For each of the following values of K, indicate whether the forward reaction, reverse reaction, or neither would be favored. a) Keq = 4.1 x 10-3 (K<<<1) b) Keq = 3.7 x 108 (K>>>1) c) Keq = 1.47 (K~1)
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For each of the following values of K, indicate whether the forward reaction, reverse reaction, or neither would be favored.
a) Keq = 4.1 x 10-3 (K<<<1)
b) Keq = 3.7 x 108 (K>>>1)
c) Keq = 1.47 (K~1)
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- Does the equilibrium lie to the left or to the right in the following reaction: H3CO: + H-Br: 2 H;CO-H + H,CO-H + Br:(Q9) The base ionization constant for (Kp) for acetate ion (CH3CO0') is equal to: O 4.75 9.25 O 1.8 x 10-5 O Is undefined (i.e., there is no such thing) 5.6 x 10-104, . Consider the following equilibrium: base + -H H-Base Which of the following base(s) would favour the product in this reaction? Он CH;O NH3 NH2 CH3CO2 (1) (II) (III) (IV) (V) (a) | (b) IV (c) I, IV and V (d) I and II (e) IIl and IV
- 1) Indicate if the left of the right species are favored at equilibrium. Use equilibrium arrows with a larger arrow to indicate the favored side. a) b) c) =H d) SH N + NaO + : OH NH F ÖH NH SNa+ + НО 00 Eye N:8:43 1 ll 5GE Question 10 of 25 Submit Construct the expression for Kb for the weak base, CsH;N. CsH,N(aq) + H20(1) = OH (aq) + CsH;NH* (aq) 1 Based on the definition of Kb, drag the tiles to construct the expression for the given base. Kp = 5 RESET [H,O] [H;O*] [OH] [C;H;N] [C;H;NH*] [C;H,N¯] 2[H;O] 2[H;O*] 2[ОН] 2[C;H;N] 2[C;H;NH*] 2[C5H&N¯] [H,O]? [H;O*]? [OH]? [CsH;N]? [C;H;NH*]? [C;H,N¯]?One way to determine the predominant species at equilibrium for an acid-base reaction is to say that the reaction arrow points to the acid with the higher value of pK. For example, NH, + H,0 NH, + H,O+ pK. pk, 9.24 pK-1.74 NH,+ + OH--→ NH, + H,0 рк, 9.24 pK, 15.7 Explain why this rule works.
- 8:43 1 5G E Question 13 of 25 Submit Determine concentration of OH in a 0.60 M solution of HNO2 (Ka = 7.1 x 10-4). 1 2 3 Based on the given values, set up ICE table in order to determine the unknown. HNO2(aq)+ H20(1) =H;O*(aq) + NO, (aq) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.60 7.1 × 10-4 1.4 x 10-11 0.30 +x -X +2x -2x 0.60 + x 0.60 - x 0.60 + 2x 0.020 - 2x 1.4 × 10-1" + x 1.4 × 10-11 - x 1.4 x 10-11 + 2х 1.4 x 10-11 - 2xF3 The value of K₂ for formic acid, HCOOH, Is 1.80x10-4. Write the equation for the reaction that goes with this equilibrium constant. (Use H3O+ Instead of H*.) $ 4 Submit Answer 000 000 F4 R LL + % 5 T G Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support A 6 MacBook Air S F6 Y H & 7 ◄◄ + F7 U J * 8 ▶11 F8 1 9 K F9 O 0 L F10 P Previous F11 + 11 1 Next Save aHCN (g)+ H2O (l) ⇌ H+ (aq) + CN- (aq) how would decreasing [CN-] shift the equilibrium?
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