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Water's accepted density is 1.00 g/mL at standard temperature and pressure so depending on temperature the 1057 grams of water will occupy just about 1057 mL.
The answer is 0,19 moles.
What you need to know to work this out is that:- Moles of gases at standard temperature pressure (With P and T constant) are proportional to the volume they occupy, divided by their specific gas constant.
any increase in temperature will cause gas to occupy a larger volume, any decrease will shrink the volume to a point it becomes liquid. further decrease will cause a solid to form. at -273 degrees celsius everything is solid
It depends on temperature and pressure. Assuming 25.0ºC and 1.00 atmospheres then 125 g CO2 occupies 54.7 dm3.
The volume is 13,64 L.
At STP, 1 mole of gas occupies a volume of 22.4 liters. Thus, 4/5 moles of gas will occupy .8*22.4 liters.
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.
8. Two cubic meters of a gas at 30 degrees Celsius are heated at a constant pressure until the volume doubles. What is the final temperature of the gas? 60.
Water's accepted density is 1.00 g/mL at standard temperature and pressure so depending on temperature the 1057 grams of water will occupy just about 1057 mL.
The answer is 0,19 moles.
7.41 L
10 mg of 'standard' pure water, at standard temperature and pressure, occupy 0.01 mL of space.
What you need to know to work this out is that:- Moles of gases at standard temperature pressure (With P and T constant) are proportional to the volume they occupy, divided by their specific gas constant.
any increase in temperature will cause gas to occupy a larger volume, any decrease will shrink the volume to a point it becomes liquid. further decrease will cause a solid to form. at -273 degrees celsius everything is solid
The mass is 10 727 kg.
The volume is 16,85 L.