   Chapter 10, Problem 64GQ

Chapter
Section
Textbook Problem

If you place 2.25 g of solid silicon in a 6.56-L flask that contains CH3Cl with a pressure of 585 mm Hg at 25 °C, what mass of dimethyldichlorosilane, (CH3)2SiCl2, can be formed?Si(s) + 2 CH3Cl(g) → (CH3)2SiCl2(g)What pressure of (CH3)2SiCl2(g) would you expect in this same flask at 95 °C on completion of the reaction? (Dimethyldichlorosilane is one starting material used to make silicones, polymeric substances used as lubricants, antistick agents, and water-proofing caulk.)

Interpretation Introduction

Interpretation:

For the given reaction under given conditions the mass of the product (CH3)2SiCl2 formed and the pressure of the product in the flask if the temperature is found to be at 95oC should be determined.

Concept introduction:

Ideal gas Equation:

Any gas can be 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.

Molar mass: The molar mass of a substance is determined by dividing the given mass of substance by the amount of the substance.

Explanation

Given,

Volume, V = 6.56 Lmass of Si = 2.25gGas constant, R = 0.0821 L atm mol-1K-1Temperature, T = 25C  =273.15+25 =298.15K Pressure, P = 585mmHg =585 mm Hg760 mm Hg=0.770atmMass of the product formed = ?Pressure of the product at 95C=?

First the mass of the product formed from the given reaction is determined as follows,

From the given balanced reaction is Si(s)+2CH3Cl(g)(CH3)2SiCl2(g) it is clear that one mole of Si requires 2 moles of CH3Cl to produce 1 mole of (CH3)2SiCl2 product.

The given amount of Si is 2.25g therefore first it should be converted into moles as follows,

moleSi=givenmassmolarmass=2.25g28.09gmol1=0.080mol

The available mole of CH3Cl is as follows,

moleofCH3Cl(g)PV=nRTn=PVRT=0

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