14 The followeing four gas samples were all held at 1.00 atm of pressure: A nitr

Question

14 The followeing four gas samples were all held at 1.00 atm of pressure: A nitrogen gas sample at -100°ca trege gas sample at .100 ee an argon gas sample at-100 and an argon gas sample at .100°c. which gas sample has the highest mass density A Arat +100°c &N; at -100 N at 100°c D. Ar at-100°C 15 A 4,00 mol quantity of O, was combined with a 2.00 mol quanty of Ny Which of the following is the partial pressure of N2 if the mixture is held at STP? A 667 Torr B 507 Torr C 333 Tor D. 253 Tor 16 What is the maximum mass of O2 that can be formed from the decomposition of 0.840 moles of H202 via the following reaction? 2H202 2H20 +02 FW (E/mol) H202 34.01 H0 18.01 02 32.00 A 53.88 B 0.420 C 1.68g D. 13.4g Form 8

Explanation / Answer

1. From gas equation, density = constant x (Molar mass/Temperature)

So option A must be the answer.

2. Pressure at STP will be 760torr

So partial pressure of N2 = mole fraction x P = (1/3) x 760 =253 torr

So option D is the answer.

3. For 2 mole of H2O2, 1 mole of O2 produces. So for 0.840 moles, 0.840/2 moles of O2 will produce. So weight will be 0.420 x 32 = 13.44g

So option D

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