   # Nitroglycerin decomposes into four different gases when detonated: 4 C 3 H 5 (NO 3 ) 3 ( ℓ ) → 6 N 2 (g) + O 2 (g) + 12 CO 2 (g) + 10 H 2 O(g) The detonation of a small quantity of nitroglycerin produces a total pressure of 4.2 atm at a temperature of 450 °C. (a) What is the partial pressure of N 2 ? (b) If the gases occupy a volume of 1.5 L, what mass of nitroglycerin was detonated? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 10, Problem 66GQ
Textbook Problem
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## Nitroglycerin decomposes into four different gases when detonated:4 C3H5(NO3)3(ℓ) → 6 N2(g) + O2(g) + 12 CO2(g) + 10 H2O(g)The detonation of a small quantity of nitroglycerin produces a total pressure of 4.2 atm at a temperature of 450 °C. (a) What is the partial pressure of N2? (b) If the gases occupy a volume of 1.5 L, what mass of nitroglycerin was detonated?

(a)

Interpretation Introduction

Interpretation:

For the given reaction under given set of conditions the partial pressure of N2 has to be calculated.

Concept Introduction:

Ideal gas Equation:

Any gas is described by using four terms namely pressure, volume, temperature and the amount of gas.  Thus combining three laws namely Boyle’s, Charles’s Law and Avogadro’s Hypothesis the following equation could be obtained.  It is referred as ideal gas equation.

nTPV = RnTPPV = nRTwhere,n = moles of gasP = pressureT = temperatureR = gas constant

Under some conditions gases don not behave like ideal gas that is they deviate from their ideal gas properties.  At lower temperature and at high pressures the gas tends to deviate and behave like real gases.

Boyle’s Law:

At given constant temperature conditions the mass of given ideal gas in inversely proportional to its volume.

Charles’s Law:

At given constant pressure conditions the volume of ideal gas is directly proportional to the absolute temperature.

Two equal volumes of gases with same temperature and pressure conditions tend to have same number of molecules with it.

### Explanation of Solution

Given:

T = 450 oC = 273.15+450 = 723.15KP = 4.2 atmPartial pressure of N2=?V=1.5LMassofNitroglycerin=?

The partial pressure for the given gas is determined as follows,

(b)

Interpretation Introduction

Interpretation:

For the given reaction under given set of conditions the mass of N2 produced has to be calculated.

Concept Introduction:

Ideal gas Equation:

Any gas is described by using four terms namely pressure, volume, temperature and the amount of gas.  Thus combining three laws namely Boyle’s, Charles’s Law and Avogadro’s Hypothesis the following equation could be obtained.  It is referred as ideal gas equation.

nTPV = RnTPPV = nRTwhere,n = moles of gasP = pressureT = temperatureR = gas constant

Under some conditions gases don not behave like ideal gas that is they deviate from their ideal gas properties.  At lower temperature and at high pressures the gas tends to deviate and behave like real gases.

Boyle’s Law:

At given constant temperature conditions the mass of given ideal gas in inversely proportional to its volume.

Charles’s Law:

At given constant pressure conditions the volume of ideal gas is directly proportional to the absolute temperature.

Two equal volumes of gases with same temperature and pressure conditions tend to have same number of molecules with it.

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