An aqueous mixture of phenol and ammonia has initial concentration of 0.200 M C_

Question

An aqueous mixture of phenol and ammonia has initial concentration of 0.200 M C_6 H_5 OH(aq) and 0.120 N NH_3 (aq). At equilibrium the C_6 H_5 O^- (aq) concentration is 0.050 M. Calculate K for the reaction C_6 H_5 OH (aq) + NH+_3 (aq) C_6 H_5 O^- + NH_4^+ (aq) a. 0.10 b. 0.24 c. 2.1 d. 4.2 e. 4.8 The equilibrium constant, K_z, for the decomposition of ammonium hydrogen sulfide is 1.8 times 10^-4 at 25 degree C NH_4 HS(s) NH_3 (g) + H_2 S (g) If excess NH_4 HS(s) is allowed to equilibrate at 25 degree C, what is the equilibrium concentration of NH_3? a. 3.2 times 10^-8 M b. 9.0 times 10^-6 M c. 1.8 times 10^-4 M d. 6.7 times 10^-3 M e. 1.3 times 10^-2 M Consider the following equilibrium CO_2 (g) + H_2 (g) CO(g) + H_2 O (g); K_c = 1.6 at 1260 K Suppose 0.019 mol CO_2 and 0.030 mol H_2 are placed in a 3.00-L vessel at 1260 K. What is the equilibrium pressure of CO(g)? (R = 0.0821 L middot atm/K middot mol) a. 4 atm b. 0.35 atm c. 1.6 atm d. 0.66 atm e. 1 atm

Explanation / Answer

Ans 27 option a 0.10

At equilibrium the concentration of phenoxide ion and ammonium ion will be equal that is 0.050 M

Kc = [ C6H5O]- [NH4]+ / [ C6H5OH] [ NH3]

= 0.050 × 0.050 / 0.200 × 0.120

= 0.10

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