Question

QUESTION 2 0.5 A vessel contains a mixture of 27.8 grams of H2 (g) and 16.0 grams of CH4. If the total pressure inside the vessel is measured at 3.21 atm, the partial pressure of H2(g) must be atm. O C 6.03 0.217 O O O O QUESTION 3 0.5 p Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H2 (g) In an experiment, 201 mL of wet Hy is collected over water at 27 °C with a total pressure of the water-hydrogen mixture of 748 torr. The vapor pressure of water at 27 °C is 26.74 torr. How many grams of Zn have been consumed? C 385 C 3.85 x 105 C 0.507 C 4.28 x 106 C 507

Answer 1

2)

Molar mass of H2 = 2.016 g/mol

Molar mass of CH4,

MM = 1*MM(C) + 4*MM(H)

= 1*12.01 + 4*1.008

= 16.042 g/mol

n(H2) = mass of H2/molar mass of H2

= 27.8/2.016

= 13.7897

n(CH4) = mass of CH4/molar mass of CH4

= 16.0/16.042

= 0.9974

n(H2),n1 = 13.7897 mol

n(CH4),n2 = 0.9974 mol

Total number of mol = n1+n2

= 13.7897 + 0.9974

= 14.7871 mol

Partial pressure of H2:

p(H2),p1 = (n1*Ptotal)/total mol

= (13.7897 * 3.21)/14.7871

= 2.99 atm

Answer: 2.99

Only 1 question at a time please