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What reactant is limiting if 3000 cm3 of Cl2 at STP react with a solution containing 25 grams of NaBr?
Cl2 + 2NaBr => Br2 + 2NaCl One mole Cl2 reacts with 2 moles NaBr Cl2 = 71 NaBr = 102.9 Molar volume = 22.414 L/mole for ideal gas @STP 3L Cl2 = 3/22.414 = 0.1338 mole 25g NaBr = 25/102.9 = 0.2430 mole 0.1338 moles Cl2 requires 0.2676 moles NaBr for complete reaction The NaBr is the limiting reagent
How many atoms in 560cm3 of ammonia at stp?
To determine the number of atoms in 560 cm3 of ammonia at STP (Standard Temperature and Pressure), we first need to calculate the number of moles of ammonia present. The molar volume of a gas at STP is 22.4 L/mol, which is equivalent to 22,400 cm3/mol. Therefore, 560 cm3 is equal to 0.025 moles of ammonia. Next, we use Avogadro's number, 6.022 x 10^23 atoms/mol, to find that there are approximately 1.51 x 10^22 ammonia molecules in 560 cm3 at STP.
How many liters are in 4.50 moles of chlorine gas?
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.
How many moles of argon are found in a 5L sample of argon at STP?
At STP, 1 mole of any gas occupies 22.4 L. Therefore, in a 5L sample of argon at STP, there would be 5/22.4 moles of argon, which is approximately 0.223 moles.
A container with a volume of 564 L holds how many moles of air at STP?
1 mole of gas occupies 22.4 liters at STP. 564/22.4 = 25.18 moles (2 decimal places)
If a large balloon contains 224 liters of gas at STP then there is 100 mole of gas in the balloon How many moles of gas are in a balloon that is 560 liters at STP?
Using the ideal gas law, at STP (standard temperature and pressure), 1 mole of gas occupies 22.4 liters. Therefore, a balloon with 560 liters at STP would contain 25 moles of gas (560 liters / 22.4 liters/mole).
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 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 reactant is limiting if 3000 cm3 of Cl2 at STP react with a solution containing 25 grams of NaBr?
Cl2 + 2NaBr => Br2 + 2NaCl One mole Cl2 reacts with 2 moles NaBr Cl2 = 71 NaBr = 102.9 Molar volume = 22.414 L/mole for ideal gas @STP 3L Cl2 = 3/22.414 = 0.1338 mole 25g NaBr = 25/102.9 = 0.2430 mole 0.1338 moles Cl2 requires 0.2676 moles NaBr for complete reaction The NaBr is the limiting reagent
What is the density of Cl2 gas at STP?
what is the volume of a balloon containing 50.0 moles of O2 gas at a pressure of 15.0 atm at 28 degrees
How many atoms in 560cm3 of ammonia at stp?
To determine the number of atoms in 560 cm3 of ammonia at STP (Standard Temperature and Pressure), we first need to calculate the number of moles of ammonia present. The molar volume of a gas at STP is 22.4 L/mol, which is equivalent to 22,400 cm3/mol. Therefore, 560 cm3 is equal to 0.025 moles of ammonia. Next, we use Avogadro's number, 6.022 x 10^23 atoms/mol, to find that there are approximately 1.51 x 10^22 ammonia molecules in 560 cm3 at STP.
How many liters are in 4.50 moles of chlorine gas?
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.
What is the volume of 2.00 moles of chlorine (cl2) at STP to the nearest tenth of a liter?
At standard temperature and pressure (STP), one mole of gas occupies 22.4 liters. Therefore, the volume of 2.00 moles of chlorine (Cl₂) can be calculated by multiplying the number of moles by the molar volume: (2.00 , \text{moles} \times 22.4 , \text{L/mole} = 44.8 , \text{L}). Thus, the volume of 2.00 moles of chlorine at STP is 44.8 liters.
How many moles of methane are presentin 5.6L of the gas at stp?
0.25 moles
How many moles are contained in 16.8 L of Xe gas at STP?
16,8 L of Xe gas at STP is equivalent to 0,754 moles.
How many moles are present in 8.4 liters of nitrous oxide at STP?
8,4 liters of nitrous oxide at STP contain 2,65 moles.
How many moles of argon are found in a 5L sample of argon at STP?
At STP, 1 mole of any gas occupies 22.4 L. Therefore, in a 5L sample of argon at STP, there would be 5/22.4 moles of argon, which is approximately 0.223 moles.
