1 atmosphere pressure = 760 torr
655 torr / ( 760 torr / ATM) = 0.86184 ATM
If you're not sure whether to multiply or divide when doing conversions, do this:
655 torr . 1 ATM
------------ * ---------
1. . 760 torr
The formatting did not display exactly as I wanted it to appear
This is read like a fraction. Since 1 ATM = 760 torr, the numerator and denominator are equal, so it's like just multiplying by 1 and won't change the value.
The torr units in numerator/denominator cancel out, and the only unit remaining is atmospheres.
1 ATM= 760 torr
1 ATM/760 torr x 685 torr = 0.895 ATM
A unit of absolute pressure in the metric.ATA(s): Abbreviation for "Atmospheres Absolute", defines as the total pressure exerted on an object, by a gas or mixture of gases, at a specific depth or elevation, including normal atmospheric pressure.
The answers are Hydrogen and Helium.
Nothing. It's still a gas. The fizz when you open a can is carbon dioxide.Nothing happens. It has to be compressed to 5.13 atmospheres before it turns solid at -56.4°C.
88.9237 moles
.271 mol
600 Torr (1 atm/760 Torr) = 0.789 atmospheres ================
atmospheres A+
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
The pressure of each gas in a mixture is called the partial pressure of that gas.
The pressure is 39,8 torr.
Rigid container holds hydrogen gas at a pressure of 3.0 atmospheres and a temperature of 2 degrees Celsius. The pressure if the temperature is raised to 10 degrees Celsius will be 15 atmospheres based on the law of pressure for gas.
500 mmHg or 500 torr is a gas pressure approximately 66% of the standard sea level air pressure of 760 torr ... it is the air pressure one would find at an altitude of approximately 3km or 10000 feet ... at sea level, 500 torr would be considered a partial vacuum of 0.66 atm.
Boyle's law states that pressure is indirectly proportional to the volume. There fore as the pressure of a gas at 760 torr is changed to 380 torr, the volume will increase. Boyle's Law: P1 x V1 = P2 x V2 Rearranging leads to: P1 / P2 = V2 / V1 Substituting our values: 760 / 380 = V2 / V1 Thus the final volume will be twice the initial volume.
140 torr
The pressure is 172,84 atmospheres.
You have to convert the temperature to Kelvins, the volume to liters, and the pressure to torr. You use the combined gas law and solve for pressure. P1V1/T1 = P2V2/T2 P1 = P2V2T1/T2V1 P1 = (608 torr)(0.300 L)(323.15 K) / (310.15 K) (0.555 L) P1 = 342.42 torr I believe that if you are using the correct number of significant digits, you would write the answer as 342 torr.
0.2