Nitrogen dioxide reacts with water to produce oxygen and ammonia. a 5.00 l sample of h2o(g) reacts at a temperature of 380 ∘c and a pressure of 712 mmhg .part ahow many grams of nh3 can be produced? 4no2(g)+6h2o(g)→7o2(g)+4nh3(g)

0.99 g

Explanation:

Using ideal gas equation to calculate the moles of water as:-

where,

P = pressure of the gas = 712 mmHg  

V = Volume of the gas = 5.00 L

T = Temperature of the gas =

R = Gas constant =

n = number of moles of hydrogen gas = ?

Putting values in above equation, we get:

Moles of water = 0.0874 moles

From the reaction,

6 moles of water forms 4 moles of ammonia

1 mole of water forms 4/6 moles of ammonia

0.0874 moles of water forms (4/6)*0.0874 moles of ammonia

Moles of ammonia formed = 0.0583 moles

Molar mass of ammonia = 17.031 g/mol

The formula for the calculation of moles is shown below:

Thus,

c. 4.54 x 10–12 j happens to be correct