5) While making an inventory of the Chemistry Laboratory, Din Djarin found a dusty amber bottle hidden in one of the cabinets and the bottle has the following label: "Compound R with empirical formula C3H302. (empirical Mw = 71 g/mol), in 50.0 g of ethanol" A preliminary test concluded that this solution boils at 79.03°C and after evaporating the ethanol it is found that there are 5.5 g of compound R. a) Calculate the molality of the solution. (Tb of alcohol = 78.4 °C, Kb = 1.22 °C/m). mol m= kg A b) Calculate the molar mass of the solute. t c) What is its molecular formula?.

5) While making an inventory of the Chemistry Laboratory, Din Djarin found a dusty amber bottle hidden in one of the cabinets and the bottle has the following label: "Compound R with empirical formula C3H302. (empirical Mw = 71 g/mol), in 50.0 g of ethanol" A preliminary test concluded that this solution boils at 79.03°C and after evaporating the ethanol it is found that there are 5.5 g of compound R. a) Calculate the molality of the solution. (Tb of alcohol = 78.4 °C, Kb = 1.22 °C/m). mol m= kg A b) Calculate the molar mass of the solute. t c) What is its molecular formula?.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

cricket A ♡ | 32% 8:47 PM 25. Some people like to make their own hand lotion because it can be less expensive than buying it and they have the ability to add only the fragrances that they like. A recipe for hand lotion calls for mixing 327 g of water (H,O) with 311 g of glycerin (C3H3O3). This recipe makes a total of 550. mL of hand lotion. (a) What is the mass percent of glycerin in the hand lotion? (b) What is the molarity of glycerin in the hand lotion? OÇR OCR Sign Delete
What is the melting point of a 100 g sample of water that contains 2 mol of ethanol? One mole of the following substance is added to 1000 grams of water. What is the final freezing point of the solution in degrees Celsius (assuming the substance dissolves completely)?Sucrose CHO, a common sweetener What type of reaction is this? 2 Mg (s) + CO (g) → C (s) + 2 MgO (s) What type of reaction is this? 2 CO (g) + O (g) → 2 CO (g)
12.
q 2req Visited 2req [Review Topics] [References] Use the References to access important values if needed for this question. The boiling point of ethanol, CH3 CH₂OH, is 78.500 °C at 1 atmosphere. Kb (ethanol) = 1.22 °C/m In a laboratory experiment, students synthesized a new compound and found that when 10.17 grams of the compound were dissolved in 204.5 grams of ethanol, the solution began to boil at 78.723 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol Submit Answer Q Graph_08-30-2....pdf NO Retry Entire Group O J A 9 more group attempts remaining I' 6 Previous Next> Show all 11:15 PM 9/12/2022
If nickel(II) sulfate is heated too strongly, the following reaction will occur NISO4(s) NiO(s) + SO3(8) If you are heating a sample of NISO4 7H20 and this reaction occurs along with dehydration, what will happen to the experimental percent water? Explain your answer.
Complete the given reaction
04/22/ 2021 ot art e b NAME Kouri KulRu DATE SECTION POSTLABORATORY ASSIGNMENT 1. Calculate the theoretical percentage of water for the following hydrates. (a) manganese(II) monohydrate, MnSO4 • H2O (b) manganese(II) tetrahydrate, MNSO4 • 4H2O 2. An unknown hydrate, AC• XH»O, has a mass of 1 .00 g before heating, and 0.738 g atter heating. What is the experimental percentage of water in the hydrate? ombvl lo slmo noihesilla logataW If the anhydrous compound (AC) has a molar mass of 101 g/mol, what is the water of crystallization (X) and the formula for the hydrate (AC XH,O)?ouphut suf (snoilgo) ai sh Formula of hydrate AC H20 Water of crystallization
[References] Use the References to access important values if needed for this question. The boiling point of ethanol, CH3 CH₂OH, is 78.500 °C at 1 atmosphere. K₁ (ethanol) = 1.22 °C/m In a laboratory experiment, students synthesized a new compound and found that when 14.95 grams of the compound were dissolved in 293.3 grams of ethanol, the solution began to boll at 78.570 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol Submit Answer Retry Entire Group 9 more group attempts remaining Show Hint Congage Learning Cengage Technical Support Previous Next Save and Exit
5. Chemical Xis a solid with white color that forms large crystals. The solubility of chemical X in water at different temperatures is shown below. Solubility of X in H20 124 10- 8- 6- 2- 0+ Ó 10 20 30 40 50 60 70 80 90100 Temperature (°C) Irina wants to dissolve 30 grams of Xin 1 liter of water. She does so by stirring 30 grams of the large crystals into 1 liter of water at 45°C. How could Irina change her method to dissolve all the X faster? Solubility (g/100 g H,O) 4-
Acetylene torches are used for welding. These torches use a mixture of acetylene gas, C2H2C2H2, and oxygen gas, O2O2 to produce the following combustion reaction: 2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g)2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g) Part A Imagine that you have a 7.00 LL gas tank and a 4.50 LL 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 125 atmatm , 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. Express your answer with the appropriate units.
The diving atmosphere used by the U.S. Navy in its undersea Sea-Lab experiments consisted of 0.036 mole fraction O2 and 0.056 mole fraction N2, with helium (He) making up the remainder. What are the masses of nitrogen, oxygen, and helium in a 8.47 g sample of this atmosphere? Mass of oxygen = Mass of nitrogen = Mass of helium =
You have a container of 17.42 M conc. acetic acid (CH3COOH(aq)) with density 1.05 g/mL, find the molality of a 150ml sample of the solution. molality = moles solute/Kg solvent moles solute = (0.150 L)(17.42 mol/L) = 2.613 mol CH3COOH molar mass of CH3COOH = 60.06 g/mol grams of solution = (150mL)(1.05 g/mL) = 157.5 g solution grams of solute = (2.613 mol)(60.06 g/mol) = 156.9 g CH3COOH so the total grams of water in this solution would be: g H2O = g solution - g CH3COOH = 157.5g - 156.9 g = 0.6g H2O 0.6g H2O = 0.0006 Kg H2O so molality = (2.613 mol CH3COOH) /(0.0006 kg H2O) = 4355 molal this seems rather high to me but if its 'concentrated' acetic acid, I know that you can get it to about 98% as glacial acetic acid so perhaps there is 4355 moles of acetic acid per kg of water. Did I do this correctly? I know that typically the solvent is the larger component of a solution but the fact that it gives me CH3COOH(aq) would imply that H2O is the solvent still in this situation, I have…