4) When naming an ionic compound, which ion is given first? The metal ion is named first 5) Give explanations for the following: a. Argon will not react with any other element It already has a complete number of eight, a full number in its valance shell so it cannot react with itself or another element b. The reaction between sodium chloride gives out a lot of heat and light. The chemical energy of the product is less then the chemical energy of the reactants. This energy is indestructible and is converted to light and heat.
Solids? Yes (Graphite) 2. Liquids? No 3. Aqueous solutions (when the covalent compounds are dissolved in water)?
We can use the same principal we used for the first experiment, Manganese dioxide is not a protein, not an enzyme, it is a catalyst. Due to this, no products are formed, and just as we anticipated, the reaction rate was given a 0. 3. The 3rd experiment is a mixture of 2 mL H2O2 and liver. In this situation, both the substrate (H2O2) and the enzyme (catalase) are present, and
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.
However majority of the solid Iodine was left at the bottom of the test tube; which leads to the conclusion that it’s not reactive on water. 2. Solid iodine in 1 mL of potassium iodide is slightly more soluble. The liquid in the small test tube turned a dark brown color. 3.
| | 1. (Points: 5.4) | | Solids have a __________ shape and are not appreciably __________. a. definite, compressible b. definite, incompressible c. indefinite, compressible d. indefinite, incompressible e. sharp, convertible | | Save Answer | | 2. (Points: 5.4) | | In the following list, only __________ is not an example of a chemical reaction. a. dissolution of a penny in nitric acid b. the condensation of water vapor c. a burning candle d. the formation of polyethylene from ethylene e. the explosive reaction of hydrogen with oxygen, which produces water, | | Save Answer | | 3.
Dalton’s law of partial pressures states that the total pressure of a mixture of gases is the sum of their partial pressures. 2. How does NO(g) act as a catalyst in the production of ozone at ground level? Show the relevant reactions. NO(g) + ½ O2(g) → NO2(g) NO2(g) + hν → NO(g) + O(g) O(g) + O2(g) → O3(g) Since NO(g) is destroyed in the first step but regenerated in the second step, it is acting as a catalyst.
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.
Observations Data Table: Qualitative Anion Tests | Name | Test Tube 1w/HCl | Test Tube 2 w/AgNO3 | w/HNO | Test Tube 3Confirmation | Bromide | NR | Brownish/gold | Not dissolved | Not dissolved | Carbonate | Gas | White | Not dissolved | Dissolved with NH4OH | Chloride | NR | Milky yellow | Not dissolved | Purplish color | Iodine | NR | Yellowish | Dissolved | Yellowish | Phosphate | NR | NR | NR | Not dissolve | Sulfate | NR | Brownish milky | Not dissolved | Gas/ no result with silver nitrate | Sulfide | GAS AND ODOR | NR | No dissolve | Not dissolve/odor rotton egg. Paper turned slightly browninsh around the edges edges | Unknown | | | | | 3 Questions Classify your ions according to the following three groups. Several of the cations belong to more than one group. Group 1: Anions that WILL NOT PRECIPITATE in the presence of silver nitrate. Sulfate Group 2: Anions that WILL PRECIPITATE in the presence of silver nitrate and the resulting precipitates WILL DISSOLVE upon acidification with nitric acid.
Moles and empirical formulae 1 Calculate the molar mass of the following: (Relative atomic masses: H = 1; N = 14; O = 16; Na = 23; S = 32; Cl = 35.5; K =39.) (a) nitric acid, HNO3 (b) sodium sulfate, Na2SO4 (c) ammonia, NH3 (d) potassium chloride, KCl (e) chlorine, Cl2 2 John says that there is no change in mass during a chemical reaction. Anna disagrees. She says that when calcium carbonate reacts with hydrochloric acid to form carbon dioxide, calcium chloride and water, the mass of the reaction vessel and contents decreases. Who is right, John or Anna?