The van der Waals equation of state for a real gas is n?a V – nb = nRT In this equation, the van der Waals constant, a, represents a correction for O a positive deviation in the measured value of P from that for an ideal gas due to the finite mass of the molecules of a real gas. O a positive deviation in the measured value of P from that for an ideal gas due to the finite volume of space occupied by molecules of a real gas. O a negative deviation in the measured value of P from that for an ideal gas due to the finite volume of space occupied by molecules of a real gas. O a negative deviation in the measured value of P from that for an ideal gas due to the attractive forces between the molecules of a real gas. O a positive deviation in the measured value of P from that for an ideal gas due to the attractive forces between the molecules of a real gas. uthool O HModio

(no subject) - ftar X с < 71″F OPA ! 1 2 app.101edu.co F1 o Mail- Francesca X 2 W F2 #m A sample of gas contains 5.25 moles at 37.8 °C in a volume of 3.61 L. If 0.530 moles of gas are removed from the initial 5.25 moles and the temperature increased to 52.8 °C while pressure is held constant, then what is the new volume of the gas, in liters? 3 E Homepage - CHI X 4 O $ 3 Aktiv Chemistry X R DII F5 % 5 G molar mass of o X T A 6 F6 Question 34.c of 34 Y University of Dela X * & 7 PrtScn FB 8 Online Payment Home 9 ✔ End F10 Sign In 1 4 7 +/- PgUp 0 2 50 8 F11 + 6 9 0 PgDn

Calculate to three significant digits the density of carbon monoxide gas at exactly −20°C and exactly 1atm . You can assume carbon monoxide gas behaves as an ideal gas under these conditions.

Real gases can exist under conditions other than STP. True O False

I only need help with part b

a sample of an ideal gas has a volume of 2.33 L at 287 K and 1.02 atm. Calculate the pressure when the volume is 1.59L and the temperature js 3.00x10^2K

What are the units of a? What are the units of b? For carbon dioxide the numerical value of a is 3.592 and the numerical value of b is 0.0429. atm Use the van der Waals equation to calculate the pressure of a sample of carbon dioxide at 55.0 °C with a molar volume of 0.515 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. atm Explanation Check

Determine the volume in L of one mole of any given gas at T= 0 degrees, 20 degrees and 40 degrees Celsius. Based on your results, discuss the validity of the commonly used molar volume of 22.414 L/mole

A 2.15 g2.15 g sample of an unknown gas at 59 ∘C59⁢ ∘C and 1.00 atm1.00 atm is stored in a 1.95 L1.95 L flask. What is the density of the gas?   What is the molar mass of the gas?

The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: n (p+₁ +²2) (v- (V-nb)=nRT The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? The van der Waals equation of state. R stands for the gas constant and n for moles of gas. What are the units of b? For ethane the numerical value of a is 5.507 and the numerical value of b is 0.0651. Use the van der Waals equation to calculate the pressure of a sample of ethane at 105.0 °C with a molar volume of 5.27 L/mol. Round your answer to the correct number of significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. 0 0 atm atm x10 DO X ロ・ロ