Q3 part A

+ |/ 00 %24 D. Two bulbs are connected by a stopcock. The 7.50 L bulb contains nitric oxide (NO) at a pressure of 0.340 bar, and the 2.50 L bulb contains oxygen (O,) at a pressure of 0.510 bar. 02 ON After the stopcock is opened, the gases mix and react to produce nitrogen dioxide (CON) 2 NO(g) + 0,(g) – 2 NO,(g) Considering that the volume remains unchanged during the experiment, how does the total pressure in the bulbs change if the reaction is allowed to go to completion? The total pressure will remain constant. O There is not enough information to determine how the total pressure will change. O The total pressure will decrease. O The total pressure will increase. MacBook Pro ( The %23 %24 7. 4. 5. 3. R %3D K. H. B C. option command MOSISO

In the following relationships, which quantities are variables and which are fixed: (a) Charles's law; (b) Avogadro's law; (c) Amontons's law? For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIUS Paragraph Arial 10pt E v E A I

A mixture of cyclopropane gas (C3H6) and oxygen (O2) in mole ratio 1.00 : 4.00 is used as an anaesthetic. What mass of each of these gases is present in a 1.15 L bulb at 14.7°C if the total pressure is 1.00 bar?m (C3H6) = ------------  gm (O2) =  -------------- g

Gas Pressure Conversions • A given P(atm) takes different column heights (h) of different liquids (p) to balance in a barometer: P(H,0) = p(H,O) gn h(H,0) P(atm) = p(Hg) g, h(Hg) 1 h oc %3D %3D ... Find mm(H,0) that measures 1 atm = 760 mmHg: %3D h(H,O) = h(Hg) x e(Ha= 760 mm(Hg) x 13.5_g/mL = [O,2le0 mm(H,O) %D %3D p(H2O) 1.0 g/mL A barometer with liquid twice as dense as water shows 1 atm as: 0.38 m 1.52 m 5.15 m 20.6 m Convert 3.11 x 10-5 atm into mTorr 1 atm =100 Torr 3.11 x 10-5 atm xloO Torr 1 atm 1 mTorr 10-3 Torr 23.0mTorr (AKA: µ) 1 in(Hg) = 25.t mm(Hg) Pa = 29.92 inHg 80.6 KPa Convert 23.8 inHg into kPa %3D 1 atm = 760 mmHg = (01325 25.4 mm(Hg)x 1 in(Hg) %3D 101325 Pa 760 mmHg 1o Pa 23.8 inHg x x 1 kPa =

The average kinetic energy of the molecules in a gas sample depends only on the temperature, T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed 3 RT rms speed %3D where R = 8.314 J/(mol-K) and M is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (kg-m²/s²). What is the rms speed of O, molecules at 411 K? rms speed: m/s What is the rms speed of He atoms at 411 K? rms speed: m/s

Given a gas sample with a Temperature of 298 K, a Pressure of 1.2 atm, and a molar quantity of 0.12 moles. Solve for Volume (in L) PV = nRT P in atm, V in Liters, n in moles, T in Kelvin R = 0.08206 (L*atm)/(mol*K)

Gas Laws (3) O a. State Boyles Law - for a fexced mass of gas at constant Temperature Volume vanes inversely with pressure P₁ V₁ = P₂ V₂. h A+ 1"  (Please type answer).

2. The form of the Ideal Gas Law that we used in class is pV = mRT, where p is absolute pressure, V is volume, R is the specific gas constant and T is absolute temperature in Kelvin (SI units) or Rankine (English traditional units). i. ii. iii. Starting with pV = mRT, use the definition of molar mass and derive an alternative form of the Ideal Gas Law: p = pRT Now use the definition of the specific gas constant to show that pV = nRuT Add these two additional forms of the Ideal Gas Law to your class notes for reference throughout the semester.

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The gas nitrous oxide, N2O, is a dental anesthetic. a) Calculate the root-mean square velocity (ums ~ m/sec) of N,0(g) at a temperature of 27°C R = 8.31 (kg-m²) / (K-mol-sec2) Urms = [ Select ] m/sec 1 3RTK { MMkg b) Calculate the kinetic energy (KE ~ in joules) of a single molecule of dinitrogen monoxide with this root-mean square velocity (Urms)? KE = [ Select ] joules 2 KE = /2 mkg • Hrms

use the ideal gas law P=nRT/V for the TV^(gamma-1) derivation and PdV=nRdT-(nRT/P)*dP how to get the derivations by using  Algebra

1. Prove that 1 L = 1 x 19-3 m3 2. Calculate the number of moles of an ideal gas given the following: P = 743.3 Torr; V = 262.84 mL; T= 100°C; R = 8.314 Pa-m3 / mol·K (HINT: Use Ideal Gas equation (PV = nRT) and SI Units. %3D 3. Plot the following using MS Excel: a) Volume (mL) vs Pressure (kPa) b) 1/volume vs Pressure Given the following data: V (mL) P (kPa) 15 16 14 12 10 8 6 100 95 105 118 131 139 180

The average kinetic energy of the molecules a gas sample depends only on the temperature, T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed 3 RT rms speed = where R= 8.314 J/(mol-K) and M is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (kg-m/s3). What is the rms speed of N, molecules at 365 K? rms speed: m/s What is the rms speed of He atoms at 365 K? rms speed: m/s