The image presents a question about chemical equilibrium, specifically asking for which reactions the equilibrium constants \( K_p \) and \( K_c \) are equal.**Question:**For which of the following reactions is \( K_p = K_c \)?I. \( \text{CO(g)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{CO}_2\text{(g)} + \text{H}_2\text{(g)} \)II. \( \text{H}_2\text{(g)} + \text{Br}_2\text{(l)} \rightleftharpoons 2\text{HBr(g)} \)III. \( 2\text{NO(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{NO}_2\text{(g)} \)IV. \( \text{N}_2\text{(g)} + 2\text{H}_2\text{(g)} \rightleftharpoons \text{N}_2\text{H}_4\text{(g)} \)V. \( \text{Cl}_2\text{(g)} + \text{F}_2\text{(g)} \rightleftharpoons 2\text{ClF(g)} \)**Options:**- IV only- I only- III only- II only- V only**Explanation:**For \( K_p \) to be equal to \( K_c \), the change in the number of moles of gas (\( \Delta n \)) in the reaction must be zero. The reactions with no change in the number of gas molecules on either side will have \( K_p = K_c \).**Solution:**- Reaction I: \( \Delta n = 1 \) (1 gas product, 0 gas reactants)- Reaction II: \( \Delta n = 1 \) (1 gas product, 0 gas reactants)- Reaction III: \( \Delta n = 0 \) (2 gas products, 2 gas reactants)- Reaction IV: \( \Delta n = -1 \) (1 gas product, 2 gas reactants)- Reaction V: \( \Delta n = 0 \

For which of the following reactions is Kp = Kc? I. CO(g) + H20(1) = CO2(g) + H2(g) II. H2(g) + Br2(1) = 2HBr(g) III. 2NO(g) + O2(g) = IV. N2(g) + 2H2(g) = N2H4(g) V. Ch(9) + F2(9) = 2CIF(g) 2NO2(g) IV only I only O Ill only O Il only O vonly

For which of the following reactions is Kp = Kc? I. CO(g) + H20(1) = CO2(g) + H2(g) II. H2(g) + Br2(1) = 2HBr(g) III. 2NO(g) + O2(g) = IV. N2(g) + 2H2(g) = N2H4(g) V. Ch(9) + F2(9) = 2CIF(g) 2NO2(g) IV only I only O Ill only O Il only O vonly

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the reaction at a particular temperature: 2NO2(g) = 2NO(g) + O2(g) K, = 8.1 x 1012 Determine the Kp in scientific notation of the following reaction at the particular temperature: 4NO2(g) = 4NO(g) + 202(g) If the answer is 2.5 x 10, express the answer as 2.5E-2.
Consider the reaction: N₂O4 (9) — 2NO2 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: N₂(g) +202 (g) = N₂O4 (9) K₁ 1/2N₂(g) + O2(g) — NO2(g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K=
The Keg for the equilibrium below is 7.82 · 10-2 at 510.0 °C. 2Cl, (g) + 2H20 (g) =4HCI (g) + 02 (g) What is the value of Keg at this temperature for the following reaction? Cl2 (g) + H20 (g) = 2HCI (g) + 02 (g) O 0.280 O 0.0376 O 6.12 - 10-3 O 0.150 O 0.0782
Gg.124.
Consider the following reaction where Kc = 1.20×10-2 at 500 K:PCl5 (g) PCl3 (g) + Cl2 (g)A reaction mixture was found to contain 0.115 moles of PCl5 (g), 4.47×10-2 moles of PCl3 (g), and 4.16×10-2 moles of Cl2 (g), in a 1.00 liter container.Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium PCl5(g) must be consumed . 2. In order to reach equilibrium Kc must increase . 3. In order to reach equilibrium PCl3 must be consumed . 4. Qc is less than Kc. 5. The reaction is at equilibrium. No further reaction will occur.
H2(g) + I2(g) 2 HI(g) AH=120 kJ e) In which direction will the equilibrium shift (for the first reaction) when (i) HI(g) is removed, (ii) the temperature is decreased, (ii) the volume of the reaction system is increased, (ii) H2(g) is added?
3. Phosphoryl chloride, POCI3(g), is used in the manufacturing of flame retardants. It is manufactured in an equilibrium process in which phosphorus trichloride reacts with nitrogen dioxide to form POCI3(8)and NO(g) according to the following equation: PCI3 (g) + NO2 (g) = POCI3 (g) + NO (g) The Keg for this reaction at 800 K is 6.90. If 1.25 mol PCI3 (g) and 1.94 mol NO2 (g) are placed into a 2.0 L container, what is the concentration of each gas at equilibrium at 800 K? PCI3 (g) NO2 (g) POCI3 (g) NO(g) Keq = 6.90 + + E
For which one of the following reactions is Kp equal to Kc? CaCO3(s) = CaO(s) + CO₂(g) 2NH3(g) = 3H₂(g) + N₂(g) 302(g) = 203(g) SnO2(s) + 2H₂(g) Sn(s) + 2H₂O(g) NH41(s) NH3(g) + HI(g)
Consider the following reaction where K, = 6.50x10-3 at 298 K. 2NOBR(g) =2NO(g) + Br2(g) A reaction mixture was found to contain 8.79x10-2 moles of NOBR(g), 2.03x10-2 moles of NO(g), and 4.53x10 2 moles of Bro(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
Consider the following equilibrium: 2NO(g) + Cl₂ (g) 2NOCI (g) AG=-41. kJ Now suppose a reaction vessel is filled with 1.55 atm of chlorine (C1₂). about this system: T Under these conditions, will the pressure of NOCI tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOC1 will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if said the pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. and 4.77 atm of nitrosyl chloride (NOCI) at 683. °C. Answer the following questions Orise Ofall yes Ono atm O x10 X S
4) Choose the reactions below where K and K are equal. 302 (g) = 203 (9) CO (g) + H2O (g) = CO2 (g) + H2 (9) N2 (g) + 3H2 (g) 2NH3 (g) N2 (g) + O2 (9) : 2ΝΟ ( g)