A gas contains 0.1 mol of oxygen and .4 moles of Nitrogen. If the sample is at standard temperature and pressure, what is the partial pressure of nitrogen?

The partial pressure of nitrogen is 1.25 atm

Explanation:

From ideal gas equation:

where,

R = Gas constant =

T = temperature of the gas = 273K (at STP)

P = pressure of the gas = 1 atm   (at STP)

n = number of moles = 0.1 +0.4 = 0.5

To calculate the partial pressure of the solution, we use the law given by Dalton, which is:

Or,

where,  = mole fraction nitrogen =

We are given:

Total pressure = 1 atm

Putting values in above equation, we get:

Thus the partial pressure of nitrogen is 1.25 atm

the earth would become to overheated and everything alive on it will eventually die from overheating. plants will eventually die as well, water will evaporate, and it will be nothing but a hot planet without anything living on it.

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.