Which of the following substances is suitable for Dumas method to determine its molar mass?a. n-butane (boiling point = -0.5 °C)b. toluene (boiling point = 110.6 °C)%3Dc. propionic acid (boiling point = 141 °C)d. propane (boiling point = -43 °C)e. bromine (boiling point = 59 °C)Clear my choice

Which of the following substances is suitable for Dumas method to determine its molar mass? a. n-butane (boiling point = -0.5 °C) b. toluene (boiling point 110.6 °C) c. propionic acid (boiling point = 141 °C) d. propane (boiling point = -43 °C) e. bromine (boiling point = 59 °C) Clear my choice

Which of the following substances is suitable for Dumas method to determine its molar mass? a. n-butane (boiling point = -0.5 °C) b. toluene (boiling point 110.6 °C) c. propionic acid (boiling point = 141 °C) d. propane (boiling point = -43 °C) e. bromine (boiling point = 59 °C) Clear my choice

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 58QAP: Silicon carbide, SIC, is one of the hardest materials known. Surpassed in hardness only by diamond,...

See similar textbooks

Similar questions

A(n) always has the same composition.
Silicon carbide, SIC, is one of the hardest materials known. Surpassed in hardness only by diamond, it is sometimes known commercially as carborundum. Silicon carbide is used primarily as an abrasive for sandpaper and is manufactured by heating common sand (silicon dioxide, SiO2) with carbon in a turn ace. :math>SiO2(s)+C(s)CO(g)+SiC(s) at mass of silicon carbide should result when 1.0 kg of pure sand is heated with an excess of carbon?
A sample of ascorbic acid (vitamin C) is synthesized in the laboratory. It contains 30.0 g carbon and 40.0 g oxygen. Another sample of ascorbic acid, isolated from lemons (an excellent source of the vitamin), contains 12.7 g carbon. Compute the mass of oxygen (in grams) in the second sample.
24. Sulfur trioxide reacts with water to produce H2SO4. How much sulfuric acid, in grams, can be produced from 10.0 mL of water (d = 1.00 g/mL) and 25.6 g of SO3? use dimensional analysis
A 0.235 mL sample of carbon tetrachloride (density = 1.59 g/mL, MM = 153.81 g/mol) contains how many AMU of Cl? Note: Use 6.022 x 1023 and/or 1.661 x 10-24 as appropriate.
1. A student collected the following data during Lab: Mass of MgCO3 hydrate = 0.9987 g. Constant mass of anhydrous MgCO3 = 0.4831 g How many moles of water were in the MgCO3 hydrate? 2. A student uses gravimetric determination to find the water of hydration of a hydrated sample of cobalt (II) sulfate. The student’s sample contained 0.0098459 moles of anhydrous cobalt(II) sulfate (CoSO4) and 0.068921 moles of water (H2O). What is the formula of the cobalt(II) sulfate hydrate? 3. A student has a sample of CaSO4 hydrate and it weighs 0.4813 grams. He heats it strongly to drive off the water of hydration, and after subsequent heatings, the student finds the anhydrous compound has a constant mass of 0.3750 grams. Find the formula of the hydrate.
Make a dilution series to get to 1:100. Start with making 1:10 dilution by adding 1mL of sample and 9mL of diluent, now continue the series to get to 1:100. The formula you may use is V1D1=V2D2
Calculate the mass % of Na in sodium permanganate. Round your answer to 4 significant figures. Thank you in advance :D
How many grams O in 115.6 g Fe(OH)g? Molar mass of Fe(OH)g is 106.867 Hint: 1 mole Fe(OH)g has 3 mol O; use as a conversion factor Alternatively, use percent by mass Hint: do not need Avogadro's number Put the answer in the box in regular (non-scientific) notation. Use one figure past the decimal.
1.08 ×10-3 mol H2S 57.2 mmol SO3 1.19 mol xenon dioxide m(H2S) = m(SO3)= m(xenon dioxide)=
A mixture weighing 30.500 g contained 4.518 g NH4Cl, 15.250 g SiO2, with the remainder being NaCl. Find the percent, by weight, of each component. Show your method for making the calculations.
Nitrogen ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) N2 (g) 0 0 191.6 N (g) 472.7 455.6 153.3 NH3 (g) -46.1 -16.5 192.5 NH3 (aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 NO (g) 90.3 86.6 210.8 NOCl (g) 51.7 66.1 261.8 NO2 (g) 33.2 51.3 240.1 N2O (g) 82.1 104.2 219.9 N2O4 (g) 9.2 97.9 304.3 N2O4 (l) -20.0 97.0 209.0 N2O5 (s) -42.0 134.0 178.0 N2H4 (l) 50.6 149.3 121.2 N2H3CH3 (l) 54.0 180.0 166.0 HNO3 (aq) -207.4 -111.3 146.4 HNO3 (l) -174.1 -80.7 155.6 HNO3 (g) -135.1 -74.7 266.4 NH4ClO4 (s) -295.0 -89.0 186.0 NH4Cl (s) -314.4 -202.9 94.6 NH4Cl (aq) -299.7 -210.5 169.9 NH4NO3 (s) -365.6 -183.9 151.1 NH4NO3 (aq) -339.9 -190.6 259.8 Oxygen ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) O2 (g) 0 0 205.1 O (g) 249.2 231.7 161.1 O3 (g)…