Question 1a) At T= 100 K, 1.00 mol of CO2 occupies a volume of 1.00 L. Calculate the pressures givenby the ideal gas equation and the van der Waals equation. (a= 3.610 atm dm° mol-?) and (b =4.29 dm³ mol-1).b) At a temperature of 100° C and a pressure of 27.6 MPa (1 MPa = 1 x 106 Pa), two moles ofcarbon dioxide occupy a volume of 140.06 cm³. Calculate the compressibility factor.

given data from the question are - a) volume = V = 1 lit temperature =T = 100K a = 3.610 atm dm6…

Question 1 a) At T= 100 K, 1.00 mol of CO2 occupies a volume of 1.00 L. Calculate the pressures given by the ideal gas equation and the van der Waals equation. (a= 3.610 atm dm mol2) and (b = 4.29 dm' mol-!). b) At a temperature of 100° C and a pressure of 27.6 MPa (1 MPa = 1 x 106 Pa), two moles of carbon dioxide occupy a volume of 140.06 cm³. Calculate the compressibility factor.

Question 1 a) At T= 100 K, 1.00 mol of CO2 occupies a volume of 1.00 L. Calculate the pressures given by the ideal gas equation and the van der Waals equation. (a= 3.610 atm dm mol2) and (b = 4.29 dm' mol-!). b) At a temperature of 100° C and a pressure of 27.6 MPa (1 MPa = 1 x 106 Pa), two moles of carbon dioxide occupy a volume of 140.06 cm³. Calculate the compressibility factor.

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

Please help me to give you thumbs up
What pressure (in torr) of carbon dioxide gas can be produced by the combustion of 1.00 g of benzene (C6H6) in a closed, 25.0 L container at a temperature of 15°C? 2C6H6(l)+15O2(g)-->12CO2(g)+6H2O(l)
How many liters of 0.22 M NaOH is needed to completely react with 0.187 L of 0.63 M H2SO4? 2 N2OH(aq) + H2SO4(aq) --> 2 H20(1) + Na2SO4(aq) Express you answer with two significant figures.
Answer part a and b
I only need help with part b
Ammonia, NH,, reacts with oxygen to form nitrogen gas and water. 4 NH, (aq) + 3 0,(g) → 2 N, (g) + 6 H,O(1) If 2.65 g of NH, reacts with 3.98 g of O, and produces 0.450 L of N, at 295 K and 1.00 atm, which reactant is limiting? O NH; (aq) '3 0,(g) What is the percent yield of the reaction? percent yield: %
I have a hard time
#4
What pressure will be exerted, in kPa, by 0.200 moles of carbon dioxide gas with a volume of 0.500 L at a temperature of 27°C? (Number only, no units) Blank 1:
I need the answer as soon as possible
A gaseous organic compound containing only carbon, hy-drogen, and nitrogen is burned in oxygen gas, and the volume ofeach reactant and product is measured under the same conditions of temperature and pressure. Reaction of four volumes of thecompound produces four volumes of CO₂, two volumes of N₂,and ten volumes of water vapor. (a) What volume of O₂ was re-quired? (b) What is the empirical formula of the compound?
2. (a) How many moles of oxygen gas are present if the volume is 500 milliliters at a temperature of 25o C and a pressure of 90 atm ?(R= 0.0821 L*atm/mole*K). (b) Helium balloons have a volume of 10 liter at 100o C and a pressure of 800 mmHg, what is the new volume at 350 K and a pressure of 1.5atm?