A7.20 l container holds a mixture of two gases at 29 °c. the partial pressures of gas a and gas b, respectively, are 0.179 atm and 0.749 atm. if 0.200 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?

P(total) = 1.63 atm

Explanation:

Given data:

Volume of container = 7.20 L

Temperature = 29°C

Number of moles of third gas = 0.200 mol

Pressure of gas A = 0.179 atm

Pressure of gas B = 0.749 atm

Total pressure = ?

Solution:

According to the Dalton's law of partial pressure,

"The total pressure exerted by the mixture of gases is the sum of partial pressure of the individual gases"

P(total) = P₁ + P₂ + P₃ +Pₙ

First of all we will determine the pressure of third gas.

PV = nRT

P = nRT /V

P = 0.200 mol × 0.0821 atm.L. mol⁻¹. k⁻¹ × 302 K / 7.20 L

P = 5 atm. L / 7.20 L

P = 0.7 atm

P(total) = PA + PB + P₃

P(total) = 0.179 + 0.749 + 0.7

P(total) = 1.63 atm

35. a insulated cylinder of solid gold (k 310 kw/m-k) of radius v2 m and height 5 m is heated at one end until the temperature at each point in the cylinder is given by w(r, y, z) (30 z2)(2-(r2+ y2). determine the rate of heat flow across each horizontal disk given by z 1, z 2, and z 3, identifying which has the greatest rate of heat flow across it.

explanation: