1.7(a) In an attempt to determine an accurate value of the gas constant, R, a student heated a container of volume 20.000 dm filled with 0.251 32 g of helium gas to 500°C and measured the pressure as 206.402 cm of water in a manometer at 25°C. Calculate the value of R from these data. (The density of water at 25°C is 0.997 07 g cm; the construction of a manometer is described in Exercise 1.6a.)

1.7(a) In an attempt to determine an accurate value of the gas constant, R, a student heated a container of volume 20.000 dm filled with 0.251 32 g of helium gas to 500°C and measured the pressure as 206.402 cm of water in a manometer at 25°C. Calculate the value of R from these data. (The density of water at 25°C is 0.997 07 g cm; the construction of a manometer is described in Exercise 1.6a.)

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

A 1.00 L rigid cylinder contains one mole of neon gas at 25 °C. Calculate the pressure using (a) the ideal gas law, and (b) the van der Waals equation. (c) A much more accurate equation is the virial equation, B(T) + V pVm C(T) 1+ RT Vm where B(T) and C(T) are functions of temperature. For neon at 25°C, the values of B(T) and C(T) are 11.42 cm³.mol-1 and 221 cmé.mol2, respectively. Assuming the pressure calculated using the virial equation is the "true" value, determine the percent error by using ideal gas law and van der Waals equation.
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: ( p+a |(V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. 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? What are the units of b? For ammonia the numerical value of a is 4.169 and the numerical value of b is 0.0371. | atm Use the van der Waals equation to calculate the pressure of a sample of ammonia at 170.0 °C with a molar volume of 5.01 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. O atm APR 24 w A olo
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+a- (V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. 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. For water the numerical value of a is 5.464 and the numerical value of b is 0.0305. | atm Use the van der Waals equation to calculate the pressure of a sample of water at 445.0 °C with a molar volume of 2.47 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 APR 49 X W 24 : MacBook Air DD 80 DO0 O00 888 F9 F10 F7 F8 F5 F6 F2 F3 F4
Because of their different molar masses, H₂ and D₂ effuse at different rates . (a) If it takes 16.5 min for 0.10 mol of H₂ to effuse, how long does it take for 0.10 mol of D₂ to do so in the same apparatus at the same T and P? (b) Howmany effusion steps does it take to separate an equimolar mix-ture of D₂ and H₂ to 99 mol % purity?
In a container of 80 I at 50 ° C under vacuum, 7 g of N2, 16 g of O2 and 3.03 g of H2 are introduced. Calculate the partial pressure of each gas, the total pressure, and the composition of the mixture in mole percent.
6. On a certain day a laboratory barometer indicates that the atmospheric pressure is 786.2 torr. A sample of gas is placed in a flask attached to an open-end mercury manometer, and a meter stick is used to measure the height of the mercury in the two arms of the U tube. The height of the mercury in the open-end arm is 80.4 mm, and the height in the arm in contact with the gas in the flask is 123.5 mm. What is the pressure of the gas in the flask (a) in atmospheres, (b) in kilopascals?
5. Does the pressure-volume relationship follow the ideal gas law PV=nRT (is PV constant at constant n and T) Using the room temperature calculate the number of moles in the pressure/volume experiment when the pressure is 1.00atm in 3.1
5.69 You want to store 165 g of CO2 gas in a 12.5-L tank at room temperature (25°C). Calculate the pressure the gas would have using (a) the ideal gas law and (b) the van der Waals equation. (For CO2, a = 3.59 atm L^2/mol^2 and b = 0.0427 L/mol.)
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: 2 p+a (V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. v? 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? What are the units of b? For ammonia the numerical value of a is 4.169 and the numerical value of b is 0.0371. atm Use the van der Waals equation to calculate the pressure of a sample of ammonia at 195.0 °C with a molar volume of 4.12 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 O
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.
The critical pressure, Pe, and the critical temperature, Te, of gas A are 3.040 × 10° Pa and 473 K, respectively. (i) Calculate the van der Waals constants, a and b, for this gas. (ii) Gas A obeys the van der Waals equation. Calculate the pressure exerted by one mole of gas A if the molar volume occupied by this gas is 2.75 L/mol at 298 K.
Calculate the experimental value of R when a student uses 0.28 g Mg, the atmospheric pressure is 770 torr, the temperature of the water bath is 25 °C, and the volume of gas collected after equalizing the water levels in the Florence flask and trough is 500. mL PV = nRT n is the moles of hydrogen, T is temperature, V its volume in liters, and P the pressure in torr.