A30-liter volume of gas at 25°c contains 12 g of methane, 1 g of nitrogen, and 15 g of carbon dioxide. calculate (a) the moles of each gas present, (b) the partial pressure exerted by each gas, (c) the total pressure exerted by the mixture, and (d) the percentage by volume of each gas in the mixture. you may assume ideal gas behavior

Explanation:

Mass of methane gas = 12 g

Mass of nitrogen gas = 1 g

Mass of carbon dioxide = 15 g

Volume of the container ,V= 30 L

Temperature of the gases,T= 25°C = 298.15 K=

a) Moles of methane gas:

Moles of nitrogen gas:

Moles of carbon dioxide gas:

b) Partial pressure exerted by each gas.

The total pressure of the gases can be calculated by using an ideal gas equation:

P = 0.92 atm = Total  pressure of the mixture

Partial pressure of all the gases can be determined by using Dalton's law of partial pressure

Partial pressure of methane gas

Partial pressure of nitrogen gas

Partial pressure of carbon dioxide gas

c) The total pressure exerted by the mixture is 0.92 atm.

d) Percentage by volume of each gas in the mixture

Volume of the methane gas:

Volume percentage of methane :

Volume of the nitrogen gas:

Volume percentage of nitrogen:

Volume of the carbon dioxide gas:

Volume percentage of carbon dioxide:

where is the following

explanation:

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.