The effect of acid rain on building materials Essay Example for Free

The effect of astringent rain on building materials EssayDue to dissolved carbon dioxide rainwater is naturally acidic in the wee of the weak carbonic acid. However burn outes such as sulphur dioxide and nitrogen oxides cause acid rain, which is answerable for the corrosion of buildings and damage to the wildlife. The burning of fossil fuels releases these gases into the atmosphere when the small quantities of sulphur react with the oxygen in the air, forming sulphur dioxide. The aim of this investigation is to investigate the way in which one factor alters the rate of wearing away of building materials such as stonework and metals. To conduct this try I can use marble chips (calcium carbonate) or magnesium ribbon and in place of sulphuric acid dilute hydrochloric acid go out be used. This is because sulphuric acid produces an insoluble salt which prevents any further reaction with the acid. The two possible equations for the experiment are 1) Mg + 2HCl MgCl + H 2) CaCO? + 2HCl CaCl + CO + H O I have decided to conduct my experiment using magnesium ribbon and so equation 1 will be used. here is a list of the factors which I could investigate book of acid Concentration of acid. Temperature of reaction Mass/ length of magnesium ribbon Particle size (no. of unclothes of magnesium) The factor which I have decided to investigate is the account book of hydrochloric acid. The range of tidy sums I have opted to use are 10cmi , 20cmi , 30cmi , 40cmi and 50cmi. The concentration of acid will remain at 2M throughout the investigation and the investigation will be conducted at room temperature. Also 1 strip of magnesium ribbon of mass 0. 05g will be used throughout the investigation.For each volume of acid used I will time how long it takes for 50cmiof hydrogen gas to be produced and collected in a gas syringe. Apparatus Conical Flask (with bung) 100cmi gas syringe Scales Measuring cylinder stop watch Hypothesis I believe that as the volume of acid i ncreases so will the rate of gas produced. This is because there will be much acid molecules and so there will be more chance of collisions between the magnesium and hydrochloric acid, thus a higher rate of reaction. I believe that the volume of acid will be directly proportional to the rate of reaction and so the following will be trueTherefore, if the volume of acid is doubled then the rate of gas produced should double. Diagram manner First of all the gas syringe was connected to the conical flask. 0. 05g of magnesium ribbon was weighed using the scales and displace inside the conical flask. The first volume of 2M hydrochloric acid, 10cmi , was measured out using a measuring cylinder and then added to the flask. Simultaneously the stop watch was started and the bung was placed on the conical flask. When 50cmi hydrogen had been collected the stopwatch was stopped.This was repeated 3 times with each of the volumes of hydrochloric acid, 10, 20, 30, 40 and 50cmi. For each volume an average time was careful and then using that time the rate of reaction was calculated with the following equation Rate (cmi /s) = Volume of gas produced (cmi ) Time (s) Results Time Taken (s) Volume of HCl (cmi ) see 1 Reading 2 Reading 3 Average Reading Rate of Reaction (cmi /s).