any grammar error or anything to fix to make clearer
The scope of this experiment delves thoroughly in relationship between these acid and metal. The sulfuric acid is a highly corrosive mineral acid that is commonly used in industrial processes while magnesium a chemical element, and is known as lightest structure metal.
Collision theory plays in a role between magnesium and sulfuric acid as magnesium atom collides with sulfuric acid molecules as overcoming the activation energy barrier forming magnesium ions and hydrogen gas (OpenStax, 2019). The reaction between metal and acid produces salt and hydrogen which links to product in this scenario magnesium sulphate and hydrogen gas (BBC, 2023).
Mg (s)+ H2SO4 (aq) → MgSO4 (aq) + H2 (g)
The rate of reaction refers to the speed at which the concentration of reactants decreases and is concerted into products and there are five key factors that influence the rate of chemical reaction such as concentration, pressure, surface area, temperature, and catalysts (LibreTexts, 2013).
Based on hypothesis as an increasing concentration of sulfuric acid would increase rate of reaction.
The purpose of this student experiment is to investigate whether the concentration of Sulfuric acid (0.1M, 0.5M, 0.75M, 1M, and1.5M) affects the volume of hydrogen gas produced when reacting with 0.05g of magnesium ribbon, aiming to determine if there is a significant variation in the outcomes. This research question holds significance for industrial processes, as it not only validates a perplexing assertion but also aids in hazard management by raising awareness of the potential for rapid reactions.
The scope of this experiment thoroughly examines the relationship between sulfuric acid and metal, specifically magnesium. Sulfuric acid is a highly corrosive mineral acid commonly used in industrial processes, while magnesium is a chemical element known for being the lightest structural metal.
The collision theory is relevant to the interaction between magnesium and sulfuric acid. When a magnesium atom collides with sulfuric acid molecules, it overcomes the activation energy barrier and forms magnesium ions and hydrogen gas (OpenStax, 2019). This reaction between the metal and acid produces salt and hydrogen, resulting in magnesium sulfate and hydrogen gas in this particular scenario (BBC, 2023).
Mg (s)+ H2SO4 (aq) → MgSO4 (aq) + H2 (g)
The rate of reaction refers to the speed at which the concentration of reactants decreases and is converted into products. There are five key factors that influence the rate of a chemical reaction: concentration, pressure, surface area, temperature, and catalysts (LibreTexts, 2013).
Based on our hypothesis, an increasing concentration of sulfuric acid would result in an increased rate of reaction.
The purpose of this student experiment is to investigate whether the concentration of sulfuric acid (0.1M, 0.5M, 0.75M, 1M, and 1.5M) affects the volume of hydrogen gas produced when reacting with 0.05g of magnesium ribbon. The aim is to determine if there is a significant variation in the outcomes. This research question holds significance for industrial processes, as it not only validates a perplexing assertion but also aids in hazard management by raising awareness of the potential for rapid reactions.
The scope of this experiment thoroughly investigates the relationship between sulfuric acid and metal. Sulfuric acid is a highly corrosive mineral acid commonly used in industrial processes, while magnesium is a chemical element known as the lightest structural metal.
The collision theory plays a role in the reaction between magnesium and sulfuric acid. When a magnesium atom collides with sulfuric acid molecules, it overcomes the activation energy barrier, forming magnesium ions and hydrogen gas (OpenStax, 2019). This reaction between the metal and acid produces salt and hydrogen. In this scenario, the products are magnesium sulfate and hydrogen gas (BBC, 2023).
Mg (s) + H2SO4 (aq) → MgSO4 (aq) + H2 (g)
The rate of reaction refers to how quickly the concentration of reactants decreases and is converted into products. There are five key factors that influence the rate of a chemical reaction: concentration, pressure, surface area, temperature, and catalysts (LibreTexts, 2013).
Based on the hypothesis, an increasing concentration of sulfuric acid would increase the rate of the reaction.
The purpose of this student experiment is to investigate whether the concentration of sulfuric acid (0.1M, 0.5M, 0.75M, 1M, and 1.5M) affects the volume of hydrogen gas produced when reacting with 0.05g of magnesium ribbon. The aim is to determine if there is a significant variation in the outcomes. This research question holds significance for industrial processes, as it not only validates a perplexing assertion but also aids in hazard management by raising awareness of the potential for rapid reactions.