The student claims that as a result of the loss of the liquid from the beaker, the calculated number of moles of O2(g) produced is greater than the actual number of moles of 029) produced during the first 60 seconds.
Celebrities that live in maryland 2019
- Calculate the number of aspirin tablets you have prepared: Calculate the percent yield of your aspirin from the formula below. The quantity in the denominator (2.5 g) represents the theoretical yield of aspirin based on the moles of salicylic acid and acetic anhydride used in the synthesis.
- 2.9 What term describes the process that occurs when oxygen is produced? Oxidation . Lab Analysis (TI-Nspire pages 2.10-2.16) Screenshots below show sample data for the experiment. Students’ data will vary and this will cause a variance in the answers to the questions asked. 2.12 Calculate the moles of oxygen produced.
In a certain experiment 2.00 moles of NH3(g) and 10.00 moles. of O2(g) are contained in a closed flask. After the reaction is. complete, 6.75 moles of O2(g) remains. Calculate the number. of moles of NO(g) in the product mixture: (Hint: You cannot. do this problem by adding the balanced equations because you
- 2 (g), is initially present in the container at a pressure of . 0.40 atm. (i) How many moles of Cl 2 (g) are in the container? (ii) How many grams of carbon disulfide, CS 2 (g), are needed to react completely with the Cl 2 (g) ? (b) At 30°C the reaction is thermodynamically favorable, but no reaction is observed to occur. However, at
45. Calculate the number of moles of chlorine needed to form 14 moles of iron(III)chloride. 2Fe(s) + 3Cl2(g) ( 2FeCl3(s) 46. Calculate the mass of oxygen produced from the decomposition of 75.0 g of potassium chlorate. 2KClO3(s) ( 2KCl(s) + 3O2(g) 47. Calculate the mass of silver needed to react with chlorine to produce 84 g of silver chloride.
- Alkali Metal Proton number Number of electrons Electron arrangement Number of valence electrons Lithium 3 Sodium 11 Potassium 19 Rubidium 37 37 220.127.116.11.1 Caesium 55 55 18.104.22.168.8.1 1) Lithium , sodium and potassium have similar chemical properties .
1.For beaker 2 during the 60-second period, calculate the following. The number of moles of O2(g) that was produced. The mass of H2O2 (aq) that decomposed. 2. The student continues the experiment for an additional minute. For beaker 2, will the mass of H2O2(aq)consumed during the second minute be greater than, less than, or equal to the mass of ...
- Changes in reaction conditions can have a tremendous effect on the course of a redox reaction. For example, under standard conditions, the reaction of Co(s) with Ni 2+ (aq) to form Ni(s) and Co 2+ (aq) occurs spontaneously, but if we reduce the concentration of Ni 2+ by a factor of 100, so that [Ni 2+] is 0.01 M, then the reverse reaction occurs spontaneously instead.
May 16, 2014 · You are given a cube of pure copper. You measure the sides of the cube to find the volume and weigh it to find its mass. When you calculate the density using your measurements, you get 8.78 grams/cm 3. Copper’s accepted density is 8.96 g/cm 3. What is your percent error? Solution: experimental value = 8.78 g/cm 3 accepted value = 8.96 g/cm 3
- calculating the number of moles of AgCl. One point is earned for conversion to moles of MgCl 2. (ii) The percent by mass of MgCl 2 in the original mixture 0.0191 mol MgCl 2 × 2 2 95.20 MgCl g 1 mol MgCl = 1.82 g MgCl 2 2 1.82 g MgCl 2.94 g sample × 100% = 61.9% MgCl 2 by mass One point is earned for calculating the correct percentage.
(Use grams moles moles grams) 2.46 g H2O × 1 mol H2O 18.02 g H2O × 2 mol C4H10 10 mol H2O × 58.12 g C4H10 1 mol C4H10 =1.59 g C4H10 d. Moles of oxygen used? 2.46 g H2O × 1 mol H2O 18.02 g H2O × 13 mol O2 10 mol H2O =0.177 mol O2 e. Grams of oxygen used? 2.46 g H2O × 1 mol H2O 18.02 g H2O × 13 mol O2 10 mol H2O × 32.00 g O2 1 mol O2 = 5 ...
- 30. ( Measure 1.0 g of solid sodium hydroxide (NaOH) and set it aside. 31. ( Record the exact mass in Table 2 above. 32. ( Collect temperature data as the reactants are mixed by following the steps you used earlier in the lab: a. Start recording data. (6.2) b. After 60 seconds add the NaOH pellets.
Mr.Gabriel Chemistry Notebook complete, 2017-2018