At STP, Standard Temperature and Pressure, one mole of gas takes up 24dm3 of volume. One mole of nitrogen weighs 14g, so in 888g there are 63.4 moles of nitrogen. This takes up a volume of 63.4 x 24 = 1522.3dm3.
56.1 L
PV=nRT (my Chemistry teacher taught me to pronounce it Pivvy equals Nert to remember the formula.)
set it up so that V=(nRT)/P
n= number of moles of CO2 --> convert 110g CO2 to moles (the answer is around 2.499 moles)
R= 0.0821 (liters X atm)/(mol X K)
T = 273.15K at STP
P= 1 atm
Plug all of those numbers into V=(nRT)/P and you get 56.1 L
Density of CO2 is 1.977 g/L at 1 atm and 0oC , so 88.4 g takes
88.8(g) / 1.977(g/L) = 44.7 L at 1 atm and 0oC .
At any other higher temperature this value should be corrected by multiplying the answer with the T(C)factor :
(273 + T(oC)) / (273)
Number of Moles= Mass/ RAM
n= 88/44
n=2
volume= 2/22.4
Volume=0.089286 dm3
{| |- | 0.089286
0.089286
|}
You find the answer by mulitplying the 8 moles by 22.4, L/mol, which is the volume of any one mole of gas at STP. So the answer is 179.2 L
At 25 0C and 1 atmosphere the molar gas volume is 24,465 litres.
The density of carbon dioxide at STP is 0,769 g/L.
22.41 liters.
456g
Dry ice is CO2. Molar mass CO2 = 44 g/mole. 1 lb is approx. 454 g thus this = 454 g x 1 mol/44 g = 10.3 moles of CO2. At STP, 10.3 moles x 22.4 L/mole = 231 liters.
There are several different possible reactions of Fe2O3 with CO, depending on temperature and ratio of reactants. The simplest is probably Fe2O3 + CO ==>2FeO + CO21.00 Kg x 1000 g/Kg x 1 mole Fe2O3/160 g = 6.25 moles Fe2O3 moles CO2 produced = 6.25 moles CO2 Volume CO2 at STP = 6.25 moles x 22.4 L/mole = 140 Liters
The volume is 102 mL.
The volume of CO2 is 53,18 litres.
Density of CO2 at STP = 44.01 g/mol divided by the 22.4 liters. 1.96 grams/Liter
Density: BF3 = 0.00276 g/cm3 (anhydrous gas)Volume: 0.155 (g) / 0.00276 (g/cm3) = 56.16 = 56.2 cm3 (gas volume at STP)
Dry ice is CO2. Molar mass CO2 = 44 g/mole. 1 lb is approx. 454 g thus this = 454 g x 1 mol/44 g = 10.3 moles of CO2. At STP, 10.3 moles x 22.4 L/mole = 231 liters.
Under these conditions, the volume will be directly proportional to the number of moles. And the number of moles varies with the number of grams. 110 g/30 g = 3.67, so there are 3.67 x more moles in 110 g as there are in 30 g. And the volume will be 3.67 x greater or 3.67 x 410 ml = 1503 ml = 1.5 liters (to 2 significant figures)
There are several different possible reactions of Fe2O3 with CO, depending on temperature and ratio of reactants. The simplest is probably Fe2O3 + CO ==>2FeO + CO21.00 Kg x 1000 g/Kg x 1 mole Fe2O3/160 g = 6.25 moles Fe2O3 moles CO2 produced = 6.25 moles CO2 Volume CO2 at STP = 6.25 moles x 22.4 L/mole = 140 Liters
.75
The volume of ammonia is 19,5 L.
Molar mass CaCO3 = 100.087 g/mol Moles CaCO3 = 152 g / 100.087 = 1.52 the ratio between CaCO3 and CO2 is 1 : 1 so we get 1.52 moles of CO2 At STP p=1 ATM and T = 273 K V = nRT / p = 1.52 x 0.0821 x 273 /1 = 34.1L
15.2 g CaCO3 / 100.1 g CaCO3 x 22.4 L (STP)=3.40 L
The volume is 102 mL.
0.00922 g of H2 gas will occupy approximately 0.100 L at STP
The volume of CO2 is 53,18 litres.
Density of CO2 at STP = 44.01 g/mol divided by the 22.4 liters. 1.96 grams/Liter