Question

Given that ${C_4}{H_{10\left( g \right)}} + \dfrac{{13}}{2}{O_{2\left( g \right)}} + 4C{O_{2\left( g \right)}} + 5{H_2}O\left( l \right) \to ;\Delta H = - 2878kJ$
\[\Delta H\] is the heat of combustion of butane gas. If true enter 1 else 0

Answer 1

Hint: First, we see what enthalpy of a response is,
Enthalpy:
The enthalpy change is characterized as the energy ingested or delivered in any response.
If energy is absorbed by the reaction it is said to be endothermic and is positive and more energy is needed to break the bonds and the reactants are lower in energy than the products.
If energy is released by the reaction is said to be exothermic and is negative and more energy is released while forming bonds and the energy of the product is lower than the reactants.

Complete step by step answer:
We need to remember that the warmth of ignition is the measure of heat developed when one mole of the substance is totally burned in air or oxygen.
The reaction is,
${C_4}{H_{10\left( g \right)}} + \dfrac{{13}}{2}{O_{2\left( g \right)}} + 4C{O_{2\left( g \right)}} + 5{H_2}O\left( l \right) \to ;\Delta H = - 2878kJ$
In the above response, 1 mole of butane goes through burning. Henceforth, $\Delta H$ is the heat of combustion of butane gas. Hence the statement is true.

Additional information:
Now, we discuss the enthalpy of fusion.
Enthalpy of fusion:
We must need to know that the heat which a solid absorbs when it melts is termed the enthalpy of fusion or heat of fusion and is sometimes quoted on a molar basis. For instance, when \[1mol\] of ice is melted, we discover the molar enthalpy of fusion of ice is \[ + 6.01kJmo{l^{-1}}\], and we can write that as,
${H_2}O\left( s \right)\xrightarrow{{{0^ \circ }C}}{H_2}O\left( l \right)$
$\Delta {H_m} = 6.01\,kJ/mol$

Note: Now we can discuss about the concept of enthalpy of Vaporization as,
We must need to know that when a liquid is boiled, the difference of temperature with the heat supplied is analogous to that found for melting. When heat is supplied at a gentle rate to a liquid at air pressure, the temperature rises until the boiling point is attained. After the boiling point the temperature remains constant until the enthalpy of vaporization \[(\Delta Hm)\] is supplied and again the temperature rises once all the liquid has been converted to vapor. In such cases of water the molar enthalpy of vaporization is \[40.67kJmo{l^{ - 1}}\] .