Calculate the volume of 0.250 M H2SO4 that contains 0.250 g H2SO4. 0.250 g H2SO4 x 1 mole x 1 L = 0.0102 L 98.12 g 0.250 mole 5. 1.50 g of NaCl is dissolved in 100.0 mL of water. Calculate the concentration. 6.
Calculate the molarity of the original vinegar solution and its concentration in gdm-3, given that it reacts with NaOH in a 1:1 ratio. 7. 2.5 g of a sample of ethanedioic acid, H2C2O4.nH2O, was dissolved in water and the solution made up to 250 cm3. This solution was placed in a burette and 15.8 cm3 were required to neutralise 25 cm3 of 0.1 moldm-3 NaOH. Given that ethanedioic acid reacts with NaOH
29.4 atm B. 4.89 atm C. 25.1 atm D. 36.0 atm _____ 5. The vapor pressure of pure ethanol at 60 °C is 349 mm Hg. Calculate the vapor pressure at 60 °C of a solution prepared by dissolving 10.0 mol of naphthalene (nonvolatile) in 90.0 mol of ethanol. A.
If the water in this experiment did not boil at 100°C, what could be the reason? a. Atmospheric pressure takes effect with the higher sea levels, causing the water to boil at a lower temperature. B) While heating two different samples of water at sea level, one boils at 102°C and one boils at 99.2oC. Calculate the percent error for each sample from the theoretical 100.0°C. a.
We used .112 moles of bromobenzene, and .0103mole of magnesium moles of Methyl benzoate was the limiting reagent in the experiment. In calculating the theoretical yields. We used the limiting reagent multiplied by the molecular weight of the product. The initiation of the Grignard reaction began after about ten minutes of gentle heating was applied to thereaction flask containing the crushed magnesium turnings and first portion of the bromobenzene/anhydrous diethyl ether solution. This initiation was evident by cloudiness and graying of solution as well as the evolution of bubbles off the surface of the metal.
Eighth, and last, I found molecular weight of sugar and diluted it. Data Tables and Observations: Data Table 1: Length measurements. | Object | Length (cm) | Length (mm) | Length (m) | CD or DVD | 5.2 | 52.0 | .052 | Key | 12.0 | 120.0 | .120 | Spoon | 18.6 | 186.0 | .186 | Fork | 21.0 | 210.0 | .210 | Data Table 2: Temperature measurements. | Water | Temperature (°C) | Temperature (°F) | Temperature (K) | Hot from tap | 46 | 114.8 | 319.15 | Boiling | 100 | 212 | 373.15 | Boiling for 5 minutes | 100 | 212 | 373.15 | Cold from tap | 18 | 64.4 | 291.15 | Ice water – 1 minute | 0 | 32 | 273.15 | Ice water – 5 minutes | 0 | 32 | 273.15 | Data Table 3: Mass measurements. | Object | Estimated Mass (g) | Actual Mass (g) | Actual Mass (kg) | Pen or pencil | 5 | 5.4 | .0054 | 3 Pennies | 6 | 7.6 | .0076 | 1 Quarter | 5 | 5.7 | .0057 | 2 Quarters, 3 Dimes | 15 | 18.2 | .0182 | 4 Dimes, 5 Pennies | 15 | 21.6 | .0216 | 3 Quarters, 1 Dime, 5 Pennies | 25 | 31.9 | .0319 | Key | 10 | 9.2 | .0092 | Key, 1 Quarter, 4 Pennies | 20 | 24.9 | .0249 | Data Table 4: Liquid measurements.
5 g of copper is placed in a solution of silver (I) nitrate containing excess AgNO3. The silver metal produced a mass of 15.2 grams. What is the percent yield? (89.4 %) Gas Laws 1. How many moles of gas does it take to fill a 1.0 L flask at a pressure of 1.5 atm at 100 celsius?
Thermal Insulating Materials: A Self-Directed Experiment In our most recent lab, we determined the specific heat of a solid and learned the relative heat properties of substances having different specific heats. For this self-directed lab, we will determine what makes the best coffee-cup calorimeter and then determine which of various common substances is the best thermal insulating material is. We must first understand that thermal energy flows between two samples of matter at different temperatures. In order to prevent heat from escaping, thermal insulating materials are required to minimize the heat transfer by reducing the transfer of heat between two objects in direct contact, and the transfer of heat by electromagnetic waves. For this experiment we will be using cups of: metal, ceramic, plastic, and Styrofoam for our calorimeters.
There is still carbon dioxide gas dissolved in the liquid at atmospheric pressure. The amount is very small and depends on temperature. It would be interesting to try this experiment again with a cold bottle and a warm bottle. Because carbon dioxide affects the pH of the soda it might be interesting to compare the pH of the fresh out of the bottle and the "defizzed" soda. What is the pressure that is used to put the carbon dioxide into the bottle in the first place?
The smaller amount will ‘limit” how much the reactant can produce. A percent yield in a chemical equation is used because chemical reactions do not predict amount of a substance. The percent yield is usually determined by the mass that is in the chemical reaction. A percentage will be produced from using the formula; This percentage is the calculation of your success of producing a product compared to the total amount of a product that can be produced. The familiar volcano experiment that we all know, mixing baking soda and vinegar, is used to create a bubbly reaction.