Get college assignment help at uniessay writers a 10.0 sample of a metal at an initial temperature of 187 degrees celsius is dropped into 10.0 g of water at 20 degreees celsius the final temp is found to be 25 degrees celsius. calculate the specific heat of the metal.
A sample of NO2 gas has a volume of 37.3 mL at a pressure of 621 mm Hg and a temperature of 52 degrees C. Determine the following for this sample a) volume, in milliliters, at T=35 degrees C and P=650 mm Hg b)volume, in liters, at T=43 degreesC and P=1.11 atm c)pressure, in milliliters of mercury, at T=125 degrees C and V= 52.4 mL d)temperature, in degrees Celsius, at P=775 mm Hg and V=23.0 mL
If a sample of gas has 4 moles at a pressure of 567.42 kPa and a volume of 12 L, what is its temperature? Round your answer to the nearest whole number. Don’t forget the units.
How many grams of hydrogen are needed to hydrogenate 30.0g of 2-butene?
What is the final concentration if 75.0 ml of a 3.50m glucose solution is diluted to a volume of 400.0ml ?
Which one of the following statements is NOT consistent with the kinetic-molecular theory? 1. Except near the liquification point, the attractive forces between molecules of a gas are very small. 2. The volume occupied by the molecules (only) of a gas becomes significant only at a very low pressure. 3. Collisions between the molecules of a gas are elastic. 4. A given sample of a gas is mostly empty space except near the liquification point. 5. The attractive forces between the molecules of a gas become significant only at very low temperatures.
Draw the structures of the two organic compounds that can be obtained by oxidizing CH3CH2CH2OH
If a bottle of nail polish remover contains 173 of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788 .
If 5.4 kcal of heat is added to 1.00 kg of water at 100 degrees celsius, how much steam at 100 degrees is produced? Please show your work for your answer.
How many pounds of CO2 are produced from the complete combustion of 1.30 of gasoline? Assume that gasoline has the formula C8H18 and has a density of 0.703
Get college assignment help at uniessay writers predict the mass of oxygen required to react with 14 g of nitrogen to make N2O5 if 16g of oxygen reacts with 14g of nitrogen to make N2O2
Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat? Question 2 answers 10.0 g Fe, CFe = 0.449 J/g°C 10.0 g H2O, CH2O = 4.18 J/g°C 10.0 g Ag, CAg = 0.235 J/g°C 10.0 g ethanol, Cethanol = 2.42 J/g°C 10.0 g Au, CAu = 0.128 J/g°C
6.0 10-8 m to nm
Using the values for delta H°f found in Appendix B of your textbook, calculate H°RXN for the reaction in which acetylene (C2H2) burns in oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). (Hint: first write the balanced equation for the reaction!)
A sample of 1.012 g of KHP (Potassium Hydrogen Phthalate, molar mass = 204.22g/mol) was dissolved in ~ 25 mL distilled water and titrated with a NaOH solution of unknown concentration. If 28.98 mL of base was used to reach the endpoint, what was the concentration of the NaOH (in moles per liter)? Use correct number of significant figures when reporting answer. Reminders:
What mass, in grams, of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?
86 grams of H20 in a calorimeter have an initial temp of 24 degress C. The temperature increased to 33 degrees Celcius when 54 g of a sample of metal initially a 99 Celcius is added to the calorimeter and then allowed to equilibrate with the water. Calculate the specific heat of the metal in joules/g C
Green checks and red X’s are not displayed for this question. You are in charge of a plant that makes methyl bromide, CH3Br. This compound is used as a fumigant for nematodes. The thermochemical equation for the reaction is: CH3OH (aq) Br1- (aq) CH3Br (aq) OH1- (aq) H = 78 kJ/mol You must maximize the yield of the product. Select all of the following actions you would take. Run the reaction with excess bromide ion Remove CH3Br as it is formed Remove bromide ion Allow excess CH3Br to build up in the reaction. Run the reaction in excess CH3OH. Heat the reaction Cool the reaction Remove CH3OH The equilibrium constant for this reaction is . 5. –/3.12 points 1/3 submissions Notes Green checks and red X’s are not displayed for this question. Two gases, A and B, are at equilibrium in a sealed cylinder. Individually, gas A is colorless, while gas B is dark colored. The reaction may be written as: A (g) 2B (g) a) The cylinder should appear as: b) When the system is heated, the cylinder’s appearance is very dark colored. The reaction must be . c) If the reaction equation were written as: 2B (g) A (g) which statements are true? The ΔH value would have the same magnitude value but opposite sign. The color of the cylinder would be darker. The value of K would not change. The K expression would be inverted. 6. –/3.12 points 0/3 submissions Notes Green checks and red X’s are not displayed for this question. You were absent during for the LeChatelier’s Experiment in lab. Your lab partner loaned you his notes to study for the practical mid-term lab exam. The notes consisted primarily of the following table: 2A B Step Procedure Observations 1 Added 5 drops of A. Solution becomes light blue. Test tube feels cool to the touch. 2 Added 10 drops of B and placed in ice. A solid precipitates out. Test tube cooled by ice. 3 Heated test tube for 5 minutes at 45 degrees C. The precipitate dissolves. Solution is light blue. a) From these observions you conclude: The reaction is exothermic; A must exist as a solid; the solution of B is light blue. The reaction is endothermic; A is a light blue solution. The reaction is endothermic; A must exist as a solid; the solution of B is light blue. The reaction is exothermic; A is a light blue solution. b) Graphically, steps 1 and 2 of the procedure could be represented as: 7. –/3.12 points 0/3 submissions Notes Green checks and red X’s are not displayed for this question. Looking back: In CH102 Lab 3, Solubility Rules, students identified ionic salts as soluble or insoluble. The solubility of ionic salts is quantified by an equilibrium constant called Ksp, the solubility product. This Ksp refers to the dissolution reaction of the ionic salts. a) Write the dissolution reaction for the ionic solids below. Please enter all coefficients, even coefficients of 1. Instructions for inputting ions Instructions for inputting chemical formulas material state coeff cation state coeff anion state CaCO3 → FePO4 → KCl → b) The concentration of cations and anions in solution can be predicted from the equation [cation]= , for ionic solids in which the ration of cation to anion is 1:1. Calculate the [cation] concentration of a saturated solution containing the salts below. Indicate if the reaction prefers reactant or product at equilibrium. material Ksp [cation] Equilibrium Preference CaCO3 4.96e-09 reactant product FePO4 9.92e-29 reactant product KCl 44 reactant product c) There is a general relationship between the charges on ions and the Ksp value. Complete the scentence below to describe the relationship: The the Ksp value, the more product that is formed at equilibrium. The lower the charges on the ions in an ionic solid, the more the solid is. 8. –/3.16 points 0/3 submissions Notes Green checks and red X’s are not displayed for this question. Looking back: In CH102 Lab 4, Qualitative Analysis, students used LeChatelier’s Principle to separate Ag1 , Pb2 , and Hg22 . A separation reaction is shown below, with the equilibrium constant of the reaction. Pb2 (aq) 2Cl1- (aq) PbCl2 (s) K = 8.55 x 104 ΔH < 0 a) The K value indicates that the are preferred. b) The following actions will result in more precipitation of the solid: cooling adding Cl1- heating adding NH3 c) The following actions will result in more dissolution of the solid: cooling heating adding NH3 removing Cl1-
If you have 310.0 mL of water at 25 degree celsius and add 100 mL of water at 95 degree celsius, what is the final temperature of the mixture? Use 1.00g/mL as the density of the water.
Calculate the mass of each product formed when 159 g of silversulfide reacts with excess hydrochloric acid. Ag2S(s) HCl(aq) →AgCl(s) H2S(g) [unbalanced] AgCl: ______ grams H2S: ______ grams
Imagine that you have a 6.50 gas tank and a 3.00 gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 135 , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases
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