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You need to get the Moles of CO2 first. 9.3 g. CO2/44 g CO2= .211 mol
Then just put it into the ideal gas law at STP. PV=nRT
1.0 ATM x P = (.211 mol) (.08206) (273.15 k)---->"Plug and Chug"
P = (.211 mol) (.08206) (273.15 k) / 1.0 ATM
P= 4.7 L ---> 4,700 mL
Wiki User
∙ 14y ago
Wiki User
∙ 12y agoUse the ideal gas law: PV=nRT
P= 1.00 ATM
V= 6.2 L
n= # of moles
R= .0821 (constant)
T= 273 K
1.00(6.20)=n(.0821)273
n= .277 moles CO2
Wiki User
∙ 12y agoAccording to Hyperphysics, at STP, carbon dioxide gas has a density of 0.001977g/mL
Divide the given mass by the known density.
6.5g / 0.001977g/mL = 3287.8mL*
*With correct significant figures, the answer should be rounded to 3300mL
Wiki User
∙ 12y ago(CO2)= 44 g/mol =molar weight
6.5g =mass
1L=1000ml
1mole=22.4L
n=m/mw 6.5g/44g/m=0.148mol CO2 = ( 0.148mole) (22.4L/1mole) (1000ml/1L) =3310ml
Wiki User
∙ 6y agoThe volume of carbon dioxide is 3 288 mL.
Wiki User
∙ 11y ago6.23 moles x 44 grams/mole = 274.12 grams
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Which sample is most likely to take the shape of and occupy the total volume of its container?
CO2(g)
What volume will 125 g of CO2 occupy?
It depends on temperature and pressure. Assuming 25.0ºC and 1.00 atmospheres then 125 g CO2 occupies 54.7 dm3.
Enteric Bacteria commonly occupy the human intestine and primarily produce what?
co2 and h2 gases
What is the volume of 10 grams of CO2 at STP?
5126 cm3
What volume of CO2 gas will be evolved at ntp by heating 7.3 g of magnesium hydrogen carbonate?
The volume is 1,1 mL.
Which sample is most likely to take the shape of and occupy the total volume of its container?
CO2(g)
What volume will 125 g of CO2 occupy?
It depends on temperature and pressure. Assuming 25.0ºC and 1.00 atmospheres then 125 g CO2 occupies 54.7 dm3.
How many grams of CO2 will occupy a volume of 2000L at an absolute pressure 0f 3 ATM and an absolute temperature of 300K?
The mass is 10 727 kg.
What volume does 22g of CO2 at STP occupy?
This depends on the temperature and the pressure. At standard temperature and pressure 1 mole will occupy 22.4 L, so multiply... 22.4 x 2.22 = 48.728 L at STP.
What is the volume in milliliters occupied by 89.2g CO2(g) at 37oC and 737 mmHg?
The volume of CO2 is 53,18 litres.
How many grams of carbon dioxide will occupy a volume 500.0 ml at STP?
We know that one mole of any gas at STP occupies 22.4 liters of volume. We also know that one mole of carbon dioxide is 44.01 grams of CO2. If there are 44.01 grams of this gas in 22.4 liters at STP, then there will be about 0.98 grams of CO2 in half a liter (500 ml) of the gas at STP.
Enteric Bacteria commonly occupy the human intestine and primarily produce what?
co2 and h2 gases
Why dry ice CO2 floats?
CO2 floats because its density is less then water. Anything will float if its density is less then water. That is; when a certain volume of CO2 (or anything else) weighs less then the same volume of water.
What is the volume of a sample of co2 at stp that has a volume of 75.0 ml at 30.0c and 91 kpa?
61ml
What volume will 10.0 grams of carbon dioxide occupy at 27.0 degree Celsius?
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.
What is the volume of 10 grams of CO2 at STP?
5126 cm3
What is the calculated molar volume of the dry CO2?
22.4 liters at STP
