + 3H2(g) ---->
2NH3(g) H
= -91.8 kJ
C(graphite) + 2H2(g) ------->
CH4(g)H
= -74.9kJ
H2(g) + 2C(graphite) + N2(g)
--------> 2HCN(g) H
= 270.3 kJ
Calculate
H for the reaction used to make HCN
CH4(g) + NH3(g) --------> HCN(g) +
3H2(g)
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