kb = 1.381 · 10-23 JK-1 NA = 6.022 · 1023 mol-1 Part A Calculate the...
Calculate the average kinetic energy 〈K〉 for 1 mole of N2 gas at 293 K in a 20 L container. kB=1.381*10^(-23) J K^-1 NA=6.022*10^23 mol^-1
General Chemistry: Gases and the Kinetic Molecular Theory Constants NA = 6.022 x 1023 Equalities 1 atm = 760 torr (exact) 1 atm = 760 mmHg 1 atm = 29.92 inHg 1 atm = 101325 Pa 1 atm = 14.7 psi Equations 9°F TE TC +32°F 5°C 5°C TC (TE - 32°F) 9°F TK = Tc + 273.15 R L.atm 0.08206 mol. PV = nRT A gas sample containing 1.50 moles at 25°C exerts a pressure of 7.74 psi. Some...
NA 6.022 x 103 molecules/mole k 1.381 x 1023 J/K c 2.997 x 108 m/s 1 cal 4.186 J mp 1.673 x 1027 kg 1 atm 1.013 bar h 6.626 x 10-34 Js R 8.315 J/(mol K) 1 bar 10% Pa 1. (15 points) 2.0 moles of a monatomic ideal gas undergo a 3 step cyclic process. The process begins in state A at 1.00 atm, 297 K. The gas is heated slowly at constant pressure until it reaches state...
Part A According to the equipartition principle, what is the overall energy in J of one mole of water at 1400 K if translational, rotational, and vibrational degrees of freedom are considered? The values of the vibrational constants of water are roughly 1600 cm-and 3700 cm ). kg = 1.381 . 10-23 JK-1 R - 8.314 JK-1 mol-1 Calculate the higher limit for the overall energy in J of one mole of water at 1400 K assuming that all vibrations...
Part A Calculate the pressure, in atmospheres, of 2.43 mol of helium gas in a 10.0L container at 25°C. Express your answer to three significant figures and include the appropriate units. P- Value Units Submit Request Answer
For the equilibrium Br2(g)+Cl2(g)⇌2BrCl(g) at 400 K, Kc = 7.0. Part A If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Br2? Express your answer to two significant figures and include the appropriate units. Part B If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Cl2?...
Boltzmann’s constant is 1.38066 × 10−23 J/K, Avogadro’s number is 6.02214 × 1023 mol−1. Use the mass of Hydrogen molecules per mole to be mH2 = 2 g/mol. Calculate the rms speed of an H2 molecule at 208◦C. Answer in units of m/s.
Part A Constants 1 Periodic Table Two cylinders each contain 0.30 mol of a diatomic gas at 270 K and a pressure of 3.0 atm. Cylinder A expands isothermally and cylinder B expands adiabatically until the pressure of each is 1.0 atm What is the final temperature of the gas in the cylinder A? Express your answer to two significant figures and include the appropriate units. n 320 K Submit X Incorrect; Try Again; 4 attempts remaining Part B What...
A 2100 cm container holds 0.13 mol of hellum gas at 350 - Part A How much work must be done to compress the gas to 1500 em at constant pressure? Express your answer to two significant figures and include the appropriate units. HAR O ? W = Value Units Submit Request Answer Part B How much work must be done to compress the gas to 1500 cm at constant temperature? Express your answer to two significant figures and include...
The molecular mass of helium is 4 g/mol, the Boltzmann’s constant is 1.38066 × 10−23 J/K, the universal gas constant is 8.31451 J/K · mol, and Avogadro’s number is 6.02214 × 1023 1/mol. Given: 1 atm = 101300 Pa. How many atoms of helium gas are required to fill a balloon to diameter 26 cm at 14◦C and 1.696 atm? What is the average kinetic energy of each helium atom? Answer in units of J. What is the RMS speed...