Zinc reacts with nitric acid to produce hydrogen gas and zinc nitrate, Zn(NO3)2. 10.00 grams of zinc react with 7.84 grams of nitric acid. How many grams of excess reactant remain?

Zn is the excess reactant and remain 5.94g

Explanation:

The reaction of Zn with HNO3 is:

Zn + 2 HNO3 → H2 + Zn(NO3)2

1 mole of Zn reacts with 2 moles of HNO3

To solve this question we must convert the mass of each reactant to moles in order to find limiting reactant. Thus, we can kknow the moles of excess reactant that will not react:

Moles Zn -Molar mass: 65.38g/mol-:

10.00g * (1mol / 65.38g) = 0.1530 moles Zn

Moles HNO3 -Molar mass: 63.01g/mol-:

7.84g * (1mol / 63.01g) = 0.124 moles HNO3

For a complete reaction of 0.124 moles of HNO3 are required:

0.124 moles HNO3 * (1mol Zn / 2 mol HNO3) = 0.0622 moles Zn. As there are 0.1530 moles, Zn is the excess reactant and will remain:

0.1530 moles - 0.0622 moles = 0.0908 moles Zn

The mass is:

0.0908 moles Zn * (65.38g / mol) =

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.

thats how its supposed to be