Lab Data Mass of magnesium (g) 0.016 Moles of magnesium (mol) 0.00066 Temperature of water (*C) 25.0 Temperature of water (K) 298.15 Vapor pressure of water (mmHg) 23.8 Barometric pressure (mmHg) 771.0 Observations the water was presenting gas conditions Volume of hydrogen gas collected (ml) 15.6 Volume of hydrogen gas collected (L) 0.0156 Pressure of hydrogen gas (mmtg) Pressure of hydrogen gas (atm) Moles of hydrogen gas produced (mol) please explain and solve

45. What is the partial pressure of methane in a container that contains 7.0 mol of methane, 5.0 mol of ethane, and 6.0 mol of propane when the total pressure is 100. mmHg? A) 65 mmHg B) 100 mmHg C) 28 mmHg D) 39 mmHg E) 33 mmHg

eq req < 1req For each of the following sets of volume/temperature data, calculate the missing quantity after the change is made. Assume that the pressure and the amount of gas remain constant. V=2.30 L at 22.0 °C V = 4.98 L at ? °C PC V = 120. mL at 281 K V = ? mL at 386 K mL V=49.7 mL at 37.0 °C V = ? mL at 357 K a. APR 30 b. C. Submit Answer 2 mL Retry Entire Group Show Hint tv [Review Topics] Ⓒ 9 more group attempts remaining [References] SENSA SPREC ********* Previous Next Save and Exit 3

%24 4+ # m w/ If someone takes a breath and the lungs expand from 4.5 L to 5.4 L in volume, and the initial pressure was 759 mm Hg, what is the pressure inside the lungs (in mm Hg) before any additional air is pulled in? IIO YA %23 2 5 7. 6 1

Binary compounds of alkali metals and hydrogen react with water to produce H2(g). The H2 from the reaction of a sample of NaH with an excess of water fills a volume of 0.475 L above the water. The temperature of the gas is 35 °C and the total pressure is 770 mmHg. Vapor Pressure of Water versus Temperature Temperature Pressure Temperature Pressure (mmHg) (°C) Part A Find the mass of H2 produced. ΜΕ ΑΣΦ m-29.12 ? g (°C) (mmHg) Submit Previous Answers Request Answer 0 4.58 55 118.2 5 6.54 60 149.6 × Incorrect; Try Again; 19 attempts remaining 10 9.21 65 187.5 15 12.79 70 233.7 20 17.55 75 289.1 Part B 25 23.78 80 355.1 30 31.86 85 433.6 Write a balanced chemical equation. Then find the mass of NaH that reacted. 35 42.23 90 525.8 40 55.40 95 633.9 ΕΧΕΙ ΑΣΦ ? 45 71.97 100 760.0 50 92.6 m = Submit Request Answer g

A constant pressure 1.00 L of oxygen gas at 27° c is cool to -5.0° c calculate the new volume in liters. 0.893L  0.45 L  0.560L  2.70 L

Calculate the volume of a gas in a system when 22.0 g of O2 (Molar mass = 32 g/mol) at a pressure of 12.0 atm is placed in a container at a temperature of 450K. R = 0.0821 L*atm/mol*K Egn PV= nRT O 2.12 L O 8.88 L O 4.24 L O 22.5 L Question 22 4 pts Calculate the density of a gas in a system when O2 (Molar mass = 32g/mol) is placed in a 1.0 Liter container at a pressure of 6.2 atm and at a temperature of 250K. R = 0.0821 L"atm/mol*K O 0.085 g/L

A 367 mL sample of Ar(g) at 25 ⁰C and a barometric pressure of 698 mmHg is passed through water at 25 ⁰C. What is the volume of gas when saturated with water vapor at same barometric pressure?(vapor pressure of water at 25 ⁰C = 23.8 mmHg) a. 420 ml b. 360 ml c. 120 ml d. 380 ml e. 240 ml

Calculate the theoretical amount (mols) of H2 gas that should be produced from the mass of Mg ribbon used:

What is the density (g/L) of 1 mole of argon gas at 50.5°C and 764 mmHg? (760 mmHg = 1 atm) O A. 7361 g/L B. 39.7 g/L O c.4.00 g/L O D.39.9 g/L O E. 1.51 g/L