On réalise la réaction dont l'équation stœchiométrique s'écrit : CaCO3( s)+2 H^+(aq)=Ca^2+(aq)+C

On réalise la réaction dont l'équation stœchiométrique...

On réalise la réaction dont l'équation stœchiométrique s'écrit : $$ \mathrm{CaCO}_3(\mathrm{~s})+2 \mathrm{H}^{+}(\mathrm{aq})=\mathrm{Ca}^{2+}(\mathrm{aq})+\mathrm{CO}_2(\mathrm{~g}) $$ avec $15 \mathrm{~g}$ de carbonate de calcium et $150 \mathrm{~mL}$ d'une solution d'acide chlorhydrique à $2 \mathrm{~mol} . \mathrm{L}^{-1}$. On utilise pour cela un réacteur dont le volume à vide est $1,75 \mathrm{~L}$ initialement plein d'air à la pression atmosphérique du moment, 980 millibars. Ce réacteur est équipé d'une soupape réglée pour s'ouvrir si la pression intérieure dépasse de 2 bars la pression extérieure. La température est maintenue égale à $22^{\circ} \mathrm{C}$. Décrivez ce qui va se passer, avec autant de précision que possible, qualitativement et quantitativement.

On réalise la réaction dont l'équation stœchiométrique s'écrit :
$$
\mathrm{CaCO}_3(\mathrm{~s})+2 \mathrm{H}^{+}(\mathrm{aq})=\mathrm{Ca}^{2+}(\mathrm{aq})+\mathrm{CO}_2(\mathrm{~g})
$$
avec $15 \mathrm{~g}$ de carbonate de calcium et $150 \mathrm{~mL}$ d'une solution d'acide chlorhydrique à $2 \mathrm{~mol} . \mathrm{L}^{-1}$. On utilise pour cela un réacteur dont le volume à vide est $1,75 \mathrm{~L}$ initialement plein d'air à la pression atmosphérique du moment, 980 millibars. Ce réacteur est équipé d'une soupape réglée pour s'ouvrir si la pression intérieure dépasse de 2 bars la pression extérieure. La température est maintenue égale à $22^{\circ} \mathrm{C}$.
Décrivez ce qui va se passer, avec autant de précision que possible, qualitativement et quantitativement.

Key Concepts

Pressure Safety Mechanisms

In chemical reactors, safety mechanisms such as pressure relief valves are essential to prevent dangerous over-pressurization. These devices are calibrated to open when pressure exceeds a preset threshold, allowing excess gas to escape safely. Understanding these safety features is crucial in industrial and laboratory settings to protect equipment and ensure operator safety.

Pressure Evolution in a Closed System

When a reaction occurs in a closed container, especially one that produces gas, the pressure inside the vessel can increase significantly. Understanding how the pressure evolves involves applying gas law principles and considering the initial conditions within the reactor. This concept is key for anticipating whether pressure might reach levels that require intervention, particularly under constant temperature conditions.

Ideal Gas Law Application

The ideal gas law (PV = nRT) is a fundamental equation used to relate pressure, volume, temperature, and the number of moles of a gas. It is crucial in reaction scenarios where gases are produced and collected, as it allows one to calculate and predict changes in pressure and volume within a confined space, assuming the gas behaves ideally.

Limiting Reagent Determination

In any reaction where reactants are not present in the exact stoichiometric proportions, one reactant will be consumed first, limiting the overall extent of the reaction. Determining the limiting reagent is crucial because it dictates the maximum amount of product that can be formed. This involves comparing the mole ratio of the reactants used to that required by the balanced equation.

Reaction Stoichiometry

This concept involves understanding the quantitative relationships between reactants and products in a chemical reaction. It requires balancing the reaction equation and using mole ratios to predict the amount of product formed when given specific amounts of reactants. Stoichiometry is essential for determining the proportional consumption of reactants and formation of products, which is a fundamental component of chemical calculations.

Gas Evolution in Chemical Reactions

Many reactions produce gases as products, and understanding gas formation is important both from a quantitative and qualitative standpoint. Gas evolution can influence reaction dynamics, as the formation, collection, and measurement of gas volumes under given conditions provide important insights into the progression and completeness of the reaction.

Transcript

00:01 In this question, we're going to be looking at the decomposition of calcium carbonate through a reversible reaction to produce calcium oxide plus co2.

00:10 So looking at this, what we want to do here is to have an expression.

00:15 We know that kp is equal to kc multiplied by rt raised to the power of delta n.

00:22 Now looking at the information that we've been given right here, we also know that let's just have the delta n.

00:30 Solid this is a solid and this is a gus so looking at the gasea smalls we've got zero and here in the products we've got one so delta n it is equal to one minus zero which is equal to one so we've got 1 .04 which is equal to kc multiplied by 0 .08 to 1 multiplied by the temperature in kelvin which is 117 3 .15 all of this raised to the power of 1 .1 and this gives us a casein that is equal to 0 .0108.

01:07 And this is equal to the concentration of calcium oxide multiplied by the concentration of co2 divided by the concentration of calcium carbonate.

01:21 Now looking at the information that we've been given, these are going to be in solution.

01:26 So looking at this, we have the concentration.

01:31 Of calcium or rather of co2 this is equal to 1 and this is equal to we usually don't include these in the equilibrium expression since they are solids so we are saying 0 .018 it is equal to the concentration of co2 now that we have this this is a concentration in moles per liter so what this means is looking at this we would want to determine the mass.

02:06 Mass is equal to number of moles multiplied by the molar mass...

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