Hydrogen combines with oxygen to make water which is essential to life Hydrogen gas (H2) is colorless, odorless and the most abundant element in the universe, it is less dense than air or water. The method that is going to be used to collect the H2 gas is water displacement measured in Ml. moles of H2 will be found by converting Ml to moles by dividing the number of Ml of H2O displaced by the atomic mas of magnesium (24.3 g). units that will be used for PV=nRT: p- Kpa, V- Liters, n- Moles, R- 8.31, T- kelvins. The final step will be to find the theoretical experimental yield and percent yield.
0.4J/s b. 0.4W c. 44kJ d. 444W e. None of the above 17. A calorimeter is: a. An instrument used to measure atmospheric pressure b. An isolated container with a cylinder containing a known amount of water and a thermometer to measure the temperature of water c. A device used to measure calories d. An instrument used to plot the sinusoidal function of a wave of light e. Used to measure the change in energy during centripetal motion over a period of time 18.
What is the weight percent of each element in ammonium sulfate? C. Empirical and Molecular Formulas 1. Empirical Formula - shows the number of atoms in the smallest possible ratio a. may be calculated from percent composition data b. may or may not show the true number of atoms of each kind in the molecule 2. Molecular Formula - shows the true
An anhydrous salt is a salt without the presence of water or any moisture. In this experiment the anhydrous salt was separated as well as the water from the hydrate. The mass of the anhydrous salt was one of the parts needed to be calculated in order to find the complete formula of the hydrate. The law of conservation of mass states that matter in a compound can be altered, separated, and pure substance can be destroyed, but the mass always remains the same. In this experiment, the hydrate was separated into water and the anhydrous salt.
The average density: =0.82+ 0.77+ 0.77 = 2.36 = 2.36/3= 0.79 g/ml Note that the burette was the most accurate in determining accuracy of measured amounts. The average density for all three of these methods is: = 0.76+ 0.73+ 0.79 = 2.28 =2.28/3= 0.76 g/ml Graph Procedure B. Determination of the boiling point of an unknown liquid Note that the atmospheric pressure in the lab room is 100 Kpa. (Xidos, 2013-2014) Required: An assembled boiling point apparatus. Fifteen drops of the unknown liquid was then placed into an empty
Write a balance equation for the above reaction B. Which of the 2 reactants is the limiting reagent? C. Calculate the mass of aluminium oxide formed D. How much excess reagent is left at the end of the reaction? E. If the actual yield of ammonium oxide formed was 980g what is its yield % ANS a. 2Al + Fe2O3 ( Al2O3 + 2Fe (26.98) ( 159.7) (101.96) 124 601 80 b. Al c. 234.3 d. 234 e. 34.1% 1c.
This reaction can be summed up using the following formula: 5Fe2++8H++MnO4- →5Fe3++Mn2++4H2O After standardization, the potassium permanganate solution is then titrated with 3 different magnesium oxalate solutions. To find the concentration of the C2O42- the balanced net ionic redox reaction formula is used: 5C2O42-+16H++2MnO4- →10CO2+2Mn2++8H2O It is important to note the addition of sulfuric acid (9M H2SO4) in performing this experiment because of the following reasons: 1) Sulfuric acid keeps the iron (II) from air oxidizing into iron (III) 2) Sulfuric acid keeps the iron (II) from hydrolyzing into Fe(OH)2 3) Sulfuric
At 50C our results indicated a solubility of 89 g/100mL of H2O which was close to the known solubility of 80 g/100mL. Introduction: When a salt, such as potassium nitrate or sodium chloride, is placed in water a dissolving reaction will occur. At first, the positive and negative ions of the salt compound are only attracted to each other. In order for the salt to dissolve, these bonds must be broken so that the ions disassociate from each other. In the water molecules, hydrogen is slightly positive and oxygen slightly negative so they are attracted to ions of the opposite charge, known as dipole attraction.
Purpose: To investigate the physical and chemical properties of pure chemical substances. Observations and Experimental Data: Data Table 1: Solubility or Reaction Substance Name Color Odor Effect of Heat Cold H2O Hot H2O Litmus Test Dilute HCl Dilute NaOH Mg Silver odorless nothing bubbles bubbles No color change Bubble,fizz Slightly frothy cloudy No apparent change Cu Copper Odorless Turns darker black No apparent change No apparent change Lighter blue Holes in copper ball bubbles Dark spots on copper Zn Silver Odorless Liquid Solid Solid Lighter blue Bubbles fizzes No apparent change MgO white odorless Dark grey Cloudy Cloudy Lighter blue Fizzed bubbled Cloudy no bubbles CuCO3 green odorless pops Cloudy green h2o dissolved Turns dark green pops Blue-from pink Fizzed dissolved Turns blue Cu(NO3)2 blue odorless Melts boils Light green liquid Dissolved boils Blue-from pink Dissolved green liquid Blue bubbles NaCl white odorless crackesl Grain in h2o no bubbles Stays granular Lighter blue No apparent reaction bubbles Questions: A. Did you observe any chemical changes in this experiment? Yes. B.