what is the volume of a balloon containing 50.0 moles of O2 gas at a pressure of 15.0 atm at 28 degrees
You can use the ideal gas law to solve this problem. First, convert 0.30 g of Cl2 to moles. Then use the molar volume of gas at STP (22.4 L/mol) to determine the volume of Cl2 gas needed. Convert this volume to milliliters (1 L = 1000 mL) to find the answer.
At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters. Therefore, a volume of 22.4 liters will be occupied by 1 mole of Cl2 gas at STP.
The Density of Neon at STP is: a 0.89994 mg/cm-3.
At standard temperature and pressure (STP), one mole of any ideal gas occupies 22.4 liters. Therefore, the volume of 1.9 moles of chlorine gas (Cl2) can be calculated as follows: 1.9 moles × 22.4 L/mole = 42.56 L. Rounding to the nearest option, the volume of 1.9 moles of Cl2 at STP is approximately 43 L.
The weight of chlorine gas can vary depending on the volume and temperature. At standard temperature and pressure (STP), the molar mass of chlorine gas (Cl2) is approximately 70.91 grams/mol. To convert this to pounds, you would divide the molar mass by the conversion factor of 453.592 grams per pound. Therefore, the weight of chlorine gas would be approximately 0.156 pounds per mol at STP.
You can use the ideal gas law to solve this problem. First, convert 0.30 g of Cl2 to moles. Then use the molar volume of gas at STP (22.4 L/mol) to determine the volume of Cl2 gas needed. Convert this volume to milliliters (1 L = 1000 mL) to find the answer.
At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters. Therefore, a volume of 22.4 liters will be occupied by 1 mole of Cl2 gas at STP.
At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 liters. Therefore, 5.60 liters of Cl2 at STP would be: 5.60 L / 22.4 L/mol = 0.25 moles of Cl2.
The density of hydrogen sulfide is 1.363 g/cm3.
The Density of Neon at STP is: a 0.89994 mg/cm-3.
STP stands for Standard Temperature and Pressure. At STP, the pressure of natural gas is 1 atm, and 1 mole of gas takes up 22.4 liters.
At STP (standard temperature and pressure), it is a diatomic gas, Cl2.
Ar (argon)
When 0.98L of HCl reacts with excess O2 at STP, it produces 0.49L of chlorine gas. This is because 1 mole of HCl produces 1/2 mole of Cl2 according to the balanced equation: 4HCl + O2 -> 2H2O + 2Cl2. At STP, 1 mole of any gas occupies 22.4L, so 1/2 mole of Cl2 occupies 11.2L.
At standard temperature and pressure (STP), one mole of any ideal gas occupies 22.4 liters. Therefore, the volume of 1.9 moles of chlorine gas (Cl2) can be calculated as follows: 1.9 moles × 22.4 L/mole = 42.56 L. Rounding to the nearest option, the volume of 1.9 moles of Cl2 at STP is approximately 43 L.
Chlorine is a gas at STP. Density is 71/22.4 = 3.17 g/L
Since you don't specify the conditions, I will use the current STP. At STP of 0oC (273.15 K for gases) and 100 kPa, the molar volume of a gas is 22.711 L/mol.4.50 mol Cl2 x 22.711 L/mol = 102 L Cl2, rounded to three significant figures.Just in case your teacher is using the older version of STP of 0oC (273.15 K for gases), and 1 atm, the molar volume of a gas would be 22.414 L/mol.4.50 mol Cl2 x 22.414 L/mol = 101 L Cl2, rounded to three significant figures.