A 5.00 L container contains a mixture of N2 gas and O, gas only. The total pressure in the container is 38.6 atm when the temperature is 25.0 °C. What is the mass of O, in the container if the mole fraction of N, is 0.60 ? [Molar mass of: N2 = 28.01 g and O2 = 32.0 g] R = 0.0821 L.atm/mol.K O 101 g O 96 g O I need more information 151 g O 144 g

2. A tank was filled with 11 g of oxygen (O2), 87 g of nitrogen (N2) and 6 g of carbon dioxide(CO2). At 25°C the pressure of the tank was 5.8 atm. If the partial pressure of CO2 in the tank is x atm, what is the value of x?

11. A mixture of 1.00 g of H2and 1.00g of He is placed in a 1.00L container at 27C. Calculate the partial pressure of each gas and the total pressure in atm. 12. A 10.0L flask at 27C contains 6.0grams of H2, 15.2g of N2, and 16.8g of He. a. Calculate the partial pressure of each gas in atm. b. What is the total pressure?

What is the density of CH4 gas at 134 °C and at 737 mmHg? (1 atm = 760 mmHg) OA. 0.0290 g/L OB.3.73 g/L O c. 1.86 g/L OD.0.465 g/L OE. 0.932 g/L QUESTION 18 When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic equation is: OA AgNO3 (aq) + KI (aq) AgI (s) + KNO3(aq) OBAg+ (aq) + NO3¯ (aq) → AgNO3 (aq) OC. AgNO3(aq) + KI (aq) → AgI (aq) + KNO3 (s) D-Ag+ (aq) + NO3 (aq) → AgNO3 (s) OE Ag+ (aq) + I (aq) AgI (s) Hok Click Save and Submifto save and submit. Chick Sour All Austers to save all answUCTA.

Nitesh

What volume of CO₂ gas at 1.000 atm and 800 K could be produced by the reaction of 45.0 g of CaCO, according to the equation? CaCO3(s)→ CaO(s) + CO₂(g) (Molar Masses (g/mol): CaCO3 = 100.1, CaO = 56.1, CO₂ = 44.0; R = 0.0821 atm.L/mol.K) A. 34.8 L B. 29.5 L C. 14.8 L D. 9.84 L E. 2.46 L

2. A gaseous mixture containing 1.5 mol of Ar and 3.5 mol CO2 has a total pressure of 7.5 atm. What is the partial pressure of CO2?

59. A sample of gas isolated from unrefined petroleum contains 90.0% CH4, 8.9% C2H6, and 1.1% C3H8 at a total pressure of 307.2 kPa. What is the partial pressure of each component of this gas? (The percentages given indicate the percent of the total pressure that is due to each component.)

A commercial mercury vapor analyzer can detect, in air, concentrations of gaseous Hg atoms (which are poisonous) as low as 2× 10-6 mg/L of air. At this concentration, what is the partial pressure of gaseous mercury if the atmospheric pressure is 733 torr at 26° C? B torr at standard conditions 2.5× 10-10. 1.86x 10-7 torr at standard conditions 0.0015 torr at standard conditions 0.0013 torr at standard conditions

for this question. Sodium metal reacts with water to produce hydrogen gas according to the following equation: 2Na(s) + 2H,0(1)→2NAOH(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 759 mm Hg. If the wet H, mol. The vapor gas formed occupies a volume of 9.89 L, the number of moles of Na reacted was pressure of water is 17.5 mm Hg at 20 °C.