**Chemical Equilibrium Calculation** **Problem Statement:** Enter your answer in the provided box. For the reaction: \[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \] Given that \( K_c \) is 0.393 at 485°C, calculate \( K_p \) for the reaction at this temperature. \[ K_p = \square \] **Guidance:** For a given reaction at equilibrium, the relationship between the equilibrium constants \( K_c \) and \( K_p \) can be determined using the equation: \[ K_p = K_c(RT)^{\Delta n} \] Where: - \( R \) is the gas constant, typically 0.0821 L·atm/mol·K - \( T \) is the temperature in Kelvin - \( \Delta n \) is the change in moles of gas (\( \text{moles of gaseous products - moles of gaseous reactants} \)) **Steps to follow:** 1. Convert the temperature from Celsius to Kelvin. 2. Calculate \( \Delta n \) for the reaction. 3. Substitute the known values into the \( K_p \) equation to find the answer.

Chemical Equilibrium Calculation Problem Statement: Enter your answer in the provided box. For the reaction: \[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \] Given that \( K_c \) is 0.393 at 485°C, calculate \( K_p \) for the reaction at this temperature. \[ K_p = \square \] Guidance: For a given reaction at equilibrium, the relationship between the equilibrium constants \( K_c \) and \( K_p \) can be determined using the equation: \[ K_p = K_c(RT)^{\Delta n} \] Where: - \( R \) is the gas constant, typically 0.0821 L·atm/mol·K - \( T \) is the temperature in Kelvin - \( \Delta n \) is the change in moles of gas (\( \text{moles of gaseous products - moles of gaseous reactants} \)) Steps to follow: 1. Convert the temperature from Celsius to Kelvin. 2. Calculate \( \Delta n \) for the reaction. 3. Substitute the known values into the \( K_p \) equation to find the answer.

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

4. Pls answer asap . Pls provide accurate answer. Help me thank uuu. Handwritten thank u.
AutoSave CHEM 212 Final Exam_Fall 2020 Word Search 困 ff steve M SM File Home Insert Draw Design Layout References Mailings Review View Help E Share O Comments 3a) Calculate AGon for this reaction: CH3OH (g) → CO (g) + 2 H2 (g) The equilibrium partial pressures for each component are: CH;OH = 0.620 atm, CO = 0.105 atm, H2 = 0.125 atm b) Is the reaction spontaneous? Briefly explain. 3c) Cells use the hydrolysis of adenosine triphosphate (ATP) as a source of energy. The conversion of ATP to ADP has a standard free energy change of -30.5 kJ/mol. If all the free energy from the metabolism of glucose goes to the conversion of ADP to ATP, how many mole of ATP can be produced for each mole of glucose? Page 3 of 6 492 words D Focus 80%
B?
n 25 of 25 > O Macmillan Learning Bromine monochloride is synthesized using the reaction Br₂(g) + Cl₂(g) 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 209.0 L flask initially contains 1.100 kg of Br₂ and 1.053 kg of Cl₂. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCI: 0.529 percent yield: Incorrect What is the percent yield of BrCl? 0.064 Attempt 1 Incorrect g
4. Determine the value of p for the reaction shown below from the data given. How do interpret this value? Remember: log (k/ko) = op you Y k (M'sec) CH30 CH3 21.3 24.0 -0.27 -0.17 H. 0.00 37.4 Br 0.23 95.1 NO2 0.78 1430 SO2 ОН SO3 HO.
Mastering Chemistry help.
in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working!!!!!!!
Determine the value of Ke for the following reaction if the equilibrium concentrations are as follows: [P4010leq = 3.000 moles, [P4leq= 4.000 moles, [O2leg = 5.000 M %3D %3D %3D P4010(s) P4(6) +5 02(8) Select one: O a. 4.000 O b. 5.000 O C. 4167 O d. 12500 O e. 3125
Write the equilibrium constant expression, K., for the following reaction: If either the numerator or denominator is 1, please enter 1 CoS(s) Co2*(aq) + s2-(aq) K. = Submit Answer Try Another Version 1 item attempt remaining
Macmillan Leag The reaction C(s) + 2H₂(g) = CH₂(g) 8.04 L flask and heated to 1000. K. has Kp = 0.263 at 1000. K. Calculate the total pressure at equilibrium when 4.547 g of H₂ and 23.86 g of C(s) are placed in a JOI F Ptotal = O 81 1 % 5 T G a 16 10 6 24 1 & Y 17 H 7 ♫ U 18 J 8 9 fg K 9 f10 O ▶II O L f11 ►►I - P dd f12 { 59°F + [ = insert } 1 atm 1 4:10 PM 10/1/2022 prt sc backspace dele ㅏ enter
Hi, Consider this reaction at equilibrium 2BrNO(G) <----> 2NO( g) + Br2 (g) Predict the effect (shift right, shift left, or no effect) of these changes. a) adding BrNO to the reaction mixture. Thank you,
COVID-19 & Health e. Kc = [NH3]² · [CO2] For which reactions will the position of equilibrium shift due to changing the volume of the container. Select one: O a. Only reactions which have more gaseous products than reactants. O b. Only reactions where the number of moles of gas changes. c. All reactions involving a gas. d. All reactions where the number of moles change. O e. Only reactions which have less gaseous products than reactants. Select the correct cell notation for the following reaction, which is setup as a cell with a platinum electrode: