Purpose, Context, Relevance Chemical reactions are vital in the generation of gases in experimental and theoretical chemistry; therefore, when trying to generate a gas in the laboratory, other properties such as stoichiometry, gas laws, and reaction kinetics also come into action, as in this experiment. A plastic bag of 1.5 liters is to be inflated using a specific amount of each reactant. 5.15 g of sodium bicarbonate NaHCO3 is combined with 51.1 ml of acetic acid CH3COOH. This process demonstrates the conversion of reactants to gaseous products and illustrates the quantitative relationships found in chemical equations. It is also a relevant application to real-life phenomena, including the operation of airbags in cars and the behavior of gases in every industry.
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The specific amounts of reactants have been meticulously calculated using a technique called stoichiometry, designed to ensure a near-complete reaction and an acceptable amount of carbon dioxide gas production. The balanced chemical equation is NaHCO3(s) + CH3COOH CH3COONa(aq) + H2O(l) + CO2(g). In this experiment, the ideal gas law is utilized where V is the volume in cubic meters, n is the number of moles of gas, P is pressure in units of Pascals (Pa), R is the ideal gas constant (8.314 J/molK), and T is the temperature in Kelvin. At a normal room temperature (25 °C) and pressure, the ideal gas law will be used to double-check whether the CO2 produced is enough to inflate the plastic bag, which was previously measured with water to determine the 1.5 liters. Specific Aim The experimental process involves calculating the moles of sodium bicarbonate and acetic acid to ensure a comprehensive reaction, followed by determining the theoretical yield of carbon dioxide
The specific amounts of reactants have been meticulously calculated using a technique called stoichiometry, designed to ensure a near-complete reaction and an acceptable amount of carbon dioxide gas production. The balanced chemical equation is NaHCO3(s) + CH3COOH CH3COONa(aq) + H2O(l) + CO2(g). In this experiment, the ideal gas law is utilized where V is the volume in cubic meters, n is the number of moles of gas, P is pressure in units of Pascals (Pa), R is the ideal gas constant (8.314 J/molK), and T is the temperature in Kelvin. At a normal room temperature (25 °C) and pressure, the ideal gas law will be used to double-check whether the CO2 produced is enough to inflate the plastic bag, which was previously measured with water to determine the 1.5 liters. Specific Aim The experimental process involves calculating the moles of sodium bicarbonate and acetic acid to ensure a comprehensive reaction, followed by determining the theoretical yield of carbon dioxide