Interpretation: The pressure at which
Concept introduction: The equilibrium constant
The equilibrium constant depends upon temperature.
Law of mass action is applicable on the equilibrium reactions.
The Le Chatelier’s principle states that the addition of the reactants shifts the equilibrium to the right while the addition of product shifts the equilibrium to the left at constant temperature.
The dissociation of the species is denotes by the symbol
To determine: The pressure at which
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Chemistry: An Atoms First Approach
- The atmosphere consists of about 80% N2 and 20% O2, yet there are many oxides of nitrogen that are stable and can be isolated in the laboratory. (a) Is the atmosphere at chemical equilibrium with respect to forming NO? (b) If not, why doesnt NO form? If so, how is it that NO can be made and kept in the laboratory for long periods?arrow_forwardA 2.500-mol sample of phosphorus pentachloride, PCl5, decomposes at 160C and 1.00 atm to give 0.338 mol of phosphorus trichloride, PCl3, at equilibrium. PCl5(g)PCl3(g)+Cl2(g) What is the composition of the final reaction mixture?arrow_forward12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?arrow_forward
- At 500C, k for the for the formation of ammonia from nitrogen and hydrogen gases is 1.5105. N2(g)+3H2(g)2NH3(g)Calculate the equilibrium partial pressure of hydrogen if the equilibrium partial pressures of ammonia and nitrogen are 0.015 atm and 1.2 atm, respectively.arrow_forward. Gaseous phosphorus pentachloride decomposes according to the reaction PCl5(g)PCl3(g)+Cl2(g)The equilibrium system was analyzed at a particular temperature, and the concentrations of the substances present were determined to be [PCl5]=1.1102M,[PCl3]=0.325M. and [Cl2]=3.9103M. Calculate the value of K for the reaction.arrow_forward. At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide. N2(g)+O2(g)2NO(g)Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations arc found to be [N2]=0.041M. [O2]=0.0078M, and [NO]=4.710M. Calculate the value of K for the reaction.arrow_forward
- . Suppose that for the reaction PCl5(g)PCl3(g)+Cl2(g)it is determined, at a particular temperature. that the equilibrium concentrations are [PCl5(g)]=0.0711M,[PCl3(g)]=0.0302M, and [Cl2(g)]=0.0491M. Calculate the value of K for he reaction at this temperature.arrow_forwardDescribe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.arrow_forwardAt a certain temperature, the reaction Xe(g)+2F2(g)XeF4(g)gives a 50.0% yield of XeF4, starting with Xe(Pxe=0.20atm) and F2(PF2=0.40atm). Calculate K at this temperature. What must the initial pressure of F2 be to convert 75.0% of the xenon to XeF4?arrow_forward
- At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?arrow_forwardWhy are there no changes specified for Ni in Exercise 13.61, part (f)? What property of Ni does change?arrow_forwardOne way of preparing hydrogen is by the decomposition of water. 2H2O(g)2H2(g)+O2(g);H=484kJ Would you expect the decomposition to be favorable at high or low temperature? Explain.arrow_forward
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