OPrevious Page 1 of 2 Next O Consider the following equilibrium: CO(g) + H2(g) = CO(g) + H,O(g), K. = 1.6 at 1260 K Suppose 0.046 mol CO, and 0.029 mol H2 are placed in a 4.00-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g)? (R=0.0821 L atm/(K - mol)) O 0.43 atm O 0.51 atm O 1.9 atm O 1.2 atm O 0.75 atm

OPrevious Page 1 of 2 Next O Consider the following equilibrium: CO(g) + H2(g) = CO(g) + H,O(g), K. = 1.6 at 1260 K Suppose 0.046 mol CO, and 0.029 mol H2 are placed in a 4.00-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g)? (R=0.0821 L atm/(K - mol)) O 0.43 atm O 0.51 atm O 1.9 atm O 1.2 atm O 0.75 atm

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 25QAP: Consider the decomposition of ammonium hydrogen sulfide: NH4HS(s)NH3(g)+H2S(g) In a sealed flask at...

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A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
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