Given the evidence‚ it can be determined that a reaction will occur when reactants have a kinetic energy greater than the activation energy‚ this is a theory of collision theory. For example‚ in the first experiment‚ the test tube filled with 10 mL of 3% hydrogen peroxide and had scoop of manganese dioxide‚ had a greater reaction than the other test tube. Which simply contained 10 mL of 3% hydrogen peroxide. The factor that affected the reaction rate was that the manganese was seen as a catalyst
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useful solids (Bauer 45). It was the lab group’s goal to design procedures for creating these useful solids out of the concentrated byproduct solutions. The concentrated byproduct solutions provided by the company were: 0.1 M of NaOH‚ H2SO4‚ BaCl‚ HCl‚ AgNO3‚ and Zn(NO3)2. With the byproduct solutions given‚ four different useful solids could be created. These solids are: Na2SO4‚ BaSO4‚ AgCl‚ and Zn(OH)2. Potential commercial uses for these particular solids are discussed in the “discussion” section
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Materials Available 3 x 250 mL beakers magnesium ribbon (1 cm) 3 x test tubes magnesium powder test tube rack mossy zinc 10 mL graduated cylinder copper turnings 3 x Alka Seltzer® tablets copper(II) sulfate 0.1 M hydrochloric acid‚ HCl hot bath 1.0 M hydrochloric acid‚ HCl ice bath 6.0 M hydrochloric acid‚ HCl steel wool pieces of zinc (1 cm x 1 cm) thermometer *additional materials may be made available upon request* Part 1: Affect of Temperature
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2.MATERIALS and METHODS 2.1. Nature of Reactants 2.1.1 We placed 3mL of 3 M HCl into each of 3 seperate test tubes. Next we added mossy zinc to the first test tubes‚ Sn granules to the second and Cu filings to the third and compared the rates of evolution of hydrogen gas in each test tube. 2.1.2. We mixed 3mL of 0.02 M KMnO4 and 2mL of 3 M H2SO4 in a test tube and stirred using a glass rod. Next‚ we divided the solution into two. We added 2mL of 0.03 M Na2C2O4 solution to the first half and
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Chemical Reactions Lab Introduction Four different types of chemical reactions were observed in this lab. Synthesis reactions occur when two different elements or compounds form a more complex compound as shown by equation (1). Single replacement occurs when one element replaces another to form a new compound as shown in equation (2). Double replacement occurs when two different atoms in different compounds trade places with one another to form two new compounds as shown in equation (3).Combustion
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(Cu) again. The final regeneration of copper (Cu) was then weighed to present a percent recovery of the copper (Cu) as it cycled through its series of reactions. To present an effective experiment the following equipment: copper wire‚ hot plate‚ 3M HCl(aq)‚ 6M HNO3(aq)‚ 6M NaOH (aq)‚ 2 M H2SO4‚ 100ml beaker‚ graduated cylinder‚ filter flask‚ Buchner funnel/vacuum flask ‚ scale‚ and pipets alongside the fume hood--for the omission of NO2-- was used to conduct the copper cycle experiment. First‚ the
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Lab #5 Chemical Reactions & Balancing Equations Objectives Observe and classify several chemical and physical changes. Give evidence for the occurrence of a chemical reaction. Write a balanced equation for a chemical reaction. Identify a reaction as a combination‚ decomposition‚ replacement‚ or combustion reaction. Background Physical properties can be observed without changing the chemical composition of the substance. Common physical properties that can be measured without changing the chemical
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mixing zinc and acid/let go of cotton ALLOW: cut the string NOT: heat (the acid) NOT: pull the string (b) (i) (ii) (iii) [2] [1] correct plotting including 0-0 point ( - 1 per omission or error) best curve drawn and to go through origin no more gas produced/reaction finished; all zinc reacted/used up [2] graph drawn with faster initial rate and starting at 0-0; ALLOW: straight line as initial rate ends up at 55 cm3 (c) [2] (d) (i) (ii) (iii) 2 (HCl) zinc
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Metallic zinc is the reducing agent B. Metallic zinc is reduced C. Copper ion is oxidized D. Sulfate ion in the reducing agent 10. In which set are the substances arranged in order of decreasing solubility in water? A. Al(OH)2 > Mg(OH)2 > NaOH B. BaSO4 > CaSO4 > MgSO4 C. CaCO3 > NaHCO3 >Na2CO3 D. AgCl > AgBr > AgI 11. What Volume of 10M HCl solution is required to prepare exactly 500 mL of a 0.60M HCl solution? A. 10mL B. 14mL C. 30mL D. 40mL 12. What
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and Testing for Hydrogen Gas Felicity Tyler Aim: To produce and test for hydrogen gas. Materials: * rubber stopper * dilute hydrochloric acid (HCI) * zinc pieces (Zn) * test-tube rack * matches * dilute sulphuric acid (H2SO4) * 2 cm strips of magnesium ribbon (Mg) * Iron pieces (Fe) * Test-tube Method 1. Test the different metals with the acids by separately combining each
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