The enthalpy of vaporization for acetone is 32.0 kJ/mol. The normal boiling point (@1.00 atm) for acetone is 56.5 C. What is the temperature of acetone at 560 torr? Can you explain how to solve this using the claussius formula i provided below. Im horrible at math so please help me understand it in a simple manner.

The enthalpy of vaporization for acetone is 32.0 kJ/mol. The normal boiling point (@1.00 atm) for acetone is 56.5 C. What is the temperature of acetone at 560 torr? Can you explain how to solve this using the claussius formula i provided below. Im horrible at math so please help me understand it in a simple manner.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter1: The Nature Of Chemistry

Section: Chapter Questions

Problem 13QRT

See similar textbooks

Similar questions

hyrw 2o nsn hyapsn sem St.) Calcium oxide is sometimes very challenging to etare n the Oumistry labrortory.This compound reacts with moisture in the air and is converted to calcium hydcokide. If a bottle of calcium oxide i8 left on the ehelf too long, it grodually absorbs moisture from the humidity in the laboratory. Eventually th bottle cracks and spills the colcium hydrokide that hus been produced. WrHhe the unbalancaed chemical equaher for this process. 33.) The clement tin often occurs in nature as the oxide, Sn b produce pure tin metal from this sort of tin oe, the ore Gtmol rom the usually is heated with coal Carbon) This produies pure
'cat' represnts HA 'mat' represents H3O+ 'rat' represents A- Container(i) has 1 cat, 4 mat, 4 rat. Container(ii) has 4 cat, 1 mat, 1 rat. Container(iii) has 2 cat, 3 mat, 3 rat. Container(iv) has 3 cat, 3 mat, 3 rat. Container(v) has 9 cat, 2 mat, 2 rat. From the given information, identify (a) Strongest Acid (b) Weakest Acid (c) Highest pKa
التاريخ How manymolesetcoRferafe in 6,000r000atome of Copper
J= M = i 0: = 1. NaBH4 2. dilute H* N 1. K 2. L 1.03 2. S(CH3)2 K= H3CO H3CO. M N = P = 1. NaNH2 2. Br CI L= O P 1. CN- 2. Na (s), NH3 (1), cold
/ext/map/index.html?_con%3Dcon&external_browser%3D08launchUrl%=https%253/ Chapter 6 HW # 2 Saved 3 attempts left Check my work Be sure to answer all parts. 1 A mercury mirror forms inside a test tube as a result of the thermal decomposition of mercury(II) points oxide: 2 HgO(s) →2 Hg(!) + O2(g) AH = 181.6 kJ References (a) How much heat is needed to decompose 513 g of the oxide? kJ (b) If 607 kJ of heat is absorbed, how many grams of Hg form? x 100 g Hg (Enter your answer in scientific notation.) Mc Graw Hill < Prev 3 of 15
요 Eto OEt 1. EtMgBr(xs) 2. H3O* HO
Br (CH3)¿CuLi CuLi Br K H20 MgBr H20 M МоBr
Q2: Calculate the mole fraction of 15 % (w/w) CeH12O6? Note: Atomic wt.: Na= 23, CI= 35.5, C=12, H=1, O=16
ebixoiC 4 During the production of ammonia, hydrogen is produced from the steam reforming of methane. In the reformer methane gas is reacted with excess water and the resulting mixture is found to contain 12 kg of hydrogen and 15 kg water. Assuming all the methane is reacted calculate the amount of water used.
Ten replicate analyses of the concentration of mercury in a sample of commercial gas condensate gave the following results:23.3 22.5 21.9 21.5 19.9 21.3 21.7 23.8 22.6 24.7 ng ml−1
The so called hydrogen economy is based on hydrogen produced from water using solar energy. The gas may be burned as a fuel: 2H2 (g) + O2 (g) ---> 2H2O (l) A primary advanatge of hydrogen as a fuel is that it is nonpolluting. A major disadvantege is that it is a gas and therefore is harder to store than liquids or solids. Calculate the volume of hydrogen gas at 25oC and 1.00 atm required to produce an amount of energy equivalent to that produced by the combustion of a gallon of octane (C8H18). The density of cotane is 2.66 kg/gal and its standard entalpy of formation is -249.9 kj/mol.
15. What volume (in L) of cobalt can be produced when 55.0 kg of colbalt(III) oxide reacts with 5.00 L of carbon? How many liters of excess reactant is leftover? (dCo(s) = 8.90 g cm; dcs) = 2.26 g cm -) Co,O3 (s) + C(s) → Co(s) + CO;(g) A: 4.4; 2.36