The standard free energy of formation of ammonia is \( -16.5 \, \text{kJ/mol} \).\[ \text{N}_2 (g) + 3\text{H}_2 (g) \rightleftharpoons 2\text{NH}_3 (g) \]**1st attempt**What is the value of \( K \) for the reaction below at 485.0 K? \[ \_\_\_\_\_\_\_\_\_\_\_ \]This text is part of an educational exercise that requires calculating the equilibrium constant (\( K \)) for the synthesis of ammonia from nitrogen and hydrogen gases at a specified temperature. The reaction is given as:\[ \text{N}_2 (g) + 3\text{H}_2 (g) \rightleftharpoons 2\text{NH}_3 (g) \]The standard free energy change for the formation of ammonia is provided, and the task involves determining the equilibrium constant at a specific temperature.

The reaction given is, => N2 (g) + 3 H2 (g) ------> 2 NH3 (g)…

Answered: The standard free energy of formation…

The standard free energy of formation of ammonia is - 16.5 kJ/mol. N, (g) + 3H,(g) – 2NH, (g) v 1st attempt What is the value of K for the reaction below at 485.0K?

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

Related questions

Q: The fertilizer battery An electrochemical battery is used to provide 1 milli-watt (1mW) of power to…

A: Given reaction 1/2N2 + 3/2H2 --->> NH3 and power applied is 1 milliwatt And we know ∆Gf of…

Q: Consider the following reaction and the tabulated thermochemical data at 298 K. Substance 4 NH AH°…

A: Standard entropy is the entropy of one mole of a substance at a temperature of 298 K and a pressure…

Q: For each reaction with ΔH = + 187 kJ/mol and ΔS = + 365 J/molK ,at what temperature at which the…

A: Given: ΔH = +187 KJ/mol or +187000 J/mol ΔS = +365 J/molK We have to calculate temperature(T) at…

Q: In a reaction, 1.00 mole of H2 is produced at a constant pressure of 1.00 atm and at 298 K (1 L atm…

A: Therefore, ΔE in this reaction is +483.6 kJ.Explanation:The equation for calculating ΔE is:ΔE = ΔH -…

Q: Consider the reaction: NH, (0) + HCI (g) NH,CI (4) Given the following table of thermodynamic data…

Q: A helium-filled balloon at 305.0 K and 1 atm, contains 0.35 g He, and has a volume of 1.24 L. It is…

A: Heat energy can be determined using the given formula.

Q: Caculate the ΔG°rxn for the following reaction at 298 K ? How will the calculated ΔG°rxn change…

A: since ΔG°rxn = ΔH°rxn - T ΔS°rxn And ΔH°rxn = sum of (ΔH°f of products X reaction coefficient) -…

Q: Can

A: ∆S°(surrounding) = -∆H°/ T ∆S°(surrounding) = - ( + 30kJmol-1 ) / 300K ∆S°( surrounding ) = -30…

Q: The formation of CO from incomplete burning of graphite (with the limited amount of oxygen) is given…

Q: Which reaction is more energetically favored, one with ΔG0 = - 44 kJ/mol or one with ΔG0 = + 44…

A: The spontaneity of a reaction can be found out by the change in Gibbs free energy of the reaction.…

Q: Consider the reaction AB + C at 298 K. Given that the forward rate constant (kf) is 0.46 s-1and the…

A: The given reaction is, A ----> B+C Thus, the…

Q: 9. A chemical reaction under standard state has the enthalpy of reaction: A,H° = +117 kJ and the…

A: B) The reaction is entropy driven.

Q: Consider the following reaction at 298 K: N₂O4 (g) 2 NO₂ (g) with Kp = 0.142. What is the standard…

A: The standard free energy change (ΔG°) in kJ/mol can be calculated from the equilibrium constant…

Q: Consider the reaction of tin(IV) oxide with carbon. SnO2 (s) + C(s) → Sn(s) + CO2(g) A;H° (kJ/mol)…

Q: IV. Calculate AH, AS and AG at 25 C, and tell if the reaction will go spontaneously (use Table 1 and…

Q: What is the free energy change at 25oC for the reaction below, if the standard entropies of…

A: Gibbs free energy is an energy which is used to do useful work. It is an extensive property which…

Q: 2) The normal boiling point of benzene is 80.1 °C and the heat of evaporation (AH°vap) is 30.7…

Q: A helium-filled balloon at 300.0 K and 1 atm, contains 0.40 g He, and has a volume of 1.30 L. It is…

Q: A helium-filled balloon at 310.0 K and 1 atm, contains 0.30 g He, and has a volume of 1.27 L. It is…

A: Given data contains, Initial temperature is 310.0 K. Pressure is 1 atm. Mass of He is 0.30 g Initial…

Q: All of the following have the free energy of formation value zero except: a) Fe(s) b) N2(g)…

A: All Have Zero free energy of formation except

Q: s the lowest pH?

A: Lower pKa value results in stronger acid whereas higher pKa value results in weaker acid.

Q: Calculate the standard free energy change (kJ/mol) for the reaction shown at a temperature of 298.15…

Q: All of the following has a zero value for free energy of formation except: 12(s) 03(g) Br2(1) Li(s)…

A: Free energy of formation is that change of energies when one of substance is formed from its…

Q: 55 For a certain chemical reaction, AH° = -40.0k] and AS = -150.OJ/K. (a) Does the reaction lead to…

Q: A helium-filled balloon at 310.0 K and 1 atm, contains 0.35 g He, and has a volume of 1.22 L. It is…

A: Moles of Helium is calculated as follows,

Q: For each of the reactions listed in Table 3, predict the sign of AS. Use examples help Based on the…

A: "Since you have asked multiple questions, we will solve the first question for you (B. Question 1).…

Q: Consider the reactions (data for 25°C), i) Pb(s) + CO(g) → PbO(s) + C(s) kJ mol-1 AG° = -51 kJ mol…

A: ∆H is change in enthalpy of reaction.∆G is Gibbs free energy change.∆S is change in entropy for the…

Q: Beta O It is stable and does not undergo decay. QUESTION 15 Find the temperature (in K) below which…

A: [15.] ΔH = - 201.5 kJ/mol = - 201.5 × 103 J/mol ΔS = - 70.2 J/k.mol T = ?

Q: Using the information below, what is the standard free energy change at 25 °C for the reaction…

Q: Determine of T/F. The ΔGo of a reaction is -5 kJ/mol at 25oC so the reaction is at equilibrium.

A: Given value of standard Gibbs free energy value is negative

Q: If a reaction has a ΔH = 150 kJ/mole and a ΔS = -2550 J/mole K, at what temperature range would…

A: Gibbs free energy change is negative for spontaneous reaction

Q: Find AS for the formation of 1 mole of PCl<(g) from its elements. J/K

A: The entropy change for the reaction is shown by the sum of the entropies of the products minus the…

Q: If the Delta*H = 135kJ / m * ol and AS 92 J/K mol, at what temperature does this reaction become…

Q: Which reaction is spontaneous? O A-> B +C Delta G = 333kJ O D-> E +F Delta G = 0J O G-> H + I Delta…

A: The reaction which is spontaneous has to be given.

Q: A helium-filled balloon at 305.0 K and 1 atm, contains 0.35 g He, and has a volume of 1.29 L. It is…

Q: 29 O O O 0 0 For the following reaction, AH = 137 kJ, ASn = 120 J/K. C₂H6(g) → C₂H4(g) + H₂(g) This…

A: Given data : deltaH= 137 KJ = 137000 J( 1 KJ= 1000J) deltaS = 120 J/K The reaction : C2H6(g)…

Q: The standard free energy of formation of ammonia is -16.5 kJ/mol. N2 (g) + 3H, (g) = 2NH,(g) What is…

A: Formula ∆Gr° = -2.303RT log K -16.5 x 103 J = -2.303 x 8.314 x 365 log K log K = 2.36 = log ( 2.30…

Q: For the following reaction, AGºrxn = -12.17 kJ/mol at 1700 C. 2 A(g) + B(g) 2 C(g) a. What is the…

A: Given- 2A+B<->2C. ∆G°rxn=-12.17KJ/mol Moles of A=2mol Moles of B=1.40mol Moles of…

Q: Consider the reaction CO(g) + Cl₂(g) →→CoCl₂(g) Use the standard thermodynamic data in the tables…

A: Reaction CO(g) + Cl2(g) → COCl2(g) Partial pressure pCOCl2=17.87 mmHg=17.87760atm=0.0235…

Q: Anammox bacteria are known to obtain energy from the anaerobic autotrophic oxidation of one mole of…

A: The main aim of this question is to show the electron equivalent energy reaction for the anammox…

Q: A helium-filled balloon at 315.0 K and 1 atm, contains 0.15 g He, and has a volume of 1.35 L. It is…

A: Specific heat capacity is the amount of heat that is required to rise a temperature of 1 kg…

Q: d. The rxn = 79.7 J/( mol-K), at what temperature will this 9) Given AH = 57.2 kJ/mol and AS,…

A: A reaction with negative ΔG means the reaction occurs with a release in energy. This means that…

Q: E. If the statement depicts a spontaneous process write capital letter S, and if the statement does…

A: A spontaneous reaction occurs without any input of energy and proceeds on its own. The…

Q: Determine the ΔSsystem given the reaction. C6H12O6(s) + O2(g) ----> CO2(g) + H2O(l).

A: Given, C6H12O6(s) + O2(g) ----> CO2(g) + H2O(l). The ∆s(system) equals to:

Q: A reaction has H=225kj/mol and S= 630 j/molK. At what temp in K will it become spontaneous?

Q: the K for a reaction is determined to 3.81 at 20.26 ºC, then what is ΔG for the reaction (in J/mol,…

A: Given-> K = 3.81 T = 20.26 °C = 20.26 + 273 = 293.26 K

Question

The standard free energy of formation of ammonia is \( -16.5 \, \text{kJ/mol} \).

\[ \text{N}_2 (g) + 3\text{H}_2 (g) \rightleftharpoons 2\text{NH}_3 (g) \]

**1st attempt**

What is the value of \( K \) for the reaction below at 485.0 K? \[ \_\_\_\_\_\_\_\_\_\_\_ \]

This text is part of an educational exercise that requires calculating the equilibrium constant (\( K \)) for the synthesis of ammonia from nitrogen and hydrogen gases at a specified temperature. The reaction is given as:

\[ \text{N}_2 (g) + 3\text{H}_2 (g) \rightleftharpoons 2\text{NH}_3 (g) \]

The standard free energy change for the formation of ammonia is provided, and the task involves determining the equilibrium constant at a specific temperature.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

In liver cells the usual concentrations of some solutes are: [ATP] = 3.4 mM; [ADP] = 1.3 mM and [Pi] = 5 mM. Calculate the real variation of energy free by hydrolyzing ATP in the liver into ADP and Pi. a) at 25ºC b) at 37ºC (ΔGº’ ATP hydrolysis = -30.5 kJ / mol)
Explain correctly step by step
The following reaction is exothermic. MgO(s) → Mg²+(g) + O2-(g) + 02 (g) O True False
Calculate ΔG for the reaction below, where the T = 298K, ΔH = 28.05 kJ, and the ΔS = 109 J/K. NH4NO3(s) + H2O(l) NH4+ (aq) + NO3- (aq)
A 0.582-g sample of Mg reacts with excess 1.0 M HCl (60.0 mL) according to the procedure used in this experiment. The initial and final temperatures were 24°C and 68°C. What is the ∆H of the reaction per mole of magnesium? Assume that the specific heat capacity for the solution is 4.187 J/oC∙g and that the density of the 1.0 M HCl is 1.00 g/mL. (Hints: the magnesium contributes to the mass of the solution; take care with your sig figs.) (answer: - 4.7 × 102 kJ/mol)Show your solution to this problem in the space below. It is your solution which will be graded.
What is the free energy change at 25oC for the reaction below, if the standard entropies of reactants and products are So (C(gr)) = 5.74 J/mol*K, So(H2(g)) = 130.68 J/mol*K, and So (C4H10(g)) = 310.1000 J/mol*K and the heat of formation of C4H10(g) is -126.1400 kJ/mol.4C(gr) + 5H2(g) ↔ C4H10(g) ΔGo = -16.995 kJ ΔGo = 16.995 kJ ΔGo = 235.285 kJ ΔGo = -235.285 kJ
3.
2 For the synthesis of ammonia where AG = -33.3 kJ/mole, determine whether the reaction is spontaneous at 25 C with the following pressures: PN, = 1.0 atm, PH, = 3.0 atm, PNH, = 0.020 atm N2(8) + 3H2(g) = 2NH3(g)
Spontaneous or non-spontaneous
Calculate ΔGo in kJ for the following chemical reaction at 60oC, given the ΔHf values below, and given that the change in entropy for the reaction is EITHER (i.e. you have to choose which) positive or negative 284.5 J/mol K. NH4Cl (s) <--> NH3 (g) + HCl (g) -314 -45 -92 (kJ/mol)
Given the following information, calculate AGO for the reaction below at 27 °C. Ni(s) + 1/2O₂(g) → NIO(s) ΔΗ, = -401.7 kJ and AS° = -94.6 J/K KJ
The following reactions (in the left column) have been observed to be spontaneous. For each reaction decide which OA is stronger and which RA is stronger in the right column. An example is shown.