A sample of hydrogen gas has a volume of 8560. mL at standard temperature and a pressure
of 1.50 atm. Calculate the number of moles of H, present in this gas sample.

5.26 moles

Explanation:

Given that:

Volume of hydrogen gas V = 8560mL

(since 1000 mL = 1dm3

8560mL = 8560/1000= 8.56dm3)

Standard temperature T = 25°C

Convert temperature in Celsius to Kelvin

(25°C + 273 = 298K)

Pressure P = 1.5atm

Number of moles of hydrogen = ?

Note that Molar gas constant R is a constant with a value of 0.0082 ATM dm3 K-1 mol-1

Then, apply ideal gas equation

pV = nRT

1.5 atm x 8.56dm3 = n x (0.0082 atm dm3 K-1 mol-1 x 298K)

12.84atm dm3 = n x 2.44atm dm3 mol-1

n = (12.84atm dm3 / 2.44atm dm3 mol-1)

n = 5.26 moles

Thus, there are 5.26 moles of Hydrogen, H present in this gas sample.

because u need two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei to form isotopes.

so since they all have the same shape? i mean maybe because m& m and reeses are both chocolates