Equal amounts of two acids—HCl and HCO2H (formic acid)—are placed in aqueous solution. When equilibrium has been achieved, the HCl solution has a much greater electrical conductivity than the HCO2H solution. Which reaction is more product-favored at equilibrium?
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Chapter 3 Solutions
Chemistry & Chemical Reactivity
- Calculate equilibrium constants for the following reactions at 208 K. Indicate whether the equilibrium as written is reactant- or product-favored at equilibrium. (a) Co(s) + Ni2+(aq) Co2+(aq) + Ni(s) (b) Fe3+(aq) + Cr2+(aq) Cr3+(aq) + Fe2+(aq)arrow_forwardHydrogenation, the addition of hydrogen to an organic compound, is an industrially important reaction. Calculate rH, rS, and rG for the hydrogenation of octene, C8H16, to give octane, C8H19 at 25 C. Is the reaction product- or reactant-favored at equilibrium? C8H16(g) + H2(g) C8H18(g) Along with data in Appendix L, the following information is needed for this calculation.arrow_forwardConsider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?arrow_forward
- Heating a metal carbonate leads to decomposition. BaCO3(s) BaO(s) + CO2(g) Predict the effect on the equilibrium of each change listed below. Answer by choosing (i) no change, (ii) shifts left or (iii) shifts right. (a) add BaCO3 (b) add CO2 (c) add BaO (d) raise the temperature (e) increase the volume of the flask containing the reactionarrow_forwardThe formation of ammonia from its elements is an important industrial process. 3 H2(g) + N2(g) 2 NH3(g) 1. Does the reaction shift to the right or to the left, or does it remain unchanged, when extra H2 is added? (a) shift left (b) shift right (c)unchangedarrow_forwardUsing the following data, calculate the value of Ksp for Ba(NO3)2, one of the least soluble of the common nitrate salts. Species Gfo Ba2+(aq) 561 KJ/mol NO3(aq) 109 KJ/mol Ba(NO3)2(s) 797KJ/molarrow_forward
- Given the following descriptions of reversible reactions, write a balanced net ionic equation (simplest whole-number coefficients) and the equilibrium constant expression (K) for each. (a) Liquid acetone (C3H6O) is in equilibrium with its vapor. (b) Hydrogen gas reduces nitrogen dioxide gas to form ammonia and steam. (c) Hydrogen sulfide gas (H2S) bubbled into an aqueous solution of lead(ll) ions produces lead sulfide precipitate and hydrogen ions.arrow_forwardConsider the system SO3(g)SO2(g)+12 O2(g)H=98.9kJ (a) Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by 1. adding oxygen gas. 2. compressing the system at constant temperature. 3. adding argon gas. 4. removing SO2(g). 5. decreasing the temperature. (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forwardFor the reaction below, indicate whether the equilibrium tends "to the left", "to the right" or "no effect" when the pressure increases. Al3+(aq) + 3 OH-(aq) ⇌ Al(OH)3(s)arrow_forward
- Consider the two statements below for the equilibrium reaction H2 + I2 = 2 HI (1) At some point in the reaction, the amounts of H2, I2, and HI no longer change and the reaction stops. (2) For acids - both strong and weak - the equilibrium reaction with water is product favored. Group of answer choices Both (1) and (2) are correct Only (2) is correct and (1) is incorrect. Both (1) and (2) are incorrect Only (1) is correct and (2) is incorrect.arrow_forwardPredict the effect of the following changes on the reaction whether if favours reverse, forward or no reaction direction in the space provided. 2 NO(g) + O2 (g) <-> 2 NO2 (g) Ho = -120 kJ Adding catalyst a. reverse b. forward c. no reaction Increasing the temperature of the reaction. a. reverse b. forward c. no reactionarrow_forward3H2 + N2 <--> 2NH3 Keq at 300 K = 4.34 x 10-3 At some point after the reaction above has begun, a sample of the reaction mixture is taken and analyzed for concentration. The concentrations found are: [NH3]= 0.01M [N2]= 0.2M [H2]=0.3M Calculate Q. Has the reaction reached equilibrium? If not, which direction does the reaction have to go to reach equilibrium?arrow_forward
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