Using the ideal gas law: PV = nRT, and R = 0.08206 L·atm·mol-1·K-1 (see related link), we have:
Assuming you meant 10.0 moles and 4.5 atmospheres: (4.5 atm)*(V) = (10.0 mol)*(0.08206 L·atm·mol-1·K-1)*(200 K ), Solving for V is 3.6471 liters
Roughly 3.123 liters (at the same pressure). Nitrogen is 78.08% of dry air by volume. 3.123 liters of nitrogen at STP is about 0.14 moles, or just under 2 grams.
The volume occupied by 3 moles of nitrogen gas will be different, depending on the temperature and pressure of the gas.
Number of Moles = concentration * volume (in litres)
Molarity = moles of solute/Liters of solutionLiters of solution = moles of solute/MolarityLiters NaOH = 3.25 moles NaOH/2.5 M NaOH= 1.30 Liters NaOH=============
Molarity = moles of solute/Liters of solutionOr, for our purposes....,Liters of solution (volume) = moles of solute/MolarityVolume (liters) = 0.150 moles HCl/4.00 M HCl= 0.0375 liters = 37.5 milliliters======================
Because you're in STP conditions, you can use molar volume in a proportion. Molar volume is the volume one mole of an ideal gas will take up at STP: 22.4 liters/mole. To set up a proportion, think: if one mole of a gas occupies 22.4 liters, then 4.0 moles of a gas will occupy x liters.1 mole/22.4 L = 4.0 mole/X Lx = 44.8 liters
Molarity = moles of solute/Liters of solution ( 20.0 ml = 0.02 Liters ) moles of solute = Liters of solution * Molarity 0.02 Liters * 0.800 M MgCl2 = 0.016 moles MgCl2 -------------------------------
Pressure, volume and temperature, and moles of gas are the four principal variables to describe a gas (for example, see related questions on Ideal Gas Law and others). The standard units are: Pressure: atmospheres (atm) Volume: liters (L) Temperature: Kelvin (K) Number of moles are measure in, well, moles.
atmospheres
Molarity = moles of solute/Liters of solution Or, for our purposes, Moles of solute = Liters of solution * Molarity Moles Na2CO3 = 10.0 Liters * 2.0 M = 20 moles Na2CO3 --------------------------
Need to find moles NaCl. 526 grams NaCl (1 mole NaCl/58.44 grams) = 9.0 moles NaCl --------------------------------now, Molarity = moles of solute/Liters of solution or, for our purposes Liters of solution = moles of solute/Molarity Liters of solution = 9.0 moles NaCl/3.0 M = 3.0 liters in volume ---------------------------------
This is a mass-mole conversion problem and a gas law problem all rolled into one! First, let's figure out how many moles of CO2 we have. CO2 has 44 grams to the mole, according to the periodic table. If you set up a direct proportion with the given mass, 10.0g, you get 0.23 moles of CO2. Second, figure out what volume 0.23 moles of CO2 will occupy at standard temperature and pressure. Every gas occupies 22.4 liters of space at STP, so 22.4 liters x 0.23 moles = 5.15 liters at STP. Third, convert all temperatures to degrees Kelvin. 27 Celsius = 300 Kelvin, and 0 Celsius (from STP) = 273 Kelvin. Finally, use the gas laws. Set up a direct proportion between the STP volume and temperature and the given temperature, with the new volume as the unknown. Temperature and volume share a direct relationship: 5.15/273=x/300. Solving for x gets you 5.66 liters, which is the answer.