The correct answer is 0.011330374846536 Hope this helps ;D
Answer:
Explanation:
The pressure of a gaseous mixture is equal to the sum of the partial pressures of the individual gases:
Σ
![= P_1+P_2+P_3+...+P_n](https://tex.z-dn.net/?f=%3D%20P_1%2BP_2%2BP_3%2B...%2BP_n)
The prompt is trying to confuse you, but it actually tells us the pressure of the mixture to be 1 atm, but this can be converted to torr. Furthermore, we are informed only three gases are in the mixture: diatomic nitrogen, diatomic oxygen, and carbon dioxide:
![P_g_a_s=1 \ atm = 760 \ torr= P_N_2+P_O_2+P_C_O_2\\760 \ torr = 582.008 \ torr + P_O_2 \ + 0.285 \ torr](https://tex.z-dn.net/?f=P_g_a_s%3D1%20%5C%20atm%20%3D%20760%20%5C%20torr%3D%20P_N_2%2BP_O_2%2BP_C_O_2%5C%5C760%20%5C%20torr%20%3D%20582.008%20%5C%20torr%20%2B%20P_O_2%20%5C%20%2B%200.285%20%5C%20torr)
Solve for Po2:
![P_o_2=(760-582.008-0.285) \ torr = 177.707 \ torr](https://tex.z-dn.net/?f=P_o_2%3D%28760-582.008-0.285%29%20%5C%20torr%20%3D%20177.707%20%5C%20torr)
Thus, the partial pressure of diatomic oxygen is 177.707 torr.
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Explanation:
Both cohesion and molecular interchange contribute to liquid viscosity. The impact of increasing the temperature of a liquid is to reduce the cohesive forces while simultaneously increasing the rate of molecular interchange. The former effect causes a decrease in the shear stress while the latter causes it to increase.
temperature?
The viscosity of liquids decreases rapidly with an increase in temperature, and the viscosity of gases increases with an increase in temperature. Thus, upon heating, liquids flow more easily, whereas gases flow more sluggishly.
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