15.2 kPa is 0.1500123 ATM
10.13 kPa = .1 ATM
20.26kPa is 0.2atm
151.98 kPa is about 1.5 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.
To find the volume of 2.5 mol of hydrogen gas, we can use the Ideal Gas Law equation: PV = nRT. We are given the pressure (152 kPa), temperature (-20.0 degrees Celsius which is equivalent to 253.15 K), and the number of moles (2.5 mol). We can rearrange the equation to solve for volume (V), V = (nRT)/P. Plugging in the values, V = (2.5 mol x 8.314 J/mol·K x 253.15 K) / 152 kPa = 3.51 L. Therefore, 2.5 mol of hydrogen gas will occupy a volume of 3.51 liters at -20.0 degrees Celsius and 152 kPa.
Each liquid has a different boiling point; 101,3 kPa is he standard atmosphere pressure (atm).
152 mm Hg is equal to 0,2 atmosphere.
The standard atmosphere (symbol: atm) is a unit of pressure and is defined as being equal to 101.325 kPa.
There are several units for used to indicate pressure. The SI unit is the Pascal (Pa). The English unit is psi which equals 6,891 Pa. A Bar is equal to 100 kPa. A Tor is equal to 1 kPa. An atmosphere (atm) is equal to 101.3 kPa.
15.20kPa is 0.15 ATM
20.26 kPa is 0.2 ATM
Percent means "out of 100", so 152% can be written as 152/100 And because 152 and 100 have a common factor, you can simplify the fraction further ... 152% = 152/100 = 76/50 = 38/25