I need help determining the gas A CH4 B NH3 C C2H6 D CO2

Option D. CO2.

Explanation:

Data obtained from the question include:

Mass = 0.301 g

Volume = 0.153 L

Next, we shall determine the density of the gas. This is shown below:

Density = mass /volume

Density = 0.301/0.153

Density = 1.967 g/L

At standard temperature and pressure, the volume occupied by 1 mole of a gas is 22.4L.

Note: When we divide the molar mass of any gas by its density at STP, the volume obtained is 22.4L.

Now let us determine the identity of the gas.

For CH4:

Molar mass of CH4 = 12 + 4 = 16 g/mol

Density = 1.967 g/L

Volume =?

Volume = molar mass / Density

Volume = 16/1.967

Volume = 8.13 L

For NH3:

Molar mass of NH3 = 14 + (3x1) = 17 g/mol

Density = 1.967 g/L

Volume =?

Volume = molar mass / Density

Volume = 17/1.967

Volume = 8.64 L

For C2H6:

Molar mass of C2H6 = (12x2) + (6x1) = 30 g/mol

Density = 1.967 g/L

Volume =?

Volume = molar mass / Density

Volume = 30/1.967

Volume = 15.25 L

For CO2:

Molar mass of CO2 = 12 + (2x16) = 44 g/mol

Density = 1.967 g/L

Volume =?

Volume = molar mass / Density

Volume = 44/1.967

Volume = 22.4 L

From the above illustration, only CO2 gave a value of 22.4 L which is the standard value for the volume of a gas at stp.

Therefore, the gas is CO2.

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"

2b2t

explanation:

2b2t