Part B: NazCO; Reaction: 1. Determine the experimental mole-to-mole ratio of NazCO3 to NaCl from reaction data. a) First, convert the mass of both Na2CO3 used and mass of NaCl obtained to moles. Na2CO3 NaCl b) Then, divide your answers from (a) by the lower mole value to determine the simplest mole-to- mole ratio between Na2CO3 and NaCl. Calculate your answers a) before rounding to the nearest whole number and b) after rounding to the nearest whole number. What is the expected mole-to- mole ratio?

Part B: NazCO; Reaction: 1. Determine the experimental mole-to-mole ratio of NazCO3 to NaCl from reaction data. a) First, convert the mass of both Na2CO3 used and mass of NaCl obtained to moles. Na2CO3 NaCl b) Then, divide your answers from (a) by the lower mole value to determine the simplest mole-to- mole ratio between Na2CO3 and NaCl. Calculate your answers a) before rounding to the nearest whole number and b) after rounding to the nearest whole number. What is the expected mole-to- mole ratio?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter9: Gases

Section: Chapter Questions

Problem 86E: During the discussion of gaseous diffusion for enriching uranium, it was claimed that 235UF6...

See similar textbooks

Similar questions

The highest building in Montreal is the ‘1 square building’, with a height of 203m.The atmospheric pressure in the streets of Montreal is P1 = 9.9 x 104Pa.Suppose air density is constant : ρair= 1,2 kg/m3 and g = 9.8 m/s2. Suppose the rooftop temperature to be T = 298K, and the air composition is 100%N2 molecules. The collision cross-section of N2 molecules is 0.43 nm2.*f. Find the collision frequency. Is it in the order of magnitude that you wereexpecting?
In Part B, you used a similar procedure to that of Part A to determine the mass percent of CaCO3 in an antacid tablet. The commercially accepted range of CaCO3 in an antacid tablet is 25–35% by mass. Miranda obtained the data below from her Part B trial: TRIAL PRESSURE (torr) MASS OF TABLET (g) TEMPERATURE (°C) VOLUME CO2 RECOVERED (mL) 1 750.5 0.5702 21.3 69.6 2 750.5 0.5622 21.2 68.2 Miranda determined her average % Recovery of CO2 to be 65.0% from Part A. Based on her data collected from Part A, was the average percent mass of CaCO3 in her antacid tablet within the commercially accepted range? Yes, her mass percent does fall within the commercially accepted range. No, her mass percent does not fall within the commercially accepted range.
Soil vapor extraction (SVE) is used to remove volatile or-ganic pollutants, such as chlorinated solvents, from soil at haz-ardous waste sites. Vent wells are drilled, and a vacuum pump is applied to the subsurface. (a) How does this remove pollutants?(b) Why does heating combined with SVE speed the process?
the following experiment is reference from this video link, they are the first 2 experiments ; reference https://www.youtube.com/watch?v=NFTBOIvTLtI
Eugenol, the main component of clove oil, can be prepared by heating 2-allyl guaiacol (in the absence of oxygen) to temperatures >205 °C. In practice, however, it is most cost-effective to extract eugenol from cloves, its natural source. Given a weight percentage of eugenol in cloves at 15.0%, calculate the minimum mass of cloves one needs to obtain 8.00 g of eugenol as a product. Report your answer (as a mass in grams, without units) with three significant digits.
A student dissolves 10.3g of ammonium nitrate NH4NO3 in 300.g of water in a well-insulated open cup. He then observes the temperature of the water fall from 22.0°C to 19.3°C over the course of 3.1 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH4NO3s -> NH+4aq + NO−3aq You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔHrxn per mole of NH4NO3.
Combustible vapor-air mixtures are flammable over a limitedrange of concentrations. The minimum volume % of vapor thatgives a combustible mixture is called the lower flammable limit(LFL). Generally, the LFL is about half the stoichiometric mix-ture, the concentration required for complete combustion of thevapor in air. (a) If oxygen is 20.9 vol % of air, estimate the LFL forn-hexane, C₆H₁₄. (b) What volume (in mL) of n-hexane (d=0.660 g/cm³) is required to produce a flammable mixture of hexane in 1.000 m³of air at STP?
5 In the plot of lnK vs 1/T, data is not actually a straight line? What does this indicate about ΔH°? Does it indicate anything about ΔS° ?
You have a lot of paperwork laying around. A ream of stacked paper is 500 sheets and is 2.0 inches thick. Let's say you had a mole of paper. (1 mole of paper = 6.022 x 1023 sheets of paper) and it was all stacked up in 10 stacks of equal height, each containing a tenth of a mole of sheets. The ten stacks sit one on top of the other. How high are they? (Hint: find the height of a stack of containing 0.1 mole of paper. USE DIMENSIONAL ANALYSIS!) Here are are some conversions you might need: 2.54 cm = 1 in; around 9.46 x 1015 meters / light yr and 3.26 light yr / parsec.
Salicylic acid and ethanamide were made to react in basic medium to produce aspirin and substance X. A chemist is doing a research regarding the synthesis and have seen in scientific references that the process would produce an expected amount of 8.6 grams of aspirin at 74.2% efficiency given the right condition and amount of starting material: Density Ethanamide: 1.16g/mLA. What is the probable identity of Substance X? B. How much (grams) of substance X is produced? C. How many grams of Salicylic acid was used? D. How many grams of ethanamide should be used? E. What volume of excess ethanamide must be taken from the stock ethanamide solution? F. Show the mechanism of the reaction. OWN SOLUTION AND ANSWER ALL FOR UPVOTE
Salicylic acid and ethanamide were made to react in basic medium to produce aspirin and substance X. A chemist is doing a research regarding the synthesis and have seen in scientific references that the process would produce an expected amount of 8.6 grams of aspirin at 74.2% efficiency given the right condition and amount of starting material: Density Ethanamide: 1.16g/mLA) What is the probable identity of Substance X?B) How much (grams) of substance X is produced?C) How many grams of Salicylic acid was used?OWN SOLUTIONS AND NOT AI FOR UPVOTE
During the discussion of gaseous diffusion for enriching uranium, it was claimed that 235UF6 diffuses 0.4% faster than 238UF6. Show the calculation that supports this value. The molar mass of 235UF6 = 235.043930 + 6 ×18.998403 = 349.034348 g/mol, and the molar mass of 238UF6 = 238.050788 + 6 × 18.998403 = 352.041206 g/mol.