Introduction:
In this question, we are given the formula of the higher oxide of an element (EO3) and the percentage of hydrogen in its hydride (2.47%). We need to determine the identity of the element (E) based on this information.

Analysis:
To solve this problem, we need to consider the valency of the element (E) and the ratio of hydrogen atoms in the hydride. Let's analyze each option and determine the most suitable element.

A) Te (Tellurium):
The higher oxide of tellurium is TeO3. Tellurium has a valency of +6, which matches the formula EO3. However, the hydride of tellurium is H2Te, which contains two hydrogen atoms per tellurium atom. Therefore, option A is not the correct answer.

B) Se (Selenium):
The higher oxide of selenium is SeO3. Selenium has a valency of +6, which matches the formula EO3. Additionally, the hydride of selenium is H2Se, which contains two hydrogen atoms per selenium atom. Therefore, option B is not the correct answer.

C) S (Sulfur):
The higher oxide of sulfur is SO3. Sulfur has a valency of +6, which matches the formula EO3. However, the hydride of sulfur is H2S, which contains two hydrogen atoms per sulfur atom. Therefore, option C is not the correct answer.

D) Si (Silicon):
The higher oxide of silicon is SiO3. Silicon has a valency of +4, which does not match the formula EO3. Therefore, option D is not the correct answer.

Conclusion:
After analyzing all the options, none of them satisfy both the valency requirement and the hydride composition. Therefore, none of the given options (A, B, C, D) is the correct answer. It is possible that the question may have a typographical error or missing information.

Sulphur (S) has highest oxidation of +6 ,so EO3 satisfy to sulphur as it also for So3but others don't form like teo3 & seo3