Gases carbon monoxide and nitrogen monoxide

Questions: Produce Word Document that covers the following topics: 1. Consider the reaction between gases carbon monoxide and nitrogen monoxide: 2CO + 2NO 2CO2 + N2 Using Boltzmann distribution and collision theory explain what would happen to the rate of a reaction if temperature and pressure were independently increased. Also explain what would happen is a suitable catalyst was used. 2. Have complete Foundation Biology enzymes and rates. 3. Consider the reversible reaction between nitrogen and hydrogen gases to produce ammonia gas the Haber Process N2 + 3H2 2NH3 - The forward reaction is exothermic Explain what is meant by Le Chateliers Principle and use it to explain what happens to the position of the equilibrium if: The concentration of nitrogen is increased Ammonia is removed as soon as it is produced Overall pressure of the system is increased Overall temperature of the system is increased 4. Explain and give examples of what is meant by the following: Acid Base Alkali pH Strong Acid / Base Weak Acid / Base Acid / Base Neutralisation 5. Consider the weak acid, Ethanoic Acid in a buffer solution containing Sodium Ethanoate CH3COOH CH3COO- + H+ CH3COONa CH3COO- + Na+ Explain what would happen to the pH if small volumes of hydrochloric acid or sodium hydroxide were added. 6.Experimentally determine by titration the concentration of sample of a sample of hydrochloric Answers: 1. Consider the reaction between gases carbon monoxide and nitrogen monoxide: 2CO + 2NO 2CO2 + N2 Using Boltzmann distribution and collision theory explain what would happen to the rate of a reaction if temperature and pressure were independently increased. Also explain what would happen is a suitable catalyst was used If the temperature increases independently, the rate of reaction will increase as the will have more energy and the particles will be colliding more. The rate of reaction will increases if they pressure is increased (Barnett and Harrison, 2013). If the pressure is increased, the reactant particles become more crowded, there is greater chance of collision, and the rate of reaction will increase. A catalyst is a substance when added to a reaction it will increase the rate of reaction. If platinum is added to the reaction, the reaction will be very fact. 2. Have complete Foundation Biology enzymes and rates, assessment criteria The chemical principles to analyse a typical analytical technique for the enzymes are the Investigate catalyse activity in plant extracts. Investigate of an enzyme-controlled reaction. Investigate to measure the effect of temperature on lipase activity (Oriakhi, 2009). 3.Consider the reversible reaction between nitrogen and hydrogen gases to produce ammonia gas the Haber Process N2 + 3H22NH3 - The forward reaction is exothermic Explain what is meant by Le Chateliers Principle and use it to explain what happens to the position of the equilibrium if: The concentration of nitrogen is increased Ammonia is removed as soon as it is produced Overall pressure of the system is increased Overall temperature of the system is increased Le Chateliers principle states that if a equilibrium is disturbed by changing the conditions, the position of the equilibrium shifts to counteract the change to re-establish an equilibrium. If the concentration of the nitrogen is increase then: The equilibrium will shift to the right, as the nitrogen will shift the reaction to the right (Haber, Kiwi and Kiwi, 2013). More ammonia will produced. Increase in the heat release. If ammonia is removed as soon as it is produced: The chemical concentration of the right will decrease. If Overall pressure of the system is increased: By increasing the pressure, the reaction will favour the forward reaction. The speed of reaction will increase. More number of Ammonia will produced (Haber, Bars and Schmitz, 2011). If Overall temperature of the system is increased More number of nitrogen and hydrogen will produced. 4. Explain and give examples of what is meant by the following: Acid Base Alkali pH Strong Acid / Base Weak Acid / Base Acid / Base Neutralisation Acid: Acids are the compounds that can donate hydronium ions when dissolved in water. Example: HCL Base: Bases are the substances, which produced hydroxide ions when dissolved in water. Example: Baking soda (Kauzmann, 2013). Alkali: Alkali are the substances which produces hydronium ions in water. Example: sodium hydroxide pH: it is a measure of the hydrogen ion concentration. Solution Strong Acid / Base: acids and bases, which are totally ionized when dissolved in water, are called strong acid and strong bases. Example: HCL is a strong acid. Weak Acid / Base: acids and bases, which are not completely ionized in water, are called weak acid and weak bases. Example: acetic acid is a weak acid. Acid / Base Neutralisation: When a strong acid and a strong base solution are mixed then neutralization reaction occurs. The product produced does not have the characteristics of both acids and the bases. 5. Consider the weak acid, Ethanoic Acid in a buffer solution containing Sodium Ethanoate CH3COOH CH3COO-+ H+ CH3COONa CH3COO-+ Na+ Explain what would happen to the pH if small volumes of hydrochloric acid or sodium hydroxide were added By the addition of hydrochloric acid, the pH remains the same. 6. Experimentally determine by titration the concentration of sample of a sample of hydrochloric acid using a known concentration of sodium carbonate A solution of hydrochloric acid is prepared and standardized against the pure sodium carbonate, and the percentage of the carbonate is determined in the sample (Moore and Langley, 2007). The percentage of Na2Co3 are calculated from the sample from two ways Molarity of the HCL: It is calculated by the following formula MHCl = moles HCl /liter = moles Na2CO3 x 2 (ml HCl/1000) = (wt of Na2CO3) x 2 / (mol wt Na2CO3) (ml HCl/1000) Percentage of the Na2CO3 in sample are calculated by the following %Na2CO3 = wt of Na2CO3 in sample / g sample x 100 References Barnett, C. and Harrison, M. (2013).Plasmas. Burlington: Elsevier Science. Haber, J., Kiwi, L. and Kiwi, L. (2013).Heat Management for Process Intensification of Fast Exothermic Reactions in Microstructured Reactors. Lausanne: EPFL. Haber, R., Bars, R. and Schmitz, U. (2011).Predictive control in process engineering. Weinheim: Wiley-VCH. Kauzmann, W. (2013).Kinetic Theory of Gases. Newburyport: Dover Publications. Moore, J. and Langley, R. (2007).Chemistry for the utterly confused. New York: McGraw-Hill. Oriakhi, C. (2009).Chemistry in quantitative language. Oxford: Oxford University Press.