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How many milliliters of Cl2 gas must you have to obtain 0.30g at STP in chemistry?
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.
What volume will the Cl2 occupy at STP?
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.
What is the density of neon gas at STP?
The Density of Neon at STP is: a 0.89994 mg/cm-3.
The molar mass of a certain gas is 49 g. What is the density of the gas in gL at STP?
To find the density of a gas at standard temperature and pressure (STP), we can use the formula: density = molar mass / molar volume. At STP, the molar volume of an ideal gas is approximately 22.4 L. Therefore, the density of the gas with a molar mass of 49 g is calculated as follows: density = 49 g / 22.4 L ≈ 2.19 g/L.
What is the volume of 1.9 moles of chlorine gas (Cl2) at standard temperature and pressure (STP) 12 L 22.4 L 43 L 81 L?
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.
How many milliliters of Cl2 gas must you have to obtain 0.30g at STP in chemistry?
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.
What volume will the Cl2 occupy at STP?
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.
How many moles are in 5.60 L Cl2 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.
What is the density of H2S gas at STP?
The density of hydrogen sulfide is 1.363 g/cm3.
What is the density of neon gas at STP?
The Density of Neon at STP is: a 0.89994 mg/cm-3.
Density of natural gas at STP?
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.
State of matter of chlorine?
At STP (standard temperature and pressure), it is a diatomic gas, Cl2.
How many liters of chlorine gas can be produced when 0.98L of HCl react with excess O2 at STP?
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.
If the density of a noble gas is 1.783 gL at STP that gas is .?
Ar (argon)
The molar mass of a certain gas is 49 g. What is the density of the gas in gL at STP?
To find the density of a gas at standard temperature and pressure (STP), we can use the formula: density = molar mass / molar volume. At STP, the molar volume of an ideal gas is approximately 22.4 L. Therefore, the density of the gas with a molar mass of 49 g is calculated as follows: density = 49 g / 22.4 L ≈ 2.19 g/L.
What is the volume of 1.9 moles of chlorine gas (Cl2) at standard temperature and pressure (STP) 12 L 22.4 L 43 L 81 L?
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.
What is the density of clorine?
Chlorine is a gas at STP. Density is 71/22.4 = 3.17 g/L
