The Exciting Chemistry Challenge on Limiting Reagent and Volume of CO2 Formation
In this exciting chemistry challenge, we are tasked with determining the limiting reagent and the volume of CO2 formed in a reaction involving 11L of Cs2 and 18L of O2 to produce CO2 gas and SO2 gas at STP.
The STP conditions, which refer to the standard temperature and pressure, provide us with the necessary information to make these calculations. At STP, the pressure values are at 1 atmosphere and the temperature is at 0 ° C, making them reference values for gases. Additionally, at these conditions, 1 mole of any gas occupies an approximate volume of 22.4 liters.
By applying a rule of three, we can calculate the amount of moles of CS2 and O2 based on their respective volumes of 11L and 18L. This step is crucial in determining the limiting reagent, which is the reagent that is completely consumed first in the reaction, thus impacting the amount of product formed.
Upon calculating the moles of CS2 and O2 and using the reaction stoichiometry, we find that O2 is the limiting reagent in this reaction scenario. This means that O2 will be completely consumed before CS2, determining the amount of product formed.
Next, we calculate the amount of moles of CO2 produced based on the stoichiometry of the reaction and the limiting reagent. Once the moles of CO2 are determined, we can then calculate the volume of CO2 formed by considering the STP conditions and the amount of moles of CO2 produced.
Therefore, the exciting chemistry challenge concludes with the volume of CO2 formed when 11L Cs2 reacts with 18L O2 to produce CO2 gas and SO2 gas at STP is 6.0 L. This result showcases the fascinating world of chemical reactions and the meticulous calculations involved in understanding and predicting the outcomes of such reactions.