CHM 101L M6 Ideal Gas Law Constant Lab Report Complete

Pls help ASAP. Pls circle the final answer and place give proper units and decimals.

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 =

H2O2 mass %

Need to calculate R and the average of R for each determination.  Gas law constant data Determination 1 2 3 4 5 mass Mg, g 0.0196 0.0168 0.0196 0.0166 0.0206 moles Mg, mol 0.0008064 mol 0.00069121 0.0008064 0.0006830 0.0008476 initial syringe volume, mL 0.93 0.91 1.09 1.05 1.01 final syringe volume, mL 21.09 18.47 21.47 18.40 22.38 volume H2, mL 20.16 17.56 20.38 17.35 21.37 barometric pressure, torr             760 T 760T 760T 760T 760T vapor pressure water, torr 22.4 T 22.4 T 22.4 T 22.4 T 22.4 T corrected pressure, atm* 0.970526 0.970526 0.970526 0.970526 0.970526 temperature, °C 24 C 24 C 24 C 24 C 24 C temperature, K 297  K 297  K 297  K 297  K 297  K R, mL*atm/K/mol ? ? ? ? ? average R, mL*atm/K/mol ? ? ? ? ?

ials-CHEM-T0 O Question 9 of 15- Unit 2 m/sac/4768186%2#/4768186/8/-1 ssignment Score: O Hint Check Answer 72% Resources puestion 9 of 15 A balloon filled with helium has a volume of 41.1 L at 297 K. What volume will the balloon occupy at 265 K? V = V 3:33 45 backspec 96 24 4. %23 5n 6.

IReview I Co (Pages 420- 425) Section 10.4 while Part A A syringe containing 1.66 mL of oxygen gas is cooled from 90.9 °C to 0.4 °C. What is the final volume Vf of oxygen gas? ΑΣφ ? DA mL Request Answer Submit Provide Feedback

I need help with both parts of the question please

Kinetic Energy: Question #1 The gas nitrous oxide, N2O, is a dental anesthetic. a) Calculate the root-mean square velocity (ums ^ m/sec) of N20(g) at a temperature of 27°C R = 8.31 (kg-m2) / (K-mol-sec²) Urms = [ Select ] m/sec 3RTK 13 {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

Calcium Chloride Ammonium Chloride   Trial 1 Trial 2 Trial 3 Trial 1 Trial 2 Trial 3 Mass of water 100g 100g 100g 100g 100g 100g Mass of salt 5.36g 10.28g 15.10g 5.29 10.43 15.31 Moles of salt             Initial T 21.0 21.0 21.0 20.0 20.0 20.0 Final T 29.6 36.2 43.5 17.1 13.2 10.1 ΔT 8.6 15.2 22.5 -2.9 -6.8 -9.9 ΔH(Joules)             ΔH(kj/mol)

Pressure (Atm) 25 20- 15 ▬▬▬ 10- 5 State X 2 State Y A plot of pressure-volume isotherms for an ideal gas at two different temperatures is shown below. In which of these processes would AS(gas) > 0? T = 546 K -T=273 K State Z Volume (L) A) X→ Y B) Y → Z C) Z → X D) X → Y and Y→ Z E) Y→ Z and Z → X

Please help me out with this ?? complete Thanks in advance

STARTING AMOUNT + 78°F Near record @ 2 W S # "** 3 E D C $ 4 R L 0.98692 % 5 T ADD FACTOR *(~) G 2.70 10⁰ Q Search 40 6 Pa V B 0.00355 1 & H 7 Convert 2.70 atm to torr psi 101.325 C Question 17 of 33 N 20.3 C+ 8 J 14.70 1000 mm Hg ( T M ANSWER 9 kPa K 0.001 1.01325 ) O bar O 2050 1.01325 x 10 P RESET # torr 760

Trial #1 Trial #2 nhnaun #15 Unlhraun #15 Volatile liquid Mass of flask 117,386 117.386 g Tslom oub Mass of flask and condensed sample after cooling 118.758 119.203 g Mass of condensed sample 1.372 1.817 g Temperature of gas in hot water bath 100.0 °C 99.D °C 373.0 372.1 K K Atmospheric pressure 755.6 _mm Hg 755.6 mm Hg 0.7942 atm atm Volume of flask 275.2 mL 275.2 mL 0.2752 0.2752 L Moles of sample pV=nRT (using the ideal gas law) (Show set-up) mol mol Molar mass of sample, experimental (using moles and mass of sample) g/mol g/mol Average molar mass, experimental g/mol Actual molar mass using molecular formula from page 216 mdar maxs claer Percent error in molar mass g/mol 3 possibe) % 219

Use the combined gas law by plugging in the numbers into it and solve the missing part

Need help finding correct concentrations for thermal volume expansion

P 1) Pinte X A ACTIVITY X EX_FjXNtRGOvhgYzM_rMIZzEwnvfJ17evaEjsK94/edit# Last edit was 2 minutes ago 11 BIUA 田回▼ 1三 ニ=,E▼E ... .. 1. Calculations A. Direction: Calculate the given problems and use the gas laws to determine pressure, volume, or temperature of a gas under certain conditions of change. Show your solutions. Encirce your final answer. 1. The gas inside the tire has a volume of 20.00 L at a pressure of 5.00 atm. Calculate the pressure of the gas if its volume is reduced to 10.0 at the same temperature. 2. If 150.00 mL of N2 gas was collected at 760 torr, what is the new volume of the gas when the pressure is compressed to 740 torr at the same temperature? 3. At 300 K, the given amount of fluorine gas has a volume of 30.0 L. What will be the temperature if the gas occupies a volume of 25 L at constant pressure? 4. A certain gas sample has a volume of 40.00 L at 273 K. At constant pressure. the volume increase to 50 00 L What will be the final temperature of the gas? 5 At…

Perssure (mmiay 7.5 A=025 9.4 13=6.34 12.5 バ.8 423D0.5 37.7 Nelct the data anove on the Daph below. 40 Boyles. law 35 30 25 ス6 15 10 02 0.4 0S 10 1/volumme(/m 3.

Given the following data, from the Molar Mass of CO2 Lab: Mass (before rxn): test tube + HCI(aq) + stir bar + capsule 26.042 g Mass (after rxn): test tube + HCl(aq) + stir bar + capsule 25.693 g Volume of water displaced from squirt bottle 139 mL Temperature of CO2(g) 293.6 K CO2(g) pressure 0.986 atm Calculate the density of CO2(g) in g/L. Type answer:

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