For the reaction2NH, (g) +20,(g)N,0(g) + 3H,0(g)the initial mixture contains 8.50 mol NH3 and 7.25 mol O2. At equilibrium, 2.25 mol of N20 gas are found.1st attemptl See Periodic Table O See HintHow many moles of NH3, O2, and H20 are present at equilibrium? Be sure to give your answers to two decimal places.mol NH3mol O2mol H2O

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2NH, (g) + 20,(g) - N,0(g) + 3H,0(g) the initial mixture contains 8.50 mol NH3 and 7.25 mol O2. At equilibrium, 2.25 mol of N20 gas are found. 1st attempt i See Periodic Table O See Hint How many moles of NH3, O2, and H2O are present at equilibrium? Be sure to give your answers to two decimal places. mol NH3 mol O2 mol H2O

2NH, (g) + 20,(g) - N,0(g) + 3H,0(g) the initial mixture contains 8.50 mol NH3 and 7.25 mol O2. At equilibrium, 2.25 mol of N20 gas are found. 1st attempt i See Periodic Table O See Hint How many moles of NH3, O2, and H2O are present at equilibrium? Be sure to give your answers to two decimal places. mol NH3 mol O2 mol H2O

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 3ALQ: For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each...

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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?
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