Homework Answers
This is an exothermic reaction , thus Heat can considered as a products.
P4S3 (g) + 8 O2 (g) <===> P4O10 (s) + 3 SO2 (g) + Heat
If Heat is removed :
Ans. : system will shift towards products to re-Achieve equilibrium.
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Consider the following equilibrium reaction. P4S3(g) + 8O2(g) = P4010(s) + 3SO2(9) AH = -3677 kJ...
1. Determine the change in the boiling point (ΔTB) and Bp for a solution containing 0.328...
1. Determine the change in the boiling point (ΔTB) and Bp for a solution containing 0.328 moles of naphthalene (a nonvolatile, non-electrolyte compound) in 250. g of liquid benzene (Bp° = 80.1°C)? (Kb = 2.53˚ C/m) 3.32 °C and 76.8 °C 3.32 °C and 83.4 °C 4.31 °C and 0 °C 7.41 °C and 72.7 °C 7.41 °C and 87.5 °C 2. Consider the following equilibrium reaction. P4S3(g) + 8O2(g) ⇌ P4O10(s) + 3SO2(g) ΔH = –3677 kJ If heat...
Consider the reaction 2H2 (g) + O2 (g) 2H2O(g) How will the equilibrium shift when hyDragen...
Consider the reaction 2H2 (g) + O2 (g) 2H2O(g) How will the equilibrium shift when hyDragen gas is removed? The reaction will shift toward both the reactants and products. The reaction will not shift toward either the products or reactants. The system will shift toward the reactants. The system will shift toward the products. Consider the exothermic reaction Fe2O3(s) + 2Al(s) Al2O3(s) + 2Fe(s) In what direction will the equilibrium shift when heat is removed? The reaction will shift toward...
1) 2) 3) C3H8(g) + 5 O2(g) = 3 CO2(g) + 4H2O(1) AH = -2220 kJ...
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C3H8(g) + 5 O2(g) = 3 CO2(g) + 4H2O(1) AH = -2220 kJ Decreasing the temperature will result in shift the equilibrium to the right shift the equilibrium to the left Keq is decreased O no effect in shifting the equilibrium more information is needed Which of the following expressions is the correct equilibrium-constant expression for the reaction below? P4010(s) = P4(s) + 5 O2(g) [02]-5 O [0215 [P4010] [Pd][02] [P][0215 O [P4010] [P4010) [P][0,1175 A proposed...
The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2502(g) + O2(g)...
The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2502(g) + O2(g) = 2503(g) If initial concentrations are [SO2] = 10.8 M, [O2] = 0.45 M, and (SO3) = 16.2 M, the system is not at equilibrium and will remain in an unequilibrated state. not at equilibrium and will shift to the left to achieve an equilibrium state. O at equilibrium. not at equilibrium and will shift to the right to achieve an equilibrium state.
Consider the following reaction at equilibrium: 2CO2(g) = 200 (g) + O2(g) AH° = -514 kJ...
Consider the following reaction at equilibrium: 2CO2(g) = 200 (g) + O2(g) AH° = -514 kJ Le Châtelier's principle predicts that a decrease in temperature will decrease the value of the equilibrium constant O increase the value of the equilibrium constant decrease the partial pressure of CO increase the partial pressure of CO2 (g) decrease the partial pressure of O2 (g) Consider the following reaction at equilibrium: 2NH3 (g) = N2 (g) + 3H2(g) AH° = +92.4 kJ Le Châtelier's...
A reaction that has a positive AH and a positive AS will be spontaneous at high...
A reaction that has a positive AH and a positive AS will be spontaneous at high temperatures spontaneous at low temperatures spontaneous at all temperatures nonspontaneous at all temperatures QUESTION 6 Which of the following statements is FALSE? Keg for a reaction written in reverse is the reciprocal of the key for the forward reaction A reaction quotient (Q) larger than Keq means that the reaction will shift toward reactants Chemical equilibrium indicates that reactants and products are present in...
Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above...
Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above reaction is allowed to reach equilibrium prior to the following changes. Answer the following questions by writing increase, decrease or remain the same on the line. **please also explain why** If the reaction mixture is heated up , the value of the equilibrium constant will _______________________ If SO2 (g) is added to the reaction vessel the concentration of O2(g) will____________________________. If SO3 (g) is...
Consider the following system at equilibrium where AH° = 198 kJ, and Kc - 2.9010-2 at...
Consider the following system at equilibrium where AH° = 198 kJ, and Kc - 2.9010-2 at 1150 K. 2SO3(g) 2502(g) + O2(g) When 0.33 moles of SO2(g) are added to the equilibrium system at constant temperature: The value of Kc The value of Qc Kc The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. The concentration of O2 will Submit Answer Retry...
Consider the following reaction and its equilibrium constant 0.43 SO2(g) + NO (9) = SO.(g) + NO(g) K = 0.33 A reac...
Consider the following reaction and its equilibrium constant 0.43 SO2(g) + NO (9) = SO.(g) + NO(g) K = 0.33 A reaction mixture contains 0.49 M SO. 0.14 M NO, 0.12 M SO, and 0.14 M NO. Which of the following statements is TRUE concerning this system? b. ooo The reaction will shift in the direction of reactants. The equilibrium constant will decrease. The reaction will shift in the direction of products. The reaction quotient will decrease. The system is...
Consider the following equilibrium for which H = 664.38: N2(g) + 2 H2O(g) 2 NO(g) +...
Consider the following equilibrium for which H = 664.38: N2(g) + 2 H2O(g) 2 NO(g) + 2 H2(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction? (a) NO(g) is added to the system. (b) The reaction mixture is heated. (c) The volume of the reaction vessel is reduced by 50%. (d) A catalyst is added to the reaction mixture. (e) The total pressure of the system is increased by adding...
Consider the reaction 2H2 (g) + O2 (g) 2H2O(g) How will the equilibrium shift when hyDragen gas is removed? The reaction will shift toward both the reactants and products. The reaction will not shift toward either the products or reactants. The system will shift toward the reactants. The system will shift toward the products. Consider the exothermic reaction Fe2O3(s) + 2Al(s) Al2O3(s) + 2Fe(s) In what direction will the equilibrium shift when heat is removed? The reaction will shift toward...
1)
2)
3)
C3H8(g) + 5 O2(g) = 3 CO2(g) + 4H2O(1) AH = -2220 kJ Decreasing the temperature will result in shift the equilibrium to the right shift the equilibrium to the left Keq is decreased O no effect in shifting the equilibrium more information is needed Which of the following expressions is the correct equilibrium-constant expression for the reaction below? P4010(s) = P4(s) + 5 O2(g) [02]-5 O [0215 [P4010] [Pd][02] [P][0215 O [P4010] [P4010) [P][0,1175 A proposed...
The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2502(g) + O2(g) = 2503(g) If initial concentrations are [SO2] = 10.8 M, [O2] = 0.45 M, and (SO3) = 16.2 M, the system is not at equilibrium and will remain in an unequilibrated state. not at equilibrium and will shift to the left to achieve an equilibrium state. O at equilibrium. not at equilibrium and will shift to the right to achieve an equilibrium state.
Consider the following reaction at equilibrium: 2CO2(g) = 200 (g) + O2(g) AH° = -514 kJ Le Châtelier's principle predicts that a decrease in temperature will decrease the value of the equilibrium constant O increase the value of the equilibrium constant decrease the partial pressure of CO increase the partial pressure of CO2 (g) decrease the partial pressure of O2 (g) Consider the following reaction at equilibrium: 2NH3 (g) = N2 (g) + 3H2(g) AH° = +92.4 kJ Le Châtelier's...
A reaction that has a positive AH and a positive AS will be spontaneous at high temperatures spontaneous at low temperatures spontaneous at all temperatures nonspontaneous at all temperatures QUESTION 6 Which of the following statements is FALSE? Keg for a reaction written in reverse is the reciprocal of the key for the forward reaction A reaction quotient (Q) larger than Keq means that the reaction will shift toward reactants Chemical equilibrium indicates that reactants and products are present in...
Consider the following system at equilibrium where AH° = 198 kJ, and Kc - 2.9010-2 at 1150 K. 2SO3(g) 2502(g) + O2(g) When 0.33 moles of SO2(g) are added to the equilibrium system at constant temperature: The value of Kc The value of Qc Kc The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. The concentration of O2 will Submit Answer Retry...
Consider the following reaction and its equilibrium constant 0.43 SO2(g) + NO (9) = SO.(g) + NO(g) K = 0.33 A reaction mixture contains 0.49 M SO. 0.14 M NO, 0.12 M SO, and 0.14 M NO. Which of the following statements is TRUE concerning this system? b. ooo The reaction will shift in the direction of reactants. The equilibrium constant will decrease. The reaction will shift in the direction of products. The reaction quotient will decrease. The system is...
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