I wants the detail. 17. A student adds 0.1613 g of an unknown gas to a 125-mL fl

Question

I wants the detail. 17. A student adds 0.1613 g of an unknown gas to a 125-mL flask. If the student finds the pressure to 0 be 736 torr at 20.0°C, is the gas likely to be methane (CH), nitrogen (N2), oxygen (0), neon (Ne), or argon (Ar)? A. CH4 B. N2 C. Ne D. Ar E. 02 A gas mixture consists of equal masses of methane (molecular weight 16.0) and argon (atomic weight 40.0). If the partial pressure of argon is 200. torr, what is the pressure of methane, in torr? A. 80.0 torr B. 200. torr C. 256 torr D. 500. torr E. 556 torr 18.

Explanation / Answer

17)

Given:

P = 736.0 torr

= (736.0/760) atm

= 0.9684 atm

V = 125.0 mL

= (125.0/1000) L

= 0.125 L

T = 20.0 oC

= (20.0+273) K

= 293 K

find number of moles using:

P * V = n*R*T

0.9684 atm * 0.125 L = n * 0.08206 atm.L/mol.K * 293 K

n = 5.032*10^-3 mol

mass(solute)= 0.1613 g

use:

number of mol = mass / molar mass

5.032*10^-3 mol = (0.1613 g)/molar mass

molar mass = 32.05 g/mol

This is molar mass of O2

Answer: E

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