Practice Problem BUILD
Consider a weak acid, HA, that ionizes according to the equation:
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Chemistry
- (Incorrect) For the reaction 2A(g) + B(s) C() + 2D(g) at 700 °C, Kc = 0.00577. Calculate the number of moles of D present at equilibrium if a mixture of 6.03 moles of C and 6.03 moles of D is heated to 700 °C in a 7.61-L container. 0.0074 mol (Your answer) 0.430 mol (Correct answer) 5.60 mol 0.056 molarrow_forwardGiven a K value of 4.6 X 10-12, would you expect a nearly complete reaction at equilibrium? yes no insufficient informationarrow_forwardA(aq)−⇀↽−2B(aq)Kc=6.14×10−6 at 500 KA(aq)↽−−⇀2B(aq)Kc=6.14×10−6 at 500 K If a 3.00 M3.00 M sample of AA is heated to 500 K,500 K, what is the concentration of BB at equilibrium?arrow_forward
- TUTOR Calculate K from Equilibrium Concentrations Some SO, is placed in a sealed flask and heated to 1350 K. When equilibrium is reached, the flask is found to contain SO3 (6.00×10 M), SO, (3.47x102 M), and O2 (1.59×10-² M). What is the value of the equilibrium constant for this reaction at 1350 K? 2S03(g) 2SO2(g) + O2(g) K=arrow_forwardFor the equilibrium system N2044) # 2NO26) what is the equilibrium constant when [N2O4) is 1.5 x 10-3 M and [NO2] is 0.57 M? (B) 2.2 × 102 . (A) 3.8 × 10² (C) 4.6 × 10-3 (D) 2.6 × 10-3arrow_forwardHow would the series of figures change in the presence of a catalyst? Would there be different amounts of reactants and products in the final figure (vi) in the presence of a catalyst? Match the words in the left column to the appropriate blanks in the sentences on the right. sooner increases before equilibrium decreases after equilibrium does not change A catalyst and it the rate of the reaction, the concentration of the product at equilibrium conditions. Reset Thus, condition (iii) would occur Help of reactants concentration of the product Condition (vi) would show that the concentration and thearrow_forward
- Macmillan Learn A(aq) 3 B(aq) K = 9.43 x 10-6 If a 4.10 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? at 500 K [B] = Marrow_forwardPractice Exercise At 1280°C the equilibrium constant (K) for the reaction Br2(g) 2Br(g) is 1.1 x 10 . If the initial concentrations are [Br2] 102 M, calculate the concentrations of these species at equilibrium. 6.3 x 10 2 M and [Br] = 1.2 X !!arrow_forwardQuestion 10 O out of 1 points For the reaction, N2g) + 02(g) = 2 NO(g), at 1500 K, the value of the equilibirum constant Kc = 2.9 x 105. If a sample has an initial concentration for N2 of 0.51 M and an initial concentration for 0, of 0.22 M, what is the equilibrium concentration of NO? Report your answer to the tenths place and use scientific notation (e.g., 1.2e-3 or 1.2e3).arrow_forward
- Question 21 Hydrogen iodide can be produced by the reversible reaction of hydrogen gas and iodine gas according to: H2(g) + I2(g) = 2HI(g) Keg for this reaction is 2.25 × 10³ at a temperature of 753°C. Calculate the concentration of HI in an equilibrium mixture if the concentration of H2 is 0.15 M and the concentration of I2 is 0.25 M. (a) 2.4 moles of H2(g) and 1.5 moles of I2(g) were placed in a sealed 2.0 L vessel maintained at a temperature of 753°C. After 2 hours, the number of moles of each gas present were as follows. (b) Moles of H2(g) Moles of I2(g) Moles of HI(g) 1.7 0.8 1.4 Show by calculation whether the forward or reverse reaction must increase for the system to come to a state of dynamic equilibrium.arrow_forwardQ Search this course Reference Use the References to access importantv needed for this question. The equilibrium constant, K, for the following reaction is 1.20x102 at 500 K PCI5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.164 M PCI 4.43x10 M PCI3 and 4.43x10 M C2. What will be the concentrations of the three gases equilibrium has been reestablished, if 2.27x10 mol of Ch(g) is added to the flask? once [PCI5]= [PCI3]= М [Cl2] sturbing Equilibrium Concentrations (Qua... : This is group attempt 1 of 5 Next ack 1:33 PM 9/24/2019 up Xxarrow_forwardPractice Exercise At 1280°C the equilibrium constant (K.) for the reaction Br2(g) = 2Br(g) is 1.1 x 10-3. If the initial concentrations are [Br2] 6.3 x 10-2 M and [Br] = 1.2 × 10-2 M, calculate the concentrations of these species at equilibrium.arrow_forward
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