A sample of Nitrogen gas (N) at 17° C is in a 575 mL container under 85,000 mmHG of pressure. What is the mass of the sample, in grams?

Mass = 75.6 g

Explanation:

Given data:

Temperature of gas = 17°C

Volume of gas = 575 mL

Pressure of gas = 85000 mmHg

Mass of gas = ?

Solution:

Temperature of gas = 17°C (17+273 =290 K)

Volume of gas = 575 mL (575/1000 = 0.575 L)

Pressure of gas = 85000 mmHg (85000/760 = 111.8 atm)

Formula:

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

111.8 atm × 0.575 L = n×0.0821 atm.L/ mol.K  × 290 K

64.285 atm. L = n×23.809 atm.L/ mol

n =  64.285 atm. L / 23.809 atm.L/ mol

n = 2.7 mol

Mass of nitrogen gas:

Mass = number of moles × molar mass

Mass = 2.7 mol × 28 g/mol

Mass = 75.6 g

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

did anyone actually do this? like if anyone has submitted this i rly need .