Answer:
Explanation:
The moles of H2 and N2 are as follows respectively, 0.3915mol of H2 and 0.1305 mol of N2.
The alkali metals are so reactive that they are never found in nature in elemental form. Although some of their ores are abundant, isolating them from their ores is somewhat difficult. For these reasons, the group 1 elements were unknown until the early 19th century, when Sir Humphry Davy first prepared sodium (Na) and potassium (K) by passing an electric current through molten alkalis. (The ashes produced by the combustion of wood are largely composed of potassium and sodium carbonate.) Lithium (Li) was discovered 10 years later when the Swedish chemist Johan Arfwedson was studying the composition of a new Brazilian mineral. Cesium (Cs) and rubidium (Rb) were not discovered until the 1860s, when Robert Bunsen conducted a systematic search for new elements. Known to chemistry students as the inventor of the Bunsen burner, Bunsen’s spectroscopic studies of ores showed sky blue and deep red emission lines that he attributed to two new elements, Cs and Rb, respectively. Francium (Fr) is found in only trace amounts in nature, so our knowledge of its chemistry is limited. All the isotopes of Fr have very short half-lives, in contrast to the other elements in group 1.
Answer : It takes less amount of heat to metal 1.0 Kg of ice.
Solution :
The process involved in this problem are :
Now we have to calculate the amount of heat released or absorbed in both processes.
<u>For process 1 :</u>
where,
= amount of heat absorbed = ?
m = mass of water or ice = 1.0 Kg
= enthalpy change for fusion = 
Now put all the given values in , we get:
<u>For process 2 :</u>
where,
= amount of heat absorbed = ?
m = mass of water = 1.0 Kg
= specific heat of liquid water = 
= initial temperature = 
= final temperature = 
Now put all the given values in , we get:
From this we conclude that, 
that means it takes less amount of heat to metal 1.0 Kg of ice.
Hence, the it takes less amount of heat to metal 1.0 Kg of ice.
