Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Suppose a 250. mL flask is filled with 0.90 mol of CO, 0.50 mol Of NO and 0.80 mol of CO ₂. The following reaction becomes possible: NO₂(g) + CO (g) → NO(g) + CO₂(g) The equilibrium constant x for this reaction is 0.980 at the temperature of the flask. Calculate the equilibrium molarity of No. Round your answer to two decimal places. ? olo 18 Ararrow_forwardSuppose a 500. mL flask is filled with 1.4 mol of N2 and 0.70 mol of NO. This reaction becomes possible: N2(g) + O2(g) = 2NO (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use r to stand for the unknown change in the molarity of N2. You can leave out the M symbol for molarity.arrow_forwardSetting up a reaction table Suppose a 500. mL flask is filled with 0.10 mol of H₂ and 0.60 mol of HI. This reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H₂. You can leave out the M symbol for molarity. [H₂] [42] initial change equilibrium x [HI]arrow_forward
- For the equilibrium reaction 2SO 2(g) + O 2(g) <-> 2SO 3(g), ΔHº rxn = –198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase? Add SO2 gas. Add a catalyst. None of these. Decrease the temperature. Remove O2 gas.arrow_forwardSuppose a 250. mL flask is filled with 1.0 mol of NO₂, 0.20 mol of NO and 1.7 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) +CO, (g) The equilibrium constant K for this reaction is 5.54 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M Images Xarrow_forwardNitrogen 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 125 L tank with 45. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 12. mol of nitrogen dioxide gas. The engineer then adds another 11. 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 x10arrow_forward
- Pravinbhaiarrow_forwardSuppose a 500. mL flask is filled with 1.7 mol of CO, 0.50 mol of CO2 and 0.90 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 1.14 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X Śarrow_forwardThe following reaction is investigated: Initially there are 0.44 mol of N20 and 0.45 mol of N2H4 in a container. If the amount of N2 at equilibrium is 0.174 mol, how many moles of N20 are present at equilibrium? 2N20 (g) + N2H4 (g) 5 3N2 (g) + 2H2O (g) Report your answer as a decimal with two significant figures.arrow_forward
- Suppose a 500. mL flask is filled with 0.70 mol of NO2, 1.7 mol of CO and 0.30 mol of NO. The following reaction becomes possible: NO₂(g) + CO (g) → NO(g) + CO₂(g) The equilibrium constant K for this reaction is 8.94 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. ☐M X Śarrow_forwardSuppose a 250. mL flask is filled with 1.2 mol of NO and 0.90 mol of NO 2. The following reaction becomes possible: NO3(g) + NO(g) = 2NO2(g) The equilibrium constant K for this reaction is 0.661 at the temperature of the flask. Calculate the equilibrium molarity of NO 3. Round your answer to two decimal places. Ом ☑arrow_forwardNitrogen 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 75 L tank with 23. mol of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 17.9 mol of nitrogen dioxide gas. The engineer then adds another 7.7 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.arrow_forward
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