The numerical value of the equilibrium constant,
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- At high temperatures nitrogen (N2) and oxygen (O2) will react to form NO.N2(g) + O2(g) ⇆ 2 NO(g) (4.1)The value for the equilibrium constant for reaction 4.1 is KC = 2.7 x 10^-17 at some temperature T.A system initially has [N2] = 0.0800 M and [O2] = 0.0500 M. There is no NO initially present inthe system. Find the value for [NO] that will be present at equilibrium.arrow_forward10. 1) Please choose the corect expression and circle it. Le chatelier's Principle Summarized Below Change Concentration Pressure Volume Shifts Equilibrium Change Equilibrium Constant yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no Temperature Catalyst ii) 250:(g)+0:(3)2SO:(g) The position of equilibrium moves to the right/left if the concentration of SO; is increased. Co.(g) CO(g)+O( If we increase the pressure of COg), the system will shift towards the reactants/products because it has a fewer/more number of moles of gas. CIHH:0 HO'+Cl+Heat If we decrease the temperature, the reaction will proceed towards the reactants/products because the system must regenerate/used the heat that was lost/gain. iii) Will the equilibrium in reactionarrow_forwardWhich change causes the equilibrium to shift to the product side? 2 CO) + O2(2) 2 CO2(2) AH= - (3)0) 283.3kJ (3)2) (3)2) ORemoving oxygen O Increasing the temperature O Adding carbon dioxide Removing carbon monoxide Decreasing the volumearrow_forward
- State the direction (forward or backward) in which each of the following equilibrium systems would be shifted upon the application of the stress listed beside the equation. (20 points) N,O, 2NOBr increase pressure add a + catalyst add Fe (s) remove CO, increase pressure decrease pressure increase NO, decrease H, decrease temperature increase temperature 2NO, 2NO 01. 02. 03. 04. 05. 06. 3Fe (s) + 4H,0 СаCо, (s) SnO.(s) + 2CO CO + Br. ++ Fe,O. + 4H, Cao (s) + CO, Sn(s) + 20O, CO, 2NO, 2NH, + H,O + Ha 07. 08. 09. 10. 2NO + O, N; C (s) 2S0. + O, 3H, CO: + heat 2C0 heat 2SO, ...arrow_forward2. Given the following equilibrium systems, determine the effect on the equilibrium when the named "stress" is applied. Normally the addition of solids or liquids to an equilibrium has no effect. a 2 NH3 (g) + 92.5 kJ 5 N2(9) + 3 H2 (9) Stress Equilibrium Shift 1 Remove N2 (9) 2 Add NH3 (9) 3 Remove H2 (9) 4 Remove NH3 (9) Add O2 (g) 6 Decrease Pressure 7 Add Heat b Ag2CO3 (s) 5 2 Ag1+ (aq) + CO32 (aq) Stress Equilibrium Shift 1 Add CO32" (aq) Remove Ag* (aq) 1+ 2 3 Add A92CO3 (s) 4 Add heat CANNOT ANSWER 5 Evapourate water offarrow_forward12 (9) H₂ (9) In which direction will equilibrium shift if H2 gas is added to the system? + HI is removed as soon as formed? 2HI (g)arrow_forward
- Le Chatelier’s principle states that “If you stress a system at equilibrium, the system will react to relieve the stress and return to equilibrium”. The following equation represents a chemical reaction at equilibrium: 2A (g) + 3B (g) <===> 2C (g) + 4D (g) ∆H = -378 kcal/mol (g) means gas In each case below, explain how the system reacts (forward direction, reverse direction or no change): The concentration of A is increased Heat is added to the system B is removed from the reaction Pressure is added The concentration of C is increasedarrow_forward7. 2CO2 (g) 200(g) + O2 (g). It was found that at 20 OC, the total pressure at equilibrium is 2.9 atm and that of CO2 is 0.8 atm. Calculate K. (Answer 2.14)arrow_forward1:18 Question 1 of 16 Consider the following chemical reaction at equilibrium: 2NO₂(g) = N₂O4(9) A) reactants If the container's volume is increased by a factor of 2, in which direction will the equilibrium shift? B) product Submit C) neither the reactants nor the product Tap here or pull up for additional resourcesarrow_forward
- Will the equilibrium be established when following compounds are kept in a closed container and allowed time for equilibrium? (5)CaCO3(s) = CaO(s) + CO2(g)(a) CaCO3(s)(b) CaO(s) and CO2(g) at a pressure greater than the value of Kp(c) CaCO3(s) and CO2(g) at a pressure greater than the value of Kp(d) CaCO3(s) and CaO(s)(e) CaO(s) and CO2(g) at a pressure smaller than the value of Kparrow_forwardConsider the following system at equilibrium: P4 (g) + 6 H2 (g) = 4 PH3 (g) ΔΗ 110. 5 kJ If the volume was increased, what changes would have to occur to reestablish equilibrium? Select 2 correct answer(s) The reaction would shift right. The concentration of PH3 would increase. The concentration of P4 would increase The reaction would shift left. The concentration of H2 would decrease.arrow_forward6. 0.300 mole of dinitogen tetraoxide was added to a 2.00 Litre flask. What is the equilibrium concentration of both gases? N2O4 (g) 5 2 NO2 (g) Keg = 4.50arrow_forward
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