Indicate whether either an increase or a decrease of pressure obtained by changing the volume would increase the amount of product in each of the following reactions.a. H2 (g) + F2 (9)= 2HF(g)O An increase of pressure increases the amount of product.OA decrease of pressure increases the amount of product.OPressure change has no effect.b. CO2(9) + CFA(g) 2COF2 (g)O An increase of pressure increases the amount of product.OA decrease of pressure increases the amount of product.OPressure change has no effect.2NO2 (9) = N2O4(9)C.O An increase of pressure increases the amount of product.OA decrease of pressure increases the amount of product.O Pressure change has no effect.

H2(g) + F2(g) ⇔ 2 HF (g)CO2(g) + CF4(g) ⇔ 2 COF2 (g)2 NO2 (g) ⇔ N2O4(g)

Indicate whether either an increase or a decrease of pressure obtained by changing the volume would increase the amount of product in each of the following reactions. a. H2 (9) + F2 (9) 2HF(g) O An increase of pressure increases the amount of product. OA decrease of pressure increases the amount of product. O Pressure change has no effect. b. CO2(9) + CF (9) = 2COF2(9) O An increase of pressure increases the amount of product. OA decrease of pressure increases the amount of product. OPressure change has no effect. C. 2NO2 (g) = N2O4(g) O An increase of pressure increases the amount of product. OA decrease of pressure increases the amount of product. OPressure change has no effect.

Indicate whether either an increase or a decrease of pressure obtained by changing the volume would increase the amount of product in each of the following reactions. a. H2 (9) + F2 (9) 2HF(g) O An increase of pressure increases the amount of product. OA decrease of pressure increases the amount of product. O Pressure change has no effect. b. CO2(9) + CF (9) = 2COF2(9) O An increase of pressure increases the amount of product. OA decrease of pressure increases the amount of product. OPressure change has no effect. C. 2NO2 (g) = N2O4(g) O An increase of pressure increases the amount of product. OA decrease of pressure increases the amount of product. OPressure change has no effect.

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

2 Name: Maile Velazquez Date: Period: 6 H-02 Equilibrium Assignment Instructions: Write the Law of Mass Action for each of the following chemical equations and then calculate the indicated missing variable using the provided information while at equilibrium. Ex H2O + COH₂+ CO₂ 1H2O+ 1CO1H2 + 1CO₂ [H2]¹[CO2]¹ K₂ = Кс 4.73 [H,O][CO] [CO2] = [H2]¹ (4.73)(0.0322)(0.0510) [H2O] 0.0322 M [CO₂] = = 0.0135088 (0.575) [CO] 0.0510 M [H2]¹[CO2] [CO2] = 0.0135 M [H2] 0.575 M [H,O][CO] H₂+2 A₁₂+ B₂ → AB3 [AB3] 0.146 M [A₂] 1.50 M K = K₁ = [B2] 0.240 M
The below reaction at 927 °C has a Kc = 5.78. Calculate the concentration of NO2 at equilibrium after 299 g of NO2 and 416 g of SO2 are introduced into an empty 10.0 L container and heated to 927 °C. NO2 (g) + SO2 (g) ↔ NO (g) + SO3 (g
2. Use the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO3(g). SO2(g) + O2(g) ⇌ SO3(g) Kc = 1.7 × 108 [SO2]eq = 0.0034 M [O2]eq = 0.0018 M
Help 7
Consider the reaction: 2S (s) + 30₂ (9)2SO3(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: 3 80 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K = E D S(s) + O2(g) → SO₂(g) K₁ SO₂(g) + 1/2O₂(g) SO3(9) K₂ 13 с Submit Answer $ 888 FA F4 R F Show Hint V Retry Entire Group 9 more group attempts remaining % 5 T Cengage Learning Cengage Technical Support F G 6 B MacBook Air FO Y H & 7 N F7 U J * 00 8 ➤11 FO I M ( 9 V K O < H дв ) O L F10 question. P command F11 A ; Previous { + alt #2 “ . ? option Save and Exit I 1 delete 1 ente re
12
Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.
5. Consider the equilibrium where Kc = 85.0 at 460°C. The following mixture was prepared in a reactor at 460 °C with the concentrations [SO2] = 0.0200 M; [NO2] = 0.0200 M; [NO] = 0.100 M; [SO3] = 0.100 M. What will the concentrations of the four gases be when equilibrium is reached? SO2 (g) + NO2 (g) - NO (g) + S03 (g); Ke = 85.0 I 0.02 O. 02 C -x E 6.02- 0,02-0 0.ltx 0.lto 一× +x 十 LNOJ CSOPJ ) T02=x)co-02-) కంటె CN6 kc
64. Consider this reaction at equilibrium: 2 BRNO(g) = 2 NO(g) + Br2(8) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a. NO is added to the reaction mixture. b. BINO is added to the reaction mixture. c. Brz is removed from the reaction mixture.
#9
Consider the following equilibrium: N204(g) = 2NO2(g) Suppose two different experiments were conducted on this equilibrium, at two different temperatures. Trial Temperature Initial Moles of N204 Equilibrium Moles of N204 1 25°C 1.00 0.815 55°C 1.00 0.500 What conclusion may be drawn from the above data? O Kc> Kp at all temperatures. The reaction is exothermic. The forward reaction proceeds faster than the reverse reaction. OKp =D1 at 55°C. O The equilibrium constant increases with increasing temperature.