The Combined Gas Law describes the relationship between temperature, volume, and pressure. The relationship between pressure and volume is P1V1 = P2V2, otherwise known as Boyle’s Gas Law. The relationship between temperature and volume is stated in Charles 's Gas Law, which states V1/T1 = V2/T2. The relationship between temperature and pressure, also known as Gay Lussac 's Gas Law, is P1/T1 = P2/T2. The Combined Gas Law is a combination of Boyle’s, Charles’s, and Gay Lussac 's Gas Laws, resulting in P1V1/T1 = P2V2/T2 (Chemistry: The Physical Setting). The particles in gases move very quickly and freely, constantly colliding into its surroundings and each other. According to the Kinetic Molecular Theory and based on Boyle’s Gas Law, the pressure
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This experiment uses the balanced equation Mg (s) + 2HCl (aq) → H2 (g) + MgCl2 (aq), where the total mass of the reactants equal the total mass of the products, according to the Law of Conservation of Mass. One can determine the number of moles of H2 produced by comparing it to the number of moles of Mg produced. Since the ratio is Mg:H2, then the ratio would be 1:1, therefore determining the number of moles of H2 produced. This shows that using a balanced chemical equation allows one to predict the moles of a gas produced. The volume of a gas relates to the moles of gas particles due to Avogadro’s Law. Avogadro’s Law states that equal volumes of all gasses have the same number of molecules, at the same temperature and pressure. Dalton’s Law of Partial Pressure is relevant to this experiment because the law was used to determine the pressure of H2, using the formula Ptotal = PH2+ PH20 (Experiment 2.3: Molar Volume of a Gas at STP Student Instruction Form). One can determine the pressure of H2 by plugging in the total pressure and the pressure of H2O. The total pressure given was 95.81 kPa, and the room temperature given was 24.9 °C, thus the pressure of H2O was 4 kPa (Table H Vapor Pressure of Four Liquids). By using Dalton’s Law of Partial Pressure, one was able to determine that the pressure of H2 was 91.81
This experiment uses the balanced equation Mg (s) + 2HCl (aq) → H2 (g) + MgCl2 (aq), where the total mass of the reactants equal the total mass of the products, according to the Law of Conservation of Mass. One can determine the number of moles of H2 produced by comparing it to the number of moles of Mg produced. Since the ratio is Mg:H2, then the ratio would be 1:1, therefore determining the number of moles of H2 produced. This shows that using a balanced chemical equation allows one to predict the moles of a gas produced. The volume of a gas relates to the moles of gas particles due to Avogadro’s Law. Avogadro’s Law states that equal volumes of all gasses have the same number of molecules, at the same temperature and pressure. Dalton’s Law of Partial Pressure is relevant to this experiment because the law was used to determine the pressure of H2, using the formula Ptotal = PH2+ PH20 (Experiment 2.3: Molar Volume of a Gas at STP Student Instruction Form). One can determine the pressure of H2 by plugging in the total pressure and the pressure of H2O. The total pressure given was 95.81 kPa, and the room temperature given was 24.9 °C, thus the pressure of H2O was 4 kPa (Table H Vapor Pressure of Four Liquids). By using Dalton’s Law of Partial Pressure, one was able to determine that the pressure of H2 was 91.81