Tutored Practice Problem 16.2.3 COUNTS TOWERS GUIDE Manipulate equilibrium constant expressions. The equilibrium constant for the...
Tutored Practice Problem 15.2.3 COUNTS TOWARDS GRADE Manipulate equilibrium constant expressions. The equilibrium constant for the following reaction is 2.18x10-3 at-24°C. 2 NOBr(g)2 NO(g) + Br2(g) K-2.18x103 at -24 °C Calculate the equilibrium constant for the following reactions at -24 °C. (a) 2 NO(g) +Br2g NOBr(g) K- (b) NOBr(g)_NO(1/2 Br2(g) K- Check & Submit Answer Show Approach
Tutored Practice Problem 19.3.4 COUNTS TOWARDS GRADE Calculate the equilibrium constant from the standard free energy change. Close Pr Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. N2(g) + O2(g) +2NO(g) K- Check & Submit Answer Show Approach
Close Problem Tutored Practice Problem 15.3.2 COUNTS TOWARDS GRADE Use an /CE table to calculate K A mixture of CO and Cl, is allowed to react at 585 K CO(g) + Cl2(g) cOC2(g) The initial concentration of the reactants are [cO] = 0.3050 M and [Cl2] = 0.3390 M. After the system reaches equilibrium, it is found that the Ch concentration has decreased to 0.0659 M. Based on these data, determine the value of the equilibrium constant, K, for this...
Tutored Practice Problem 16.4.1 COUNTS TOWARDS GRADE Predict and calculate the effect of concentration changes on an equilibrium system. Close Problem Some COCl2 is allowed to dissociate into CO and Cl2 at 873 K. At equilibrium, [COCI2] =0.237 M, and [CO] - [C12] = 0.128 M. Additional CO is added so that (CO)new = 0.193 M and the system is allowed to once again reach equilibrium. COC12(8) CO(g) + Cl2(g) K-6.98*10-2 at 873K (a) In which direction will the reaction...
Tutored Practice Problem 18.1.3 cOUNTS TOWARDS GRADE Use equilibrium ion concentration to calculate Ksp Close Problem The Pb2+ concentration in a saturated solution of lead chloride is measured and found to be 1.65x102 M. Use this information to calculate a K,p value for lead chloride. Ksp Check & Submit Answer Show Approach
Tutored Practice Problem 10.6.2 COUNTS TOWARDS GRADE Calculate enthalpy change using standard heats of formation. Using the standard heats of formation that follow, calculate the standard enthalpy change for the following reaction. H2S(g) 2H20(I) »3H2(g) +SO2(g) AH rxn kJ Species AHf(kJ/mol H2S(g) -20.6 H2O(D -285.8 SO2(g) -296.8 Check & Submit Answer Show Approach
Tutored Practice Problem 10.5.1 COUNTS TOWARDS GRADE Use Hess's law to calculate enthalpy change. Given the following two reactions: (1)Ca(s) + Cl2(9—+CaCl(s) AH(1) = -795.8 kJ (2)Hg(1) + Cl2(9) HgCl2(8) AH(2) = -224.3 kJ calculate the enthalpy change for the following reaction: (3) Ca(s) + HgC12(3)— CaCl2(S) + Hg(1) AH(3)=[ Check & Submit Answer Show Approach
Tutored Practice Problem 15.4.6 CESTO Determine half-life, order and k from concentration-time data The following data were collected for the gas phase decomposition of sulfuryl chloride at 600 K. SO,C12()— SO2(g) + Cl2() [SO,C1), M 2.50x103 time, min 1.25103 174.00 6.25*10+ 348.00 3.13*10+ 522.00 (a) What is the half-life for the reaction when [SO,Ch] -2.5010' M? (b) What is the half-life for the reaction when [SO_C12] -1.25 10 M? (c) Is the reaction first order? If so, what is the...
Predict and calculate the effect of concentration changes on an equilibrium system. Close Problem Some SO2Cl2 is allowed to dissociate into SO2 and Cl2 at 373 K. At equilibrium, [SO2C2] 0.206 M, and [SO2] [C12-0.127 M. Additional SO2C12 is added so that [SO2CI!new-0.35i M and the system is allowed to once again reach equilibrium. so2C2(g) 2so2(g)+ C2(g) K-7.84x102 at 373 K (a) In which direction will the reaction proceed to reach equilibri to the right to the left b) What...
Tutored Practice Problem 19.3.5 COUNTS TOWARDS GRADE Calculate temperature at which AGº changes sign. Close Calculate the temperature (in kelvins) at which the sign of AGº changes from positive to negative for the reaction below. This corresponds to the temperature at which K<1 changes to K > 1. Assume that AH and AS are constant and do not change with temperature, Fe304(8) + 4H2(e) 3Fe(8) + 4H2O(g) AH° - 151 kJ/mol and AS - 169 J/K: mol Check & Submit...