Ayield of nh₃ of approximately 98% can be obtained at 200°c and 1,000 atmospheres of pressure. how many grams of n₂ must react to form 1.7 grams of ammonia, nh₃?
a. 0.0058 g
b. 052 g
c. 1.4 g
d. 2.8 g

The mass of nitrogen gas that must be reacted is 1.4 grams

Explanation:

To calculate the number of moles, we use the equation:

     .....(1)

Given mass of ammonia = 1.7 g

Molar mass of ammonia = 17 g/mol

Putting values in equation 1, we get:

The chemical equation for the production of ammonia follows:

By Stoichiometry of the reaction:

2 moles of ammonia is produced by 1 mole of nitrogen gas

So, 0.1 moles of ammonia will be produced from of nitrogen gas

Now, calculating the mass of nitrogen gas from equation 1, we get:

Molar mass of nitrogen gas = 28 g/mol

Moles of nitrogen gas = 0.05 moles

Putting values in equation 1, we get:

Hence, the mass of nitrogen gas that must be reacted is 1.4 grams

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."