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Density = Mass/Volume = 1350 g/ 100 ml = 13.5 grams per ml
volume = mass/density mass = (204.69-96.94) = 107.75 g density = 13.53 g/cm3 volume = 107.75g / (13.53 g/cm3) volume = 7.96 cm3
9.75 L
4 g of helium occupies 22.414 liters So, 0.8 g will occupy 4.483 liters
Molar mass of propane = 44 g/mole ... 100 / 44 = 2.727 moles one mole occupies 22.4 L at STP .... 22.4 x 2.727 = 50.91 L
If the density of mercury is 13.546 g per cm cubed, the volume occupied by 999 grams of mercury is 73.7 cubic centimeters. papadantonakis.com/images/d/d0/Chem_101_Lecture_Notes_6.pdf
Given:thermometer contains 20.4g of mercury density of mercury = 13.6 g/mL Density= mass/volume 13.6g/mL = (20.4g)/volume Multiply both sides by volume to get it out of the denominator: (13.6 g/mL) x Volume = 20.4g Now Divide both sides by 13.6 g/mL to isolate volume and you have your answer: volume= 20.4g/13.6 g/mL volume = 1.50 mL Hope that helps!
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)
The volume of CO2 is 53,18 litres.
450/19=24.5mL
mercury
35.2 / 1.6 = 22 mL
To calculate the density of mercury, we need to use the formula: Density = Mass / Volume Given that the mass of 15.0 mL of mercury is 204 g, we can convert mL to L by dividing by 1000: Volume = 15.0 mL / 1000 mL/L = 0.0150 L Now we can calculate the density: Density = Mass / Volume = 204 g / 0.0150 L = 13600 g/L Therefore, the density of mercury is 13600 g/L.
I consider this question as erroneous.
4 g (1 mole) of helium will occupy 22.414 liters. So, 15 g will occupy 84.05 liters
It is approx 1.36 g/mL.
Density = Mass/Volume = 1350 g/ 100 ml = 13.5 grams per ml