
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Predict the effect of increasing the container volume on theamounts of each reactant and product in the following reactions:

Transcribed Image Text:(a) F2(g) 2F(g)
(b) 2CH4(8) C,H2(g) + 3H2(g)
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- For the reaction: 2 NO2 (g) + O2 (g) --> 2 NO3 (g) at 923 °C , Kc is 42.5. If 0.0500 moles of NO2 (g), 0.122 moles of O2 (g) and 0.300 moles of NO3 (g) are mixed in a 1.00 liter container at 923 °C, in what direction will the reaction proceed? (Show your calculation to prove that your answer is not a guess.)arrow_forwardConsider the following reaction where Kc = 55.6 at 698 K. H2(g) + I2(g) ----> 2HI(g) A reaction mixture was found to contain 4.26×10-2 moles of H2(g), 4.04×10-2 moles of I2(g) and 0.270 moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Qc, equals _____ The reaction (fill in the blank) ____ A. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium.arrow_forwardAs you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°Carrow_forward
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