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

mass =

1 mole of H

R = 0.821

n = (1.1183 x 0.00254)/ ( 0.0821 x 468.15)

= 0.00284/38.435

= 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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