Imagine that a chemist puts 0.828 mol each of HNO3 and SO2 in a 1.00-L container at a constant temperature of 341 °C. This reaction occurs: 2 HNO3(g) +  SO2(g) ⇄  H2SO4(g) + 2 NO2(g) When equilibrium is reached, 0.389 mol of H2SO4 is in the container. Find the value of Keq for the reaction.

Consider the following equilibrium: +2NOgCl2g    2NOClg =       ΔG0−41.kJ Now suppose a reaction vessel is filled with  8.37atm  of chlorine  Cl2  and  4.00atm  of nitrosyl chloride  NOCl  at  536.°C . Answer the following questions about this system: Under these conditions, will the pressure of  Cl2  tend to rise or fall?   rise     fall   Is it possible to reverse this tendency by adding  NO ?In other words, if you said the pressure of  Cl2  will tend to rise, can that be changed to a tendency to fall by adding  NO ? Similarly, if you said the pressure of  Cl2  will tend to fall, can that be changed to a tendency to rise by adding  NO ?   yes     no   If you said the tendency can be reversed in the second question, calculate the minimum pressure of  NO  needed to reverse it.Round your answer to  2  significant digits. atm

Mercury(IT) oxide decomposes to form mercury and oxygen, like this: 2HgO(s)--2Hg(l)+O2(g) At a certain temperature, a chemist finds that a 3.5 L reaction vessel containing a mixture of mercury (It) oxide, mercury, and oxygen at equilibrium has the following composition: compound amount HgO 15.3 g Hg 19.1 g O2 25.0 g Calculate the value of the equilibrium constant K, for this reaction, Round your answer to 2 significant digits.

Calculate the pressure of N2 needed to reverse the reaction (last row of the table. 0.38 is wrong). thank you!

Consider the following equilibrium: N₂O4 (g) → 2NO₂ (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 0.399 atm of dinitrogen tetroxide (N₂O4) at 588. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. O O rise fall yes no atm x10 X 5

While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 25 L tank with 1.9 mol of ethylene gas and 5.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 0.97 mol of ethylene gas and 4.77 mol of water vapor. The engineer then adds another 0.95 mol of ethylene, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. mol x10 X

Consider the following equilibrium: N₂O₂ (g) 2NO₂ (g) 2 AG=5.4 kJ Now suppose a reaction vessel is filled with 2.57 atm of dinitrogen tetroxide (N₂O4) at 138. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. rise fall O yes no 10 FAED alo Ar

Calculate the reaction quotient, QR for the following reactions and conditions:    2 NOCl(g)      :   KP = 2.5 x 103;  PNO = 0.0032 atm; PCl2 = 0.023 atm; PNOCl = 0.210 atm   2 NH3(g) N2(g) + 3H2(g)     :   KP = 17.0;  PNH3 = 0.13 atm; PN2 = 0.34 atm; PH2 = 1.1 atm

Consider the following equilibrium: 2NOC1 (g) 2NO(g) + Cl₂ (g) AG=41. KJ Now suppose a reaction vessel is filled with 3.76 atm of nitrosyl chloride (NOC1) and 6.26 atm of nitrogen monoxide (NO) at 1161. °C. Answer the following questions about this system: Under these conditions, will the pressure of NO tend to rise or fall? Is it possible to reverse this tendency by adding C1₂? In other words, if you said the pressure of NO will tend to rise, can that be changed to a tendency to fall by adding C1₂? Similarly, if you said the pressure of NO will tend to fall, can that be changed to a tendency to rise by adding Cl₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of C12 needed to reverse it. Round your answer to 2 significant digits. OO rise fall yes no atm x10 X Ś

Calculating an equilibrium constant from a partial equilibrium composition Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 2.0 L flask with 4.4 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 2.0 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = р x10 Ś ? olo 18 Ar B