Question

An important reaction in the manufacture of nitric acid is the catalytic oxidation of ammonia.
4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)
For every mole of O2 that reacts in this way, 181.8 kJ of energy are released.
A factory makes 2.50 × 105 mol of NO every day.
How much energy, in kJ, is released every day?

Method please....

Answer 1

Answer: The amount of energy released is $5.68\times 10^7kJ$

Explanation:

We  are given:

Moles of NO = $2.50\times 10^5$ moles

For the given chemical equation:

$4NH_3(g)+5O_2(g)\rightarrow 4NO(g)+6H_2O(g)$

By Stoichiometry of the reaction:

4 moles of NO are produced when 5 moles of oxygen gas is reacted.

So, $2.50\times 10^5$ moles of NO will be produced when = $\frac{5}{4}\times 2.50\times 10^5=3.125\times 10^5$ moles of oxygen gas is reacted.

We are given:

Amount of heat released when 1 mole of oxygen gas reacts = 181.8 kJ

To calculate the amount of heat released for given amount of oxygen gas, we use unitary method:

Amount of heat released when 1 mole of oxygen gas reacts is 181.8 kJ

So, the amount of heat released when $3.125\times 10^5$ moles of oxygen gas will react is = $\frac{3.125\times 5}{1}\times 181.8=5.68\times 10^7kJ$

Hence, the amount of energy released is $5.68\times 10^7kJ$

Answer 2

Answer:

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Explanation: