A gas cylinder contains 1.00 mol He, 1.90 mol Ne, and 1.10 mol Ar. If the total pressure in the cylinder is 2250 mmHg, what is the partial pressure of each of the components? Assume constant temperature. PHe= PNe=
PAr=

P_he = 562.5 mmHg

P_ne = 1068.75 mmHg

P_ar = 618.75 mmHg

Step-by-step explanation:

Formula for partial pressure is;

Partial pressure = mole fraction × total pressure

Mole fraction of Helium(He); x_he= 1/(1 + 1.9 + 1.1) = 1/4 = 0.25

Mole fraction of Neon(Ne); x_ne = 1.9/(1 + 1.9 + 1.1) = 1.9/4 = 0.475

Mole fraction of argon; x_ar = 1.1/(1 + 1.9 + 1.1) = 1.1/4 = 0.275

Thus;

Partial pressure of He;

P_he = 0.25 × 2250

P_he = 562.5 mmHg

Partial pressure of Ne;

P_ne = 0.475 × 2250

P_ne = 1068.75 mmHg

Partial pressure of Ar;

P_ar = 0.275 × 2250

P_ar = 618.75 mmHg

answer: two five pound bags one two pound

step-by-step explanation:

there are no figures how am i supposed to answer this question

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