calculate the moles of hydrogen present in a 500cm³ sample of hydrogen gas at a pressure of 760 mm of Hg and 27⁰C
Answers
Chemistry
Secondary School
+13 pts
Answered
Calculate the number of moles of hydrogen(H2) present in a 500 cm3 sample of hydrogen gas at a pressure of 760 mm Hg at 27
Answer
3.9/5
Solution: The data given in the problem isP = 760mm of Hg = 1 atm V = 500cm3 T = 270C T = 27+ 273 = 300 K R = 82.1 cm3 K-1mol-1 number of moles of hydrogen (n) = ? According to ideal gas equation PV= nRT n = PV/RT = 1 atm X 500 cm3 /82.1 cm3 K-1mol-1 X 300 K n = 0.023moS
34
3.9
4.4/5
Answer: 0.02 moles
Explanation:
According to the ideal gas equation:
P = Pressure of the gas = 760 mm Hg = 1 atm (1 atm =760 mmHg )
V= Volume of the gas =
T= Temperature of the gas = 27°C = 300 K (0°C = 273 K)
R= Gas constant = 0.0821 atmL/K mol
n= moles of gas= ?
Putting in all the values, we get
Thus the number of moles of hydrogen present are 0.02.
Answer:
By ideal gas equation ,
PV = nRT
P = 760= 1 atm
V = 500cm³= 500 ml= 0.5 L
T=300K
n= ?
R= 0.0821
n= PV/RT
= 1*0.5/0.0821*300
= 0.02 moles