pressure -- Torr which is equivalent to mmHg, Pascals or kPa, atmospheres, psi, inches Hg Volume -- usually liters Temperature -- Kelvin or Celsius which must be converted to Kelvin to be used in any gas law equations
Pressure, volume and temperature, and moles of gas are the four principal variables to describe a gas (for example, see related questions on Ideal Gas Law and others). The standard units are: Pressure: atmospheres (atm) Volume: liters (L) Temperature: Kelvin (K) Number of moles are measure in, well, moles.
Length: metreMass: kilogram Volume: litre temperature: Kelvin.
These are the corresponding units, if that's what you mean: mass: kilogram volume: cubic meter temperature: kelvin
The pressure and volume are inversely proportional. If you double one, the other will be reduced by 1/2 (as long as the temperature is constant). Boyles law states: P1V1/T1= P2V2/T2 In English that means, pressure times volume divided by temperature in the first "state" will equal to pressure times volume divided by temperature in the second state. Temperatures are all converted to degrees kelvin. So, calculate the pressure, temperature and volume of a quantity of a gas, change one of the variables of that quantity of gas for the second state and the other values will change to maintain equality. See the Related Question link to the left of this page. = "How do you solve an Ideal Gas Law problem?" =
PV=nRT T=PV\nR Convert units to SI units. T=[1.4*10^5 Pa] [1.21*10^-3]\0.58*8.314 T=348.39K
The question cannot be answered because there are no units given for the pressure not temperature.
The scale divisions indicate the value of measuring units of volume, temperature, pressure, etc.
You must know Pressure, and Volume , and Temperature when making accurate measurements of Gas quantity. Most of the world measures gas pressure in KiloPascal, volume in Cubic Metre, and temperature in degrees Centigrade . It is essential to use all Metric units Or all Imperial units, but Imperial units are only used by the USA now. The volume of all gases, changes with change of pressure and also with change of temperature. That is why you must measure all 3 units referred to .
Pressure, volume and temperature, and moles of gas are the four principal variables to describe a gas (for example, see related questions on Ideal Gas Law and others). The standard units are: Pressure: atmospheres (atm) Volume: liters (L) Temperature: Kelvin (K) Number of moles are measure in, well, moles.
Temperature, Pressure, # of moles, volume of container. If you know any three of those you can find the remaning by equation PV=nRT, where P=pressure in atmospheric units, V=volume in liters, n=number of moles of the gas, R=universal gas constant (which, in this formula, is equivalent to .08206), and T=temperature in Kelvins (not centigrade, but kelvins).
ml litre
Length: metreMass: kilogram Volume: litre temperature: Kelvin.
liters
When the temperature is increased, the volume of a container gets larger, and vice versa. This can be found by examining one of the fundamental laws of gasses, the combined gas law. It states that the product of pressure and volume, divided by temperature yields a constant value: pV/T=k Where k is a constant with units of energy/temperature. Thus, in order for k to remain constant, temperature and volume must be varied inversely to one another.
Energy
The answer depends on the density of the substance because milliliters are units of volume and milligrams are units of mass. 150 ml of pure water at standard temperature and pressure have a mass of 150 mg.
Volume, Tempature, Pressure