CONNECT IA GENERAL ORGANIC&BIO CHEMISTRY
4th Edition
ISBN: 9781260562620
Author: SMITH
Publisher: MCG
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Chapter 6.5, Problem 6.9PP
Consider the reversible reaction
More Practice: Try Problems 6.49, 6.50.
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6. Given the following reaction: 3 H2(g) + N2(g) ? 2 2 NH;(g) + heat
Fill in the following chart (please use a different font color):
Changes/Stress on
system
Ex. Adding H2
Direction of shift
Reason for shift
(left or right)
right
To decrease excess H2 and
increase NH3
Adding NH3
Decreasing the
pressure
Adding heat
Removing N,
Increasing the pressure
Chem help! 7.6
(Incorrect)
1.00 atm N₂O5 is placed in an evacuated vessel and reacts according to the equation
2 N₂O5(g) 4 NO₂(g) +O₂(g)
When equilibrium is reached, the partial pressure of NO2 is found to be 1.60 atm. Calculate Kp for this reaction?
4.1 (Your answer)
84
26
66 (Correct answer)
13
Chapter 6 Solutions
CONNECT IA GENERAL ORGANIC&BIO CHEMISTRY
Ch. 6.1 - Prob. 6.1PPCh. 6.1 - Prob. 6.1PCh. 6.1 - Prob. 6.2PPCh. 6.1 - Prob. 6.2PCh. 6.2 - Using the values in Table 6.2, give H for each...Ch. 6.2 - Prob. 6.4PPCh. 6.2 - Answer the following questions using the given...Ch. 6.2 - Given the H and balanced equation in Sample...Ch. 6.2 - Prob. 6.6PPCh. 6.3 - Prob. 6.7PP
Ch. 6.4 - Consider the reaction of ozone (O3) with nitrogen...Ch. 6.4 - Draw an energy diagram for an uncatalyzed...Ch. 6.5 - Identify the forward and reverse reactions in each...Ch. 6.5 - Write the expression for the equilibrium constant...Ch. 6.5 - Consider the reversible reaction AB, with K=1....Ch. 6.5 - Given each equilibrium constant, state whether the...Ch. 6.5 - Consider the following reaction:...Ch. 6.5 - Using the equilibrium mixture of reactants and...Ch. 6.5 - Calculate the equilibrium constant for each...Ch. 6.5 - Consider the representation depicted in the...Ch. 6.6 - Prob. 6.13PPCh. 6.6 - Prob. 6.14PPCh. 6.6 - wThe conversion of H2O to H2 and O2 is an...Ch. 6.6 - The reaction of O2 with NO to form NO2 and O2 is...Ch. 6.6 - wIn which direction is the equilibrium shifted in...Ch. 6.6 - Label each statement about the following...Ch. 6 - Prob. 11PCh. 6 - Prob. 12PCh. 6 - Prob. 13PCh. 6 - Prob. 14PCh. 6 - Prob. 15PCh. 6 - Prob. 16PCh. 6 - Prob. 17PCh. 6 - Prob. 18PCh. 6 - Prob. 19PCh. 6 - Prob. 20PCh. 6 - Prob. 21PCh. 6 - Prob. 22PCh. 6 - Prob. 23PCh. 6 - Prob. 24PCh. 6 - Prob. 25PCh. 6 - Prob. 26PCh. 6 - Prob. 27PCh. 6 - Ammonia ( NH3 ) decomposes to hydrogen and...Ch. 6 - Prob. 29PCh. 6 - Ethanol ( C2H6O ), a gasoline additive, is formed...Ch. 6 - Prob. 31PCh. 6 - Prob. 32PCh. 6 - Prob. 33PCh. 6 - Prob. 34PCh. 6 - Draw an energy diagram for the following reaction...Ch. 6 - Prob. 36PCh. 6 - State two reasons why increasing temperature...Ch. 6 - Why does decreasing concentration decrease the...Ch. 6 - Prob. 39PCh. 6 - Prob. 40PCh. 6 - Which of the following affect the rate of a...Ch. 6 - Prob. 42PCh. 6 - How does a catalyst affect each of the following:...Ch. 6 - What is the difference between a catalyst and an...Ch. 6 - Prob. 45PCh. 6 - Consider the representation depicted in the...Ch. 6 - For each value, are the reactants or products...Ch. 6 - Prob. 48PCh. 6 - Prob. 49PCh. 6 - Prob. 50PCh. 6 - Prob. 51PCh. 6 - Consider three different equilibrium mixtures...Ch. 6 - Write an expression for the equilibrium constant...Ch. 6 - Write an expression for the equilibrium constant...Ch. 6 - Prob. 55PCh. 6 - Use each expression for the equilibrium constant...Ch. 6 - Prob. 57PCh. 6 - Consider the following reaction:...Ch. 6 - Prob. 59PCh. 6 - Which of the following representations ([1][3]) of...Ch. 6 - Consider the following reaction....Ch. 6 - Consider the following reaction. H2(g)+I2(g)2HI(g)...Ch. 6 - Prob. 63PCh. 6 - Prob. 64PCh. 6 - Consider the reaction of N2(g)+O2(g)2NO(g). What...Ch. 6 - Consider the reaction of H2(g)+F2(g)2HF(g). What...Ch. 6 - Prob. 67PCh. 6 - Consider the reversible reaction ABA+B, shown at...Ch. 6 - Consider the endothermic conversion of oxygen to...Ch. 6 - Consider the exothermic reaction:...Ch. 6 - Consider the exothermic reaction:...Ch. 6 - Consider the endothermic reaction:...Ch. 6 - Consider the gas-phase reaction of ethylene...Ch. 6 - Methanol (CHO), which is used as a fuel in race...Ch. 6 - Prob. 75PCh. 6 - How does a catalytic converter clean up automobile...Ch. 6 - Prob. 77PCh. 6 - The reaction of salicylic acid with acetic acid...Ch. 6 - Prob. 79PCh. 6 - Prob. 80PCh. 6 - Prob. 81PCh. 6 - Prob. 82PCh. 6 - Prob. 83CPCh. 6 - Prob. 84CP
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- 1. (4 pts total) Consider the following equilibrium, for which Kp 0.00154 at 500 °C: N2 (g) 2 H;0 (e) 2 NO (e) 2 H2 (g) Kp = 0.00154 a) (2 pts) What predominates at equilibrium, reactants or products? Why? Circle one: Reactants or Products Why? (2 pts) Calculate Kp for the reaction below. Use the original reaction above as reference: % H,O (e) b) » H; (e) %N; (8) +] 1, % NO (8) ANSWER:arrow_forward6. A 3.75-L vessel contains 0.444 mol SO3, 0,632 mol O2, and 2.125 mol SO2 at 230°C in an equilibrium mixture. Calculate the value of Kc at 230°C. (1 2SO2(g) + O2 (g) 2SO3 (9)arrow_forwardGive correct answerarrow_forward
- 3.3 The following diagram represents the equilibrium state for the reaction: A2 (g) + 2 B (g) 2 AB (g) Key A2 00 АВ a) Assuming the volume is 1 dm', calculate the equilibrium constant for the reaction. b) If the volume of the equilibrium mixture is decreased, will the number of AB molecules increase or decrease? Say why. c) Below are two diagrams showing a microscopic representation of the reaction: X2 + Y AX + XY The diagrams represent the same reaction at two different temperatures: 300 K and 500 K. Is the reaction exothermic or endothermic? Say why. T= 300 K T= 500K Key XYarrow_forward2 and 3arrow_forwardDoarrow_forward
- 10. 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_forward1.3. You start with 15.0 atm of N₂O4(g) and no NO2(g), and you let it reach equilibrium. If you measure that the pressure of NO₂(g) is 3.0 atm at equilibrium, how much N₂O4(g) is left? N₂O4(g) 2 NO₂(g) a) 3.0 atm b) 9.0 atm c) 12.0 atm d) 13.5 atmarrow_forwardcomuarrow_forwardl Verizon ? 1:11 AM 77% 4 Question 4 of 7 Submit Consider the following reaction at equilibrium CO(g) + H20(g) =CO2(g) + H2(g) If CO(g) is removed, in which direction will the equilibrium shift? A) reactants B) products C) no change Tap here or pull up for additional resourcesarrow_forwardEquilibrium reaction Keq expression Stress applied Effect Equilibrium Shi (encircle your answer) (encircle your answer) (increase, decrease, change) in H2le) + Cl2te) 2 HCI(g) Decreasing the Forward pressure no Backward (HCI)2 the No Shift K= ( H2)(Cl2) number of moles of HCl(g) e (increase, decrease, change) in Fe;O4(s) + 4 H2(g) + heat 3 Fe(s) + 4 Increasing Forward temperature Backward no H,O(g) (H20)* the No Shift K= (H2)4 volume of water 2 NO(g) + O,(g) 2 NO2(g) + heat vapor collected f (increase, Addition Forward helium decrease, Backward no K= (NO2)? change) in the No Shift (NO)2 (02) number of moles of NO H,CO3(aq) CO.(aq) + H,0(1) Removal of C (increase, decrease, change) amount of H,CO3 (increase, decrease, change) amount of O2 Forward (CO2) K= no Backward (H2CO3) in the No Shift 4 NH3(g) + 5 0,(g)4 NO(g) H,O(g) + heat Increasing Forward + 6 (NO )* (H20) temperature K= no Backward (NH3) (02)5 in the No Shiftarrow_forwardH2(g) + 12(g) = 2HI(g) (= is equilibrium sign) At particular temperature, The equilibrium constant (K) = 100 If 1.0 mole of H2, 1.0 mol of I2 and 1.79 mol of HI are introduced into 1.00 L container. The concentration of HI when equilibrium is reached is Write your answer to 1 d.p e.g 7.6 Answer:arrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
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