a) Calculate the volume (in L) occupied by 16 g of Carbon dioxide gas at a pressure of99.7 x 103 Pa and a temperature of 100°C. (R= 8.314 JK1 mol-¹). What assumptionshave you employed with this calculation?b) Predict whether the following liquid-liquid mixtures are miscible and explain youranswer.c)1. CH3NH3 and CH3CH2CH₂CH2CH₂CH₂CH₂CH3ii. CH3CN and H₂OFor the following pairs of functional groups, predict which would likely have thehigher boiling point and justify your answer.i. Alcohol and Ketoneii. Ether and Aldehyde

Answered: Image /qna-images/answer/26380f8c-f282-4698-aa5f-ef319343123f.jpg

a) Calculate the volume (in L) occupied by 16 g of Carbon dioxide gas at a pressure of 99.7 x 103 Pa and a temperature of 100°C. (R= 8.314 JK-1 mol ¹). What assumptions have you employed with this calculation?

a) Calculate the volume (in L) occupied by 16 g of Carbon dioxide gas at a pressure of 99.7 x 103 Pa and a temperature of 100°C. (R= 8.314 JK-1 mol ¹). What assumptions have you employed with this calculation?

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

江苏高考分数线 A Acellus Applications of the Ideal Gas Law 0.0453 moles of hydrogen gas were produced by the reaction. Calculate the volume of the gas at standard temperature and pressure. Mg + 2HCI → MgCl2 + H₂ Volume H₂ = [?]L C Liters of H₂ Enter 28 2 Resources Help
To the nearest 0.1 g, how many grams of a candle wax from a different brand of candle can be burned in 5-gallon container sealed with air? Assumptions (may or may not be needed): Complete combustion to CO2 and H2O; Candle wax reacts in a ratio of 1 mol wax: 40 moles O2; MW (wax) = 370 g/mol, Air = 21% oxygen, R= 0.082 L.atm.K-1.mol-1, 1 gallon = 3.785 L, T=278 K, P = 1 atm
(b) If a 2.302g sample of impure cobalt(III) carbonate is heated, and 415mL of carbon dioxide is collected at 23°C and a pressure of 1.512atm, what is the percent cobalt(III) carbonate in the sample? (b) If a 2.302 g sample of impure cobalt(III) carbonate is heated, and 415 mL of carbon dioxide is collected at 23°C and a pressure of 1.512 atm, what is the percent. cobalt(III) carbonate in the sample?
Solid ammonium chloride, NH4Cl, is formed by the reaction of gaseous ammonia, NH3, and hydrogen chloride, HCI. NH₂(g) + HCl(g) → NH₂Cl(s) A 4.68 g sample of NH3 gas and a 4.68 g sample of HCl gas are mixed in a 1.00 L flask at 25 °C. Identify the limiting reagent. O HCI O NH₂CI O NH3 How many grams of NH₂Cl will be formed by this reaction? mass: What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH4Cl produced by the reaction. P = atm
The human body burns glucose (C6H12O6) for energy according to this chemical reaction: C6H12O6+6O2→ 6CO2+6H2O The products of the reaction are carbon dioxide CO2 and water H2O Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500.mL of air, which is typically enriched to 4% CO2 and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 0.50kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO2 is 2.0 kg/m^3 .
Say you could capture the carbon dioxide gas produced by the combustion of 1 gallon of octane at 22 degrees Celsius and 1.01 atm. Use the ideal gas law to determine the volume of co2 produced.
The best laboratory vacuum pump can generate a vacuum of about ∆H f olecular chlorine and molecular fluorine combine to form a gaseous product. Under the same conditions of temperature and pressure it is found that one volume of Cl2 reacts with three volumes of F2 to yield two volumes of the product. What is the formula of the product? (b) Methane, the principal component of natural gas, is used for heating and cooking. The combustion process is
In 1897 the Swedish explorer Andree tried to reach the North Pole in a balloon. The balloon was filled with hydrogen gas. The hydrogen gas was prepared from iron splints and diluted sulfuric acid. The reaction is Fe(a) + H,S0, (ag) + PeSO(og) + H;(s) The volume of the balloon was 4800 m and the loss of hydrogen gas during filling was estimated at 20% What mass of iron splints and 98 (by mas) H,S0, were nooded to enre the complete filling of the balloon? Assume a temperature of oC, a presaure of 10 atm during filling nd 100 yield. Mass of Fe Mass of HaS0, -
A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 550. L and heated to 520.0 °C. When the amount of CaCO3 has stopped changing, it is found that 8.46 kg have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 520.0 °C. Round your answer to 2 significant digits. P Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. 0 X
Calculate the total pressure (in atm) of a mixture of 3.00 x 10-2 mol of helium, He, and 7.00 x 10- mol of oxygen, O2, in a 6.00 L flask at 20.°C. Assume ideal gas behavior. Total pressure atm ||
5.(a) Assume for the moment that air consist of 80.00% nitrogen and 20.00% oxygen byvolume. Use these figures and typical values for temperature and pressure (1.000atm, 25.0 ºC) to calculate the density of air. (b) This calculation affords a good approximation of the density of air at sea level.However, your lab is at an altitude approximately 777 meters (2550 feet). Knowingthis, will the density of air in you lab be higher or lower than the value you justcalculated? Why? (c) Besides altitude, what else affects the atmospheric pressure? Where could you findthe actual atmospheric pressure at the time of the experiment?