How much heat, in kilojoules, is released when nitrogen and hydrogen react to form 50.0 g of ammonia?

$N_{2}(g) + 3H_{2}(g) → 2NH_{3}(g)$ ΔH = -92.2 kJ

Question

How much heat, in kilojoules, is released when nitrogen and hydrogen react to form 50.0 g of ammonia?

[latex] N_{2}(g) + 3H_{2}(g) → 2NH_{3}(g)[/latex] ΔH = -92.2 kJ

Accepted Answer

STEP 1 State the given and needed quantities (moles).

ANALYZE THE PROBLEM	Given	Need	Connect
	50.0 g of [latex]NH_{3}[/latex]	heat released, in kilojoules	ΔH = - 92.2 kJ, molar mass
	Equation
	[latex] N_{2}(g) + 3H_{2}(g) → 2NH_{3}(g) [/latex]

STEP 2 Write a plan using t he heat of reaction and any molar mass needed.

[latex] grams of NH_{3} \boxed{\begin{array}{l} ext{Molar}\ ext{Mass}\end{array}} → moles of NH_{3} \boxed{\begin{array}{l} ext{Heat of}\ ext{reaction}\end{array}} → kilojoules [/latex]

STEP 3 Write the conversion factors including heat of reaction.

[latex] \begin{array}{r c}\boxed{\begin{matrix} 1 mole of NH_{3}= 17.03 g of NH_{3}\\frac{17.03 g NH_{3}}{1 mole NH_{3}} ext{ and } \frac{1 mole NH_{3}}{17.03 g NH_{3}} \end{matrix}} & \boxed{\begin{matrix}2 moles of NH_{3} = -92.2 kj \ \frac{-92.2 kj}{ 2 moles NH_{3}} ext{ and }\frac{2 moles NH_{3}}{-92.2 kj} \end{matrix}}\end{array} [/latex]

STEP 4 Set up the problem to calculate the heat.

[latex] \underset{Three SFs }{50.0 \cancel{g NH_{3}}} imes \overset{Exact}{\underset{Four SFs }{\boxed{\frac{1 \cancel{mole NH_{3}}}{17.03 \cancel{ g NH_{3}}} }}} imes \overset{Three Sfs }{\underset{Exact }{\boxed{\frac{-92.2 kJ}{2 \cancel{ moles NH_{3}}} }}} = \underset{Three Sfs }{-135 kJ}[/latex]

Therefore, 135 kJ are released.

Question 7.17: How much heat, in kilojoules, is released when nitrogen and ...

Related Answered Questions

In the reaction of 1 mole of solid carbon with oxygen gas, the energy of the carbon dioxide gas produced is 393 kJ lower than the energy of the reactants. a. Is the reaction exothermic or endothermic? b. Write the balanced chemical equation for the reaction, including the heat of reaction. c. Is ...

Verified Answer:

On a space shuttle, LiOH is used to absorb exhaled CO2 from breathing air to form LiHCO3. LiOH(s) + CO2(g) → LiHCO3(s) What is the percent yield of LiHCO3 for the reaction if 50.0 g of LiOH gives 72.8 g of LiHCO3? ...

Verified Answer:

Verified Answer:

Carbon monoxide and hydrogen are used to produce methanol (CH4O). The balanced chemical reaction is CO(g) + 2H2(g) → CH4O(g) If 3.00 moles of CO and 5.00 moles of H2 are the initial reactants, what is the limiting reactant, and how many moles of methanol can be produced? ...

Verified Answer:

When acetylene, C2H2, bums in oxygen, high temperatures are produced that are used for welding metals. 2C2H2(g) + 5O2(g) →^Δ 4CO2(g) + 2H2O(g) How many grams of CO2 are produced when 54.6 g of C2H2 is burned? ...

Verified Answer:

In the chemical reaction of iron and sulfur, how many moles of sulfur are needed to react with 1.42 moles of iron? 2Fe(s) + 3S(s) – Fe2S3(s) ...

Verified Answer:

A salt shaker contains 73.7 g of NaCl. How many moles of NaCl are present? ...

Verified Answer:

Silver metal is used in the manufacture of tableware, mirrors, jewelry, and dental alloys. If the design for a piece of jewelry requires 0.750 mole of silver, how many grams of silver are needed? ...

Verified Answer:

Calculate the molar mass for lithium carbonate, Li2CO3, used to treat bipolar disorder. ...

Verified Answer:

How many moles of carbon are present in 1.50 moles of aspirin, C9H8O4? ...

Verified Answer: