Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- -6 Consider the following reaction where Kc = 5.10 × 10¯ at 548 K. NH4Cl(s) NH3(g) + HCl(g) A reaction mixture was found to contain 0.0527 moles of NH4 Cl(s), 0.00304 moles of NH3(g), and 0.00226 moles of HCl(g), in a 1.00 liter container. Is the reaction at equilibrium? not, what direction must it run in order to reach equilibrium? The reaction quotient, Q, equals The reaction O must run in the forward direction to reach equilibrium. O must run in the reverse direction to reach equilibrium. O is at equilibrium.arrow_forwardWhich of the following changes will result in an increase in the amount of phosphorous pentachloride formed?arrow_forwardA gas mixture consists of 3.74 atm of C₂H5Br, 4.22 atm of HBr, 0.11 atm of C₂H6, and 0.882 atm of Br₂. Calculate the reaction quotient for this system prior to the establishment of the equilibrium below. C₂H5Br(g) + HBr(g) = C₂H6(g) + Br₂(g) Report your answer to three significant figures in scientific notation. Submit Answer Tries 0/5arrow_forward
- At a certain temperature, Kc = 0.500 for the reaction SO3(g) + NO(g) — NO₂(g) + SO₂(g) If 0.100 mol SO3 and 0.200 mol NO are placed in a 2.00 L container and allowed to come to equilibrium, what will the NO2 and SO2 concentrations be? [NO₂] = [SO₂] = i M 3arrow_forwardConsider the following reaction where Kc CO(g) + Cl₂(g) CoCl₂(g) = 77.5 at 600 K: A reaction mixture was found to contain 4.16×10-² moles of CO(g), 4.43×10-² moles of Cl₂(g) and 0.106 moles of COCl₂(g), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: TF 1. In order to reach equilibrium COCI₂(g) must be consumed. 2. In order to reach equilibrium Kċ must decrease. 3. In order to reach equilibrium CO must be consumed. 4. Qc is greater than Kc. 5. The reaction is at equilibrium. No further reaction will occur.arrow_forwardConsider the following reaction CO₂ (g) +CCL, (g) -2000L₂ (g) 2COCL Calculate A-G for this reaction at 125 °C under the following conditions Pco, 0.105 bar 0.175 bar Poc, Pcoci,-0.735 bar A.G= 55.28 ΑΣΦ H C Previous Answers Request Answer X Incorrect; Try Again: One attempt remaining ? kJ molarrow_forward
- In the gaseous form, SO3 is a significant air pollutant, being the primary agent in acid rain. SO3 can further react with nitrogen monoxide to create NO2 which is also an air pollutant, as seen in the reaction below: SO3 (g) + NO (g) – NO2 (g) + SO2 (g) At 298K, the concentrations of the four gasses were found to be: [NO] = 0.18 mol/L [SO3] = 0.52 mol/L [SO2] = 1.34 mol/L [NO2]= 2.56 mol/L %3Darrow_forwardIn a suitable reaction vessel, pieces of graphite are mixed with carbon dioxide gas at 1.00 atm and 1000 K. Which two of the following changes will shift the reaction towards the products? kJ.mol-1 C(s) + CO₂ (g) 2 CO(g) → (A) increase the volume (B) decrease the temperature (C) decrease partial pressure of CO(g) (D) decrease partial pressure of CO₂(g) ΔΗ = 172arrow_forwardN2(g) + 3H2(g) + 2NH3(g) At 500°C, the value of Kc for this reaction is 0.40. The following concen- trations of gases are present in a container at 500°C: [N2(g)] = 0.10 mol/L, [H2(g)] = 0.30 mol/L, and [NH3(g)] = 0.20 mol/L. Is this mixture of gases at equilibrium? If not, in which direction will the reaction go to reach equilibrium? Is this mixture of gases at equilibrium: If "no", in which direction will the reaction go: (yes/no) (left/right/no-shift)arrow_forward
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