What is the mass of 2.54 ml of H2 at 195 0
C and 850 mmHg?
V = 0.00254
T = 468.15
P = 1.1183
1 mole of H
R = 0.821
n = (1.1183 x 0.00254)/ ( 0.0821 x 468.15)
= 0.0000738 moles of H2 1 grams H2 is equal to 0.496061273489 mole
so 0.0000738 is = 0.0001487719439998 grams
Thanks for your patience.
how does .0000738=.00014877g ? for the very last step
If 0.49606 moles of H2 is 1g then 0.0000738 moles =?
= 0.0000738/0.49606 x 1 = .00014877
how did you calculate moles of H2?
Using the formula of Ideal gas laws.
mass = 1 mole of H
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