A sealed cubical container 23.0 cm on a side contains a gas with five times Avogadro's number of neon atoms at a temperature of 30.0°C. HINT (a) Find the internal energy (in J) of the gas. 18889.4 ♥ J (b) The total translational kinetic energy (in J) of the gas. 18889.4 ♥ J (c) Calculate the average kinetic energy (in J) per atom. × J 2/N (d) Use P = 3 를(쓴)(Imvz) to calculate the gas pressure (in Pa). × Pa (e) Calculate the gas pressure (in Pa) using the ideal gas law (PV = nRT). 1040000 Pa The gas pressure can be calculated using either P = 2/N 3 (~) (m²) or the ideal gas law. To within rounding error, each expression gives the correct answ shows that the two expressions are equal. 2 P = 3\V 를(쓴) (2m²)=증(~ 2/nN 3 RT nRT A 2 = 3 V N A

In the text, it was shown that N/V=2.681025m3 for gas at STP. (a) Show that this quantity is equivalent to N/V=2.681019cm3, as stated. (b) About how many atoms are mere in one m3 (a cubic micrometer) at STP? (c) What does your answer to part (b) imply about the separation of Mama and molecules?

On a hot summer day, the density of air at atmospheric pressure at 35.0C is 1.1455 kg/m3. a. What is the number of moles contained in 1.00 m3 of an ideal gas at this temperature and pressure? b. Avogadros number of air molecules has a mass of 2.85 102 kg. What is the mass of 1.00 m3 of air? c. Does the value calculated in part (b) agree with the stated density of air at this temperature?

How many moles are there in (a) 0.0500 g of N2 gas (M = 28.0 g/mol)? (b) 10.0 g of CO2 gas (M = 44.0 g/mol)? (c) How many molecules are present in each case?

A sample of a monatomic ideal gas occupies 5.00 L at atmospheric pressure and 300 K (point A in Fig. P21.65). It is warmed at constant volume to 3.00 atm (point B). Then it is allowed to expand isothermally to 1.00 atm (point C) and at last compressed isobarically to its original state, (a) Find the number of moles in the sample. Find (b) the temperature at point B, (c) the temperature at point C, and (d) the volume at point C. (e) Now consider the processes A B, B C, and C A. Describe how to carry out each process experimentally, (f) Find Q, W, and Eint for each of the processes, (g) For the whole cycle A B C A, find Q, W, and Eint.

(a) Show that the density of an ideal gas occupying a volume V is given by = PM/KT, where M is the molar mass. (b) Determine the density of oxygen gas at atmospheric pressure and 20.0C.

An ideal gas is trapped inside a tube of uniform cross-sectional area sealed at one end as shown in Figure P19.49. A column of mercury separates the gas from the outside. The tube can be turned in a vertical plane. In Figure P19.49A, the column of air in the tube has length L1, whereas in Figure P19.49B, the column of air has length L2. Find an expression (in terms of the parameters given) for the length L3 of the column of air in Figure P19.49C, when the tube is inclined at an angle with respect to the vertical. FIGURE P19.49

A sealed box contains a monatomic ideal gas. The number of gas atoms per unit volume is 6.31×1020 atoms/cm3, and the average translational kinetic energy of each atom is 1.20×10−23 J .   What is the gas pressure? p = ? Pa   If the gas is neon (molar mass 20.18 g/mol ), what is vrms for the gas atoms? Vrms = ____ ? _____ units

n = 3.9 moles of an ideal gas are pumped into a chamber of volume V = 0.135 m3   50% Part (a)  The initial pressure of the gas is 1 atm. What is the initial temperature (in K) of the gas?  T = 421.76T = 421.8     ✔ Correct!     50% Part (b)  The pressure of the gas is increased to 10 atm. Now what is the temperature (in K) of the gas?

Problem 5:   n = 3.9 moles of an ideal gas are pumped into a chamber of volume V = 0.094 m3. Part (a)  The initial pressure of the gas is 1 atm. What is the initial temperature (in K) of the gas?  50% Part (b)  The pressure of the gas is increased to 10 atm. Now what is the temperature (in K) of the gas?