The value of gas constant taken here is 0.0821 L*atm/K* mol , Temperature is 273+ 27 = 300K and molar mass of H2S is 34.1 g/mol
Calculate the density of H2S gas at 27.0 °C and 2.00 atm. Ο 0.0270 g/L Ο...
A 1.80−L vessel contains 4.70 g of a gas at 1.00 atm and 27.0°C. (a) Calculate the density of the gas in g/L. g/L (b) What is the molar mass of the gas?
8. A gas in a 2.00 L of ballon weigh 7.14 g at 2.00 atm and 27.0°C. What is the molar mass of the gas? .. nduced in greatest quantity (almost 45 million tons ner
The density of an unknown gas is measured to be 1.63 g/L at 1 atm and 27 °C. What could be the molecular formula for the gas? Ο Ο Ο Ο Ο
If 3.68 g Ar are added to 4.79 atm He in a 2.00 L cylinder at 27.0°C, what is the total pressure of the resulting gaseous mixture? Pool Pressure 2.7 atm Volume Amount of gas 1.5 mol Temperature 3236 How does the pressure change if the volume of a fixed amount of gas decreases at constant temperature?
calculate the density of O2 gas( in g/L) at 1.22 atm and 25 degrees C
Calculate the density of neon gas at 27.0 C and 705 mm of Hg in units of g/L.
Calculate the density, in g/L, of SF6 gas at 27°C and 1.500 atm pressure. O 3.38 * 10 g/L 2.96 g/L 22.4 g/L 8.9 g/L 3.38 kg/L
9. The density of a diatomic gas is 1.634 g/L at 1.50 atm and 40.0°C. Calculate the molar mass of the gas, and use the periodic table to identify the gas (10 pts)
Part A The density of a gas is 1.48 g/L at a temperature of 24 °C and a pressure of 0.783 atm. Calculate the molar mass of the gas.
Calculate the density, in g/L, of CO2 gas at 27°C and 0.50 atm pressure. 01. 1.12 g12 OII. 2.17 Kg/L O III. 0.89 g/L 1. 46.0 g/L V. 9.93 g/L QUESTION 11 Identify the compound with ionic bonds. O1.CH4 2. Li 3. PBr3 4. CsCI 5. SiO2