1.54 atm is 156kPa
When using the pressure formula. PV=nRT. Pressure(in ATM) x Volume(in liters)=n(number of moles) x R(gas constant=.0821) x Temperature(in kelvins)If you are given pressure in kpa you have to convert to ATM
(ATM x 101.325 = kPa). So, 1.62 ATM x 101.325 = 164.146 kPa
1.30 atm is 131.7 kPa
1,013.25 kPa
104.4
151.98 kPa is about 1.5 ATM
When using the pressure formula. PV=nRT. Pressure(in ATM) x Volume(in liters)=n(number of moles) x R(gas constant=.0821) x Temperature(in kelvins)If you are given pressure in kpa you have to convert to ATM
0.975 ATM = 98 791.88 Pa = 98.791 88 kPa
84 x 0.00986 = 0.82824 atm=========================Explanation:'Standard' atmospheric pressure is defined as 101.325 kPa.84 kPa is 84/101.325 = 0.82902 standard atm pressure
1 ATM = 101325 Pascals 1 Pascal = 1/101325 ATM
kPa, kiloPascal, is a metric unit of pressure. One atmosphere, the atmospheric pressure at sea level, is about 101.325 kPa, so 1656 kPa divided by 101.325 kPa is your answer.
10.13kPa is 0.1 ATM
By definition 1 ATM = 101.325 kPa, so the gas pressure meant was: 0.1000 ATM .15 apexx
20.26 kPa is 0.2 ATM
Each liquid has a different boiling point; 101,3 kPa is he standard atmosphere pressure (atm).
(ATM x 101.325 = kPa). So, 1.62 ATM x 101.325 = 164.146 kPa
1.30 atm is 131.7 kPa