Given the following data in the Determination of Molar Mass of CO2 lab :Mass (before rxn): test tube + HCl(aq) + stir bar + capsuleMass (after rxn): test tube + HCl(aq) + stir bar + capsuleVolume of water displaced from squirt bottleTemperature of CO₂(g)26.611 g25.783 g144 mLCO2(g) pressureGas constant R293.6 K0.986 atm0.08206 L'atm/mol.Ka) Calculate the mass of CO₂(g) produced, in grams.b) Calculate the density of CO₂(g) in g/L.C) Calculate an experimental value for the molar mass of CO2 based on the mass,volume, and temperature data from the Determination of Molar Mass of CO₂ lab.d) Calculate the number of moles of CO₂(g) produced. Use the accepted valuefor the molar mass of CO2.

We are given experimental data for the reaction of the capsule with HCl(aq).

Given the following data in the Determination of Molar Mass of CO2 lab : Mass (before rxn): test tube + HCl(aq) + stir bar + capsule Mass (after rxn): test tube + HCl(aq) + stir bar + capsule Volume of water displaced from squirt bottle 26.611 g 25.783 g 144 mL Temperature of CO₂(g) 293.6 K 0.986 atm 0.08206 L atm/mol K CO2(g) pressure Gas constant R a) Calculate the mass of CO₂(g) produced, in grams. b) Calculate the density of CO₂(g) in g/L. C) Calculate an experimental value for the molar mass of CO₂ based on the mass, volume, and temperature data from the Determination of Molar Mass of CO₂ lab. d) Calculate the number of moles of CO₂(g) produced. Use the accepted value for the molar mass of CO2.

Given the following data in the Determination of Molar Mass of CO2 lab : Mass (before rxn): test tube + HCl(aq) + stir bar + capsule Mass (after rxn): test tube + HCl(aq) + stir bar + capsule Volume of water displaced from squirt bottle 26.611 g 25.783 g 144 mL Temperature of CO₂(g) 293.6 K 0.986 atm 0.08206 L atm/mol K CO2(g) pressure Gas constant R a) Calculate the mass of CO₂(g) produced, in grams. b) Calculate the density of CO₂(g) in g/L. C) Calculate an experimental value for the molar mass of CO₂ based on the mass, volume, and temperature data from the Determination of Molar Mass of CO₂ lab. d) Calculate the number of moles of CO₂(g) produced. Use the accepted value for the molar mass of CO2.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

34.0 mL of 6.0 M sulfuric acid solution is spilled on the floor. The acid is neutralized by pouring sodium hydrogen carbonate on the spilled acid. What is the volume, in L, of the carbon dioxide which is released at 25 deg. C and 1 atm? H2SO4 (aq) + 2NaHCO3 (s) --> Na2SO4 (aq) + 2H2O (l) + 2CO2 (g)
What is the pressure of a gas (in units of torr) in an open-end mercury-based (Hg density = 13,593 kg/m3) Manometer at sea level (Patompshere = 101,396 Pa) if the hydrostatic pressure head reads such that the level of the mercury exposed to the interior gas in the bulb is 51.5 mm above that of the mercury exposed to the atmosphere?
5 ral Aktiv Chemistry DeL D2L https://app.101edu.co + Ch. 1 Introduction -... Aktiv Chemistry Connect-Bio Google Docs - ▬▬▬ Q Search CG Grade Calculator .... What is the molar mass of an unknown gas with a density of 5.10 g/L at 3.00 atm and 45.0 °C? J R Point Grade Calcula... Question 16 of 21 (7 1 e Class Search Ho +
1. The compressibility factor Z = PV/nRT for O2 at -27.1°C and 537.1 atm is 1.50; at 147.4°C and 95.5 atm, it is 1.02. A certain mass of oxygen occupied a volume of 3.28 L at 147.4°C and 95.5 atm. Calculate the volume occupied by the same quantity of oxygen at -27.1°C and 537.1 atm. 2. The composition of a mixture of gases in percentage by volume is 20.5% nitrogen, 15.7% carbon monoxide, 37.8% water, and the rest sulfur dioxide. Calculate the density of the gaseous mixture at 39.8°C and 1.46 atm in grams/liter. Report your answer to the hundredths position.
← O Aktiv Chemistry Esc KU Portal D2 D2L https://app.101edu.co 457 Pantly sunny 1 X + Ch. 1 Introduction -... (@ 2 Aktiv Chemistry A chamber contains equal molar amounts of H2, N2, and O₂. If the total chamber pressure is 2.00 atm, then the partial pressure of H₂ is: #3 Connect-Bio Google Docs F3 $ 4 DII % 5 CG Grade Calculator .... R Point Grade Calcula... FS Question 28 of 30 Q FE A 6 * F7 & 7 PrtScn Class Sear Home 8
The pressure exerted on the gas entrapped in the syringe is proportional to the total mass on the platform. Make two plots. (i) Vol/mL vs. Total mass/g (ii) Vol/mL vs. 1/(total mass/g) If warranted, obtain a trendline and trendline equation. Comments in the results. Is Boyles Law obeyed? Explain.
High-pressure liquid chromatography (HPLC) is a method used in chemistry and biochemistry to purify chemical substances. The pressures used in this procedure range from around 500 kilopascals (500,000 Pa ) to about 60,000 kPa (60,000,000 Pa ). It is often convenient to know the pressure in torr. If an HPLC procedure is running at a pressure of 5.28×108 Pa , what is its running pressure in torr?
In an experiment carried out at a temperature of 4700C and a pressure of 100 atmosphere, 4.3g of a volatile liquid produced 30.6cm3of the gas. Calculate the molar mass of the liquid. (Molar gas constant, R= 8.314JKmol, molar gas volume at stp = 22400cm3, 1 atmosphere= 1.0 x 10 Nm-2)
The compressibility factor Z = PV/nRT for O2 at -38.6°C and 519.6 atm is 1.60; at 162.8°C and 105.4 atm, it is 0.99. A certain mass of oxygen occupied a volume of 2.10 L at 162.8°C and 105.4 atm. Calculate the volume occupied by the same quantity of oxygen at -38.6°C and 519.6 atm. place the answer rounded to the hundredths place Please provide only typed answer solution no handwritten solution needed allowed
Insects do not have lungs as we do, nor do they breathe through their mouths. Instead, they have a system of tiny tubes, called tracheae, through which oxygen diffuses into their bodies. The tracheae begin at the surface of the insect's body and penetrate into the interior. Suppose that a tracheae is 1.34 mm long with a cross-sectional area of 2.46 x 10-9m2. The concentration of oxygen in the air outside the insect is 0.794 kg/m3, and the diffusion constant is 1.26 x 10-5 m2/s. If the mass per second of oxygen is diffusing through a trachea is 1.66 x 10-12 kg/s, then find the oxygen concentration at the interior end of the tube.
The reaction is balanced: citric acid: 3NaHCO3 + C6H10O8 -> Na3 C6H7O8 + 3H2O + 3 CO2 Show the calculations required to determine quantities of sodium hydrogen carbonate and citric acid: (3NaHCO3 + C6H10O8) . Pressure is 100.800kPa, Temperature is 23 C and Volume is 784ml.
What final pressure must be applied to a sample of gas having a volume of 635 mL at 30.oC and 106 kPa pressure to permit the expansion of the gas to a volume of 302 mL at 30.oC? (223 kPa)