How many grams of h2 are needed to produce 10.42 g of nh3

1.84g of H₂ are needed to produce 10.42g of NH₃

Explanation:

In the production of ammonia, NH₃, the following reaction occurs

N₂ + 3H₂ ⇄ 2NH₃

From, the above, 3 moles of hydrogen gas (H₂) is required to produce 2 moles of ammonia (NH₃).

The atomic mass of Hydrogen is 1 g/mol, 3 moles of hydrogen gas are present in the reactant, hence the mass of hydrogen gas in the equation is;

3 × 2 × 1 = 6g

The atomic mass of Nitrogen is 14g/mol, that of hydrogen is 1g/mol and 2 moles of ammonia were produced. Hence the mass of ammonia in the equation is;

(2 × 14) + (2 × 3 × 1) = 34g

From the above, it can be deduced that 6g of H₂ is required to produce 34g of NH₃, hence "x" grams of H₂ are needed to produce 10.42g of NH₃

To find x (which is the unknown)

6g ⇒ 34g

x ⇒ 10.42g

x =

x = 1.84g

1.84g of H₂ are needed to produce 10.42g of NH₃

a small container that holds a source of energy a solar cell that captures light energy and converts it into electricity a voltaic cell that uses the oxidation of a fuel to produce electricity

explanation:

the answer is c i believe