A flask containing pure NO2 is heated to 1000 K, a temperature at which Kp=158 for the decomposi

step 1 Okay, today I'll be going over question number 9 -1, which gives you the decomposition of NO2, i

A flask containing pure NO2 is heated to 1000 K, a...

A flask containing pure $\mathrm{NO}_{2}$ is heated to $1000 \mathrm{K},$ a temperature at which $K_{p}=158$ for the decomposition of $\mathrm{NO}_{2}$ $$ 2 \mathrm{NO}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) $$ The partial pressure of $\mathrm{O}_{2}$ at equilibrium is 0.136 atm. a. Calculate the partial pressures of $\mathrm{NO}$ and $\mathrm{NO}_{2}$. b. Calculate the total pressure in the flask at equilibrium.

A flask containing pure $\mathrm{NO}_{2}$ is heated to $1000 \mathrm{K},$ a temperature at which $K_{p}=158$ for the decomposition of $\mathrm{NO}_{2}$
$$
2 \mathrm{NO}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})
$$
The partial pressure of $\mathrm{O}_{2}$ at equilibrium is 0.136 atm.
a. Calculate the partial pressures of $\mathrm{NO}$ and $\mathrm{NO}_{2}$.
b. Calculate the total pressure in the flask at equilibrium.

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the rates of the forward and reverse reactions become equal, meaning there is no net change in the concentration or partial pressure of the reactants and products over time. This concept is central to predicting the composition of a reaction mixture once equilibrium is established.

Equilibrium Constant (Kp) Expression

The equilibrium constant for gas-phase reactions, denoted as Kp, is defined in terms of the partial pressures of the products and reactants at equilibrium, raised to the power of their stoichiometric coefficients. This expression allows us to relate the pressures of different species in a system at equilibrium and is essential for calculating unknown pressures when at least one equilibrium value is known.

Partial Pressure

Partial pressure is the pressure contributed by a single gas in a mixture of gases. It is proportional to the mole fraction of that gas times the total pressure. Understanding partial pressures is important in analyzing gaseous equilibrium systems because each species' behavior is modeled based on its individual pressure rather than the overall pressure.

Reaction Stoichiometry

Reaction stoichiometry deals with the quantitative relationships between reactants and products in a chemical reaction, as indicated by the balanced chemical equation. It is used in equilibrium problems to relate the change in moles or pressures of different species based on their coefficients, enabling the calculation of unknown quantities in the system.

Algebraic Techniques in Equilibrium Calculations

Algebraic techniques are used to set up equations based on the equilibrium constant expression and the stoichiometric relationships of the reaction. These techniques involve expressing unknown pressures or concentrations in terms of a common variable, using known equilibrium values, and solving the resulting equations to determine the quantities of interest.

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