Consider the following chemical equation: N2(g) + 3 H2(g) = 2 NH3(g)The following equilibrium concentrations were measured at two different temperatures.temperature (K)[N₂] [H₂]5001.25 M2.00 M6003.00 M1.00 M3.00 MDetermine by calculation. If the reaction is endothermic or exothermic, and write the chemical equation including theenergy term.[NH3]30.0 M

Using integrated form of van't Hoff equation, enthalpy change of reaction can be calculated.

Consider the following chemical equation: N2 (g) + 3 H2(g) = 2 NH3(g) The following equilibrium concentrations were measured at two different temperatures. [N₂] [H₂] 1.25 M temperature (K) 500 2.00 M 600 3.00 M 1.00 M 3.00 M Determine by calculation. If the reaction is endothermic or exothermic, and write the chemical equation including the energy term. [NH3] 30.0 M

Consider the following chemical equation: N2 (g) + 3 H2(g) = 2 NH3(g) The following equilibrium concentrations were measured at two different temperatures. [N₂] [H₂] 1.25 M temperature (K) 500 2.00 M 600 3.00 M 1.00 M 3.00 M Determine by calculation. If the reaction is endothermic or exothermic, and write the chemical equation including the energy term. [NH3] 30.0 M

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ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

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When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200. °C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. Write a balanced chemical equation for the equilibrium reaction. Use bond enthalpies from Table 6.2 ( Sec. 6-6b) to estimate the enthalpy change for the reaction. Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? In which direction will the equilibrium shift as the temperature increases above 200. °C? Explain. Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? Why is the equilibrium not established at room temperature?
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
Indicate whether each statement below is true or false. If a statement is false, rewrite it to produce a closely related statement that is true. For a given reaction, the magnitude of the equilibrium constant is independent of temperature. If there is an increase in entropy and a decrease in enthalpy when reactants in their standard states are converted to products in their standard states, the equilibrium constant for the reaction must be negative. The equilibrium constant for the reverse of a reaction is the reciprocal of the equilibrium constant for the reaction itself. For the reaction H2O2(ℓ) ⇌ H2O(ℓ) + O2(g) the equilibrium constant is one half the magnitude of the equilibrium constant for the reaction 2H2O2(ℓ) ⇌ 2H2O(ℓ) + O2(g)
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
In Section 17.3 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term “closed system,” and why is it necessary for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
. Consider the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the following changes affect the number of moles of each component of the system after equilibrium is re-established by completing the table. Complete the table with the terms increase, decrease, or no change. N2 H2 NH3 Add N2(g) Remove H2(g) Add NH3(g) Add Ne(g) (constant V) Increase the temperature Decrease the volume (constant T) Add a catalyst
Use thermochemical data (Appendix C) to decide whether the equilibrium constant for the following reaction will increase or decrease with temperature. 2NO2(g)+7H2(g)2NH3(g)+4H2O(g)
Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.

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