Experiment 1: Pressure, Temperature, and Velocity Measurement Objective: The objective of this experiment is to determine the pressure and density of laboratory air, calibrate a pressure transducer and scannivalve, then determine the test section speed as a function of fan speed using three methods of velocity measurement. Equipment: Absolute pressure transducer, digital thermometer, pressure transducer (voltmeter), micromanometer, scannivalve, Pitot tube, low-speed wind tunnel. Part 1: Measurement of Atmospheric Pressure and Density 1. Read the barometer and wind-tunnel thermocouple. 2.
Name: ___________________________________ Date: ______________ Practice Test #3 ____ 1. When a precipitation reaction occurs, the ions that do not form the precipitate A) evaporate B) are cations only C) form a second insoluble compound in the solution D) are left dissolved in the solution E) none of these 2. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) ____ 3.
|Resistance |Effort | |Force, as added mass |Arm length |Work |A |B |Total force |Arm length |Work | |to resistance side (g)|(m) |(N × m or J) |Force (N) applied |Pulling force applied |B-A |(m) |(N × m or J) | |converted to (N) | | |to balance the |to the spring scale | | | | | | | |lever with no mass|(n) when mass is added| | | | | | | |on effort side |to effort side | | | | |300 g = |0.70 |2.058 |0.87 |22.74 |21.87 |0.40 |8.748 | |2.94 N | | | | | | |
Reduction Reaction | Reduction Potential | Cu2+ + 2e- Cu(s) | 0.34 V | Al3+ + 3e- Al(s) | -1.66 V | Safety 1) Don’t eat or drink anything in the lab. 2) Always wear eye protection. 3) Wear protective clothing (lab coats, etc.). 4) Don’t play around – treat the lab with respect. Questions Place one small scoop of copper chloride crystals onto a piece of Al foil.
Jose Flores 6th period 1-27-14 LAB REPORT Introduction: A substance can conduct an electrical current if it is made of positively charged and negatively charged particles that are free to move about and is called a conductor. The purpose is to figure out conductivity of substances and to check which one conducts electricity. The hypothesis is that sucrose would be the only one that could not conduct out of the other six solutions. Materials: The materials used in this lab where six solutions , napkins, 2 pairs of gloves, 2 cups (1 cup with distilled water and 1 cup with solid NaCI) and a conductivity meter. The six solutions are sodium chloride, hydrochloric acid, sodium hydroxide, acetic acid, ammonia and sucrose.
Analysis of a Commercial Bleach Lab Guidelines • Name, Exp. Name, Number, Date (we did lab), Partner(s) • Purpose • Compound Names, Formulas, and Molar Masses (5 used – no formula or molar mass for starch) • Reactions (use the four listed on the front page of the lab) • Procedure/Observations • Include initial observations and final observations/odors, masses of KI… • Results (Data Table) • Make a table that has your data of KI masses, and the three volumes (from the three trials) needed to titrate the bleach • Calculations (Data and Calculations Section in lab) 1. Use the equations given on the front page to determine the number of moles of sodium thiosulfate that are equivalent to one mole of sodium hypochlorite. 2. From your three trials, calculate the average volume of Na2S2O3 needed for the titration of 25.00mL of diluted bleach.
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.
The string is tied onto a thin metal bar at A and fixed at B. A vibration generator causes the bar to oscillate at a chosen frequency. Explain how a stationary wave is formed. Then describe the key features of the stationary wave shown in Figure 4. * Waves reflect off the clamp and the rod * Waves travelling in opposite directions superpose * Waves have same wavelength and frequency, similar amplitude * Always cancellation at nodes and constructive superposition at antinodes * Energy is not transferred along string * 4 nodes where there is zero amplitude * 3 antinodes where amplitude is maximum * Wavelength 0.80m * End antinodes in phase and middle and ends in antiphase * Between node and antinode, amplitude of oscillation increases On her next jump the gymnast decides to reach a height above position B.
Observations: Quantitative & Qualitative Data Table Table 1: Solubility Qualitative data: Substances | Time (s) | Soluble or not? (Yes/No) | X | 42 | Yes | Y | 63 | Yes | Z | >180 | No | Table 2: Appearance of the substances while melting Substance X- White rocky powdery dots Qualitative data: Time (s) | Physical appearance of substance X | 10 | White powder dots | 26 | White powder dots | 44 | White powder dots | 55 | White powder dots | 65 | The color of the white powder dots changes to brown powder dots | 82 | Starts to melt a tiny bit | 107 | It stops melting, and there are still white powder left | 125 | Stays as white powder, no melting | 155 | White powder dots, nothing happens | 178 | White powder dots, no melting | 183 | White powder dots, nothing happens | 207 | A few of the tiny white dots starts to melt again | 230 | The white powder stops finally stay still | Table 3: Appearance of the substances while melting Substance Y- White crystal dots Qualitative data: Time (s) | Physical appearance of substance Y | 3 | White crystal dots | 20 | White crystal dots, no change | 40 | White crystal dots, no physical change
In each part of the experiment, you will be observing a different property of electrolytes. Keep in mind that you will be encountering three types of compounds and aqueous solutions: Ionic Compounds These are usually strong electrolytes and can be expected to 100% dissociate in aqueous solution. Example: NaNO 3 (s) → Na+(aq) + NO 3 –(aq) Molecular Compounds These are usually non-electrolytes. They do not dissociate to form ions. Resulting solutions do not conduct electricity.