Calculating an equilibrium constant from a partial equilibrium compositionAmmonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces onlynitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 25.0 L tank with 1.6mol of ammonia gas and 10. mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be0.32 mol.Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to2 significant digits.Kс=☐ x10☑

The combustion of ammonia can be represented by the following balanced chemical equation: 4 NH₃ (g)…

Answered: Calculating an equilibrium constant…

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...

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Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 102, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10 M. N2(g) + 3H2(g) 2NH3(g) 8. Consider the chemical reaction: N2+3H2ylelds 2NH3. If the concentratlon of the reactant H2 was increased from 1.0x 102 M to 2.5 x 101 M, calculate the reaction quotlent (Q) and determine whlch way the chemical system would shift by comparlng the value of Q to K. B IU E E T T 0 Word(s) 4. If the concentration of the reactant H2 was decreased from 1.0x 102 M to 2.7 x 104 M, calculate the reaction quotlent (Q) and determine which way the chemical system would shift by comparing the value of Q to K. U T 0 Word(s)
Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 25 L tank with 7.9 mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 4.1 mol of nitrogen dioxide gas. The engineer then adds another 4.0 mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol x10 X Ś
Write the equilibrium-constant expression for any reaction?
Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3C12(g) =S2C12(g) + CCI4(g) In an experiment, 1.00 mol of CS2 and 3.00 mol of Cl2 are placed in a 2.00L to react. When the system reaches equilibrium, the mixture contains 0.250 mol of CCI4. What is the amount of Cl2 at equilibrium? 0.25 mol 0.75 mol 2.25 mol 0.50 mol 2.75 mol
In a particular experiment, it was found that when O₂(g) and CO(g) were mixed and allowed to react according to the equation 2CO(g) + O₂(g) → 2CO₂(g) the O₂ concentration had decreased by 0.041 mol L-¹ when the reaction reached equilibrium. How had the concentrations of CO and CO₂ changed? [CO] decrease = [CO₂] increase = mol/L mol/L
Steam reforming of methane ( CH, ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 25.0 L tank with 1.3 mol of methane gas and 10. mol of water vapor, and when the mixture has come to equilibrium measures the amount of carbon monoxide gas to be 0.78 mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K_ -0 ?
A gaseous mixture contains 0.26 mol CO, 0.14 mol H2, and 0.021 mol H2O, plus an unknown amount of CH4, in each liter. This mixture is at equilibrium at a certain temperature. What is the concentration of CH4 in this mixture? The equilibrium constant Kc equals 3.97. mol/L
Write all equilibrium equations Write all equilibrium concentrations Write all equilibrium expressions
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 75.0L tank with 6.5 mol of sulfur dioxide gas and 29.mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 3.3 mol.Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits
chemical equilibrium A quantity of PCl5 was heated on a 12 L flask vessel at 250 degrees Celsius. At equilibrium the flask contains 0.28 mole PCl5 and 0.35 mole PCl3. If the equilibrium constant is 1.6 x 10 -4, find the concentration of Cl2.
For the chemical equation SO, (g) + NO, (g) = so,(g)+NO(g) the equilibrium constant at a certain temperature is 2.10. At this temperature, calculate the number of moles of NO, (g) that must be added to 3.12 mol SO, (g) in order to form 1.30 mol SO, (g) at equilibrium. moles of NO,(g): mol
Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.4 × 103 at a particular temperature. If the equilibrium concentrations of H20 and H2 are 0.11 M and 0.019 M, respectively, determine the concentration of Oz at equilibrium.. 2 H20(g) =2 H2(g) + O2(g)

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