M6L1 Determination of Ideal Gas Law Constant 2022

Find moles of hydrogen gas produced and ideal gas constant.

Required information Problem 13.012 - DEPENDENT MULTI-PART PROBLEM - ASSIGN ALL PARTS NOTE: This is a multi-part question. Once an answer is submitted, you will be unable to return to this part. A gas mixture consists of 2 kg of O2, 3 kg of N2, and 5 kg of CO2. Problem 13.012.c Molar Mass and Gas Constant Determine the average molar mass and gas constant of the mixture. The universal gas constant is Ru= 8.314 kJ/kmol-K. The average molar mass is kg/kmol. The gas constant of the mixture is kJ/kg-K.

how would u solve this? this is a non-graded practice

1.A. In testing for the ideal gas law, a student not well-familiarized with the order of the procedures in the experiment, unwarily measured and recorded the temperature of the water in the beaker at 23°C before, instead of after, doing the reaction. The measured h will ________. a. increase b. indeterminate c. still be the same d. decrease 1.B. The same situation but during the course of the experiment, the lab air conditioning failed, considerably heating the water. The measured h will ____?

What to do: Check (V) the column that best describe IDEAL GAS and REAL GAS. TABLE 2. Differences between real gas and ideal gas. IDEAL GAS REAL GAS DESCRIPTION 1. It really exists in the environment. 2. Does not really exist in the environment and is a hypothetical gas. 3. Intermolecular forces of attraction. 4. No intermolecular forces of attraction. 5. No definite volume. 6. Definite volume. 7. Elastic collision of particles. 8. Non-elastic collisions between particles. 9. High pressure 10. Less pressure 11.Obey all gas laws under all conditions of temperature and pressure. 12.Obey gas laws only at low pressures and high temperature.

B. Direction: Complete the following table and use the Ideal gas equation to calculate pressure, volume, number of moles, and temperature of a gas. Express your final answer in two (2) decimal places and show your solution below the table. Pressure (P) Volume (V) Теmрerature (T) Moles (1n1) 1. 5.00 atm 25.00L 273.15 K 2. 0.55 L 308 K 0.50 mol 3. 20.00 aun 30.00 L 25.30 1Iol 4. 15.00 atm 370.00 K 3.00 mol 5. 10.50 L 280.00 K 10.00 mol

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 ? ? ? ? ?

Pls do fast and i will give like for sure Try to give solution in typed form

Option for blank one: (decrease, stay the same, increase) Option for blank two: (Avogodro's, Boyle's, Charle's)

Help please with this factors

please solve part b question 4 ASAP just have less time and do not give wrong answer please

#1

B. Direction: Complete the following table and use the Ideal gas equation to calculate pressure, volume, number of moles, and temperature of a gas. Express your final answer in two (2) decimal places and show your solution below the table. Pressure (P) Volume (V) Temperature (T) Moles (n) 1. 5.00 atm 25.00L 273.15 K 0.55 L 308 K 0.50 mol 3. 20.00 atm 30.00 L 25.30 mol 4. 15.00 atm 370.00 K 3.00 mol 5. 10.50 L 280.00 K 10.00 mol 2.

Sample exercises  (21) use Dalton's Law (23) use molar mix of gas mixture

Aktiv Chemistry X 8 https://app.101edu.co Portal D2L D2L Ch. 1 Introduction -... Aktiv Chemistry Connect-Bio Google Docs CG Grade Calculator .... R Point Grade Calcula Question 19 of 25 What is the volume in liters of 5.60 moles of CO2 at standard temperature and pressure (STP)?

Use molar mix of gas mixture

g uis proulem Part A - Relating Mole Fractions and Partial Pressures A 4.0-L vessel containing N2 at STP and a 2.0-L vessel containing H2 at STP are connected by a valve. If the valve is opened allowing the two gases to mix, what is the mole fraction of hydrogen in the moture? O 0 034 O 0.96 O 0.33 O 0.50 O 067 Submit Request Answer rovide Feedback

Please calculate pressure change (kpa), pressure change (Atm), average temperature (c) and average temperature (k) for all 4 trials

1. a. Ideal gas conditions are temperature and pressure. The assumption(s) in the kinetic molecular theory that is valid at this temperature is Blank 3: check the boxes that apply. High (blank 1) Low (blank 1) High (blank 2) Low (blank 2) Assumption (i) (blank 3) Assumption (ii) (blank 3) Assumption (iii) (blank 3)

Part A & B

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

Give good solution ASAP Thanks

Let's Find Out: About common conditions Let's Do It This Way: Identify which of the following describes Charles' Law. Put a check if it does, put a cross if it does not. Charles' Law 1. Lungs Air trapped in syringe Heating aerosol Inflating a balloon Inflated balloon 2. 3. 4. 5. Spraying aerosol Pressure cooker Deflated tire 6. 7. 8. Baking bread Hot air breeze 9. 10. Exhaling Ping-Pong Tires 11. 12 13. Placing a balloon in liquid nitrogen Hot air balloon 14. 15

1. calculate the volumetric analysis for Nitrogen in % given the ff Constituent Percentage Oxygen 23.14% Nitrogen 75.53 % Argon 1.28% CO2 0.05%

Please complete the following three graphs. Include proper axis, labels, and complete sentences where explantation(s) is required.

Determine-Molar-Volume-of-Gas (1) - Word ilings Review View Help O Tell me what you want to do 三 外|T AaBbCcDc AaBbC AaBbCcC AaB AABBCCD AaBb- AaBbCcDc I Normal T No Spac. Heading 1 Heading 2 Title Subtitle Subtle Paragraph Styles Table 3: Molar Volume - 2 trials Information Trial 1 Trial 2 Atmospheric Pressure" (mmHg) Mass of Mg Ribbon (g) Volume of H2 gas collected (mL) Temperature of H2 gas (°C) Temperature of Water Bath (°C) Vapor Pressure of Water (mmHg) *Use the atmospheric pressure given 756.14 756.14 0.0342 g 0.0350 g 36.5 36.5 21.2 21.2 21.2 21.2 18.7 18.7 Calculations A. Use the atmospheric pressure and the vapor pressure of water to determine the pressure of the hydrogen gas you collected (in atmospheres, atm). B. Use the combined gas law with your calculated pressure, measured temperature and measured volume to determine the volume of the hydrogen gas at STP. C. Calculate the moles of magnesium ribbon used. DELI

Trying to solve #1

What amount of pressure do you think the nitrogen contributed to the final total pressure? Explain your reasoning.

This is the data sheet for Molar mass of vapor3; 1. Unknown Liquid #: N/A 2. Mass of flask + cap + rubber band 56.45 g 97 3. Temperature of boiling water °C 4. Barometric Pressure 755.7 mmHg 5. Mass of flask + rubber band + cap + condensed vapor 57.88 6. Mass of condensed vapor What is the mass of condensed vapor? 1.34g O 93 O 143g O751.5 * Previous Next beatsoudio

For each set of values, calculate the missing variable using the ideal gas equation.   ? ? ? ? Set 1 264.5 kPa 1.69 L 36.1 ∘C ?1 Set 2 302 kPa 2382 mL ?2 3.23 mol Set 3 ?3 0.0250 m3 288 K 1.08 mol Set 4 104 kPa ?4 303 K 5.26 mol           ?1=  _________________ mol                         ?2= _________K ?3=________________kPa ?4=_________________L

please solve part d question 4 ASAP just have less time and do not give wrong answer please