The number of moles for ethane combustion required to heat 371 g of water is to be calculated. Concept introduction: The specific heat of a material can be referred to as the amount of heat used to raise the temperature of 1 ° C for 1 g material. The heat related with the change in temperature of a material can be determined as q = s m Δ T Here, q is the heat, s is the specific heat, m is mass, and Δ T is the change in temperature of the material. The change in temperature of the material can be determined as Δ T = T final − T initial Here, Δ T is the change in temperature, T final is the final temperature, and T initial is the initial temperature. The standard enthalpy for a reaction is the amount of enthalpy that occurs at standard conditions. The standard enthalpy of reaction is to be determined using the equation given below: Δ H ° rxn = ∑ n Δ H f ° ( products ) − ∑ m Δ H f ° ( reactants ) Here, the stoichiometric coefficients are represented by m for reactants and n for products, enthalpy of formation at standard conditions are represented by Δ H f ° . The value of enthalpy of formation of an element is zero at its most stable state.

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Chapter 5, Problem 90AP

Interpretation Introduction

Interpretation:

The number of moles for ethane combustion required to heat $371 g$ of water is to be calculated.

Concept introduction:

The specific heat of a material can be referred to as the amount of heat used to raise the temperature of $1°C$ for $1 g$ material.

The heat related with the change in temperature of a material can be determined as

$q=smΔT$

Here, q is the heat, s is the specific heat, m is mass, and $ΔT$ is the change in temperature of the material.

The change in temperature of the material can be determined as

$ΔT=Tfinal−Tinitial$

Here, $ΔT$ is the change in temperature, $Tfinal$ is the final temperature, and $Tinitial$ is the initial temperature.

The standard enthalpy for a reaction is the amount of enthalpy that occurs at standard conditions.

The standard enthalpy of reaction is to be determined using the equation given below:

$ΔH°rxn=∑nΔHf°(products)−∑mΔHf°(reactants)$

Here, the stoichiometric coefficients are represented by m for reactants and n for products, enthalpy of formation at standard conditions are represented by $ΔHf°$ .

The value of enthalpy of formation of an element is zero at its most stable state.

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