It depends on temperature and pressure. Assuming 25.0ºC and 1.00 atmospheres then 125 g CO2 occupies 54.7 dm3.
The volume is 1,1 mL.
CO2(g)
density=mass/volume
The volume of ammonia is 19,5 L.
The volume of CO2 is 53,18 litres.
It depends on temperature and pressure. Assuming 25.0ºC and 1.00 atmospheres then 125 g CO2 occupies 54.7 dm3.
The volume is 1,1 mL.
CH4(g)+2CO2(g)->CO2(g)+2H2O(g) 44g CO2(g) is obtained from 16 g CH4(g) mole of CO2 g =22g CO2(g)*1mol CO2/44g CO2 =0.5 mol CO2 (g)
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.
CO2(g)
density=mass/volume
Density = mass/volume = 36/15 = 2.4 g per cm3
Mass = 15 gm Volume = 2 cubic cm Density = Mass/Volume = 15/2 = 7 and 1/2 or 7.5 g per cm3
You will mean 15 cc or cubic centimeter. The answer is 4g / cc ( 60 g divide 15 cc )
The volume of ammonia is 19,5 L.
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)