2.5 * 14.7 = 36.75 psi
/ 2.2046 = 16.67 kg per sq in
* 9.807 = 163.48 newton / sq in
/ 645.16 = 0.253 newton / sq mm
* 1,000,000 = 253,000 newtons / sq metre (pascals)
/ 1000 = 253 kPa
ATM x 101.3 = kPa
Kilopascals is a unit of pressure, not of atom count.
253.30 OR 253 ;p
2.5atm = 253.31kPa
2.7atm equates to 273.58kPa
11.5 atm is 1,165.2 kPa
506.625 kPa
1 atm = 101.325 kpa so 203.4 / 101.325 = 2.0074 atm
By definition 1 ATM = 101.325 kPa, so the gas pressure meant was: 0.1000 ATM .15 apexx
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.
The number of moles is 0,579.
Yes, at room temperature its vapor pressure is about 0.1 Pa (0.0001 kPa, 0.000001 atm.). Be carefull, vapor of Mercury is very toxic.
101.3 kPa = 1 ATM
1 atm = 101.325 kpa so 203.4 / 101.325 = 2.0074 atm
(ATM x 101.325 = kPa). So, 1.62 ATM x 101.325 = 164.146 kPa
1.30 atm is 131.7 kPa
151.98 kPa is about 1.5 ATM
1,013.25 kPa
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, 2.5 x 101.325 = 253.312 kPa
1 ATM = 101325 Pascals 1 Pascal = 1/101325 ATM
15.2 kPa is 0.1500123 ATM
10.13 kPa = .1 ATM
0.975 ATM = 98 791.88 Pa = 98.791 88 kPa