   Chapter 10, Problem 98IL

Chapter
Section
Textbook Problem

Group 2A metal carbonates are decomposed to the metal oxide and CO2 on heating:MCO3(s) → MO(s) + CO2(g)You heat 0.158 g of a white, solid carbonate of a Group 2A metal (M) and find that the evolved CO2 has a pressure of 69.8 mm Hg in a 285-mL flask at 25 °C. Identify M.

Interpretation Introduction

Interpretation:

From the given reaction the metal involved should be identified.

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

Given:

Total amount = 0.158 gVolume of CO2=285mL=285×10-3LPressure of CO2=69.8mmHg=69.8mmHg760mmHg=0.0918atmTemperature of CO2= 25oC = 273K+25=298K

First using the ideal gas equation the moles of CO2 produced is calculated as follows,

Here, we carry an extra significant figure throughout this calculation to limit rounding errors.

nCO2=PVRT =(0.0918atm)(285×10-3L)(0

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