Consider the following equation for the formation of ammonia from nitrogen and hydrogen: ; N2 + 3H2 = 2NH3, How many hydrogen molecules are required to react with 100 molecules of nitrogen?

examrobotsa's picture

Submitted by examrobotsa on

Q: 91 (NDA-I/2009)
Consider the following equation for the formation of ammonia from nitrogen and hydrogen: ; N2 + 3H2 = 2NH3, How many hydrogen molecules are required to react with 100 molecules of nitrogen?

question_subject: 

Science

question_exam: 

NDA-I

stats: 

0,9,7,3,4,9,0

keywords: 

{'many hydrogen molecules': [0, 0, 1, 0], 'ammonia': [0, 1, 0, 2], 'nitrogen': [1, 1, 0, 2], 'hydrogen': [0, 0, 1, 3], 'n2': [1, 0, 3, 1], 'molecules': [0, 0, 1, 1], 'following equation': [0, 0, 1, 0], 'formation': [2, 1, 10, 19]}

Option 1: 100

This option suggests that 100 hydrogen molecules are required to react with 100 molecules of nitrogen. However, this is incorrect. The balanced equation tells us that three hydrogen molecules are required for every one molecule of nitrogen. So, if we have 100 molecules of nitrogen, we would need 300 hydrogen molecules, not 100.

Option 2: 200

This option suggests that 200 hydrogen molecules are required to react with 100 molecules of nitrogen. Again, this is incorrect. As mentioned before, the balanced equation states that three hydrogen molecules are needed for each nitrogen molecule. Therefore, 200 hydrogen molecules would not be enough to react with 100 molecules of nitrogen.

Option 3: 300

This option correctly states that 300 hydrogen molecules are required to react with 100 molecules of nitrogen. According to the balanced equation, the ratio of nitrogen to hydrogen is 1:3. Therefore, for every one nitrogen molecule, three hydrogen molecules are needed. With 100 molecules of nitrogen, we would need 300 hydrogen molecules.

Option 4: 400

This option suggests that 400 hydrogen molecules are required to react with 100 molecules of nitrogen. This is not correct. As previously explained, the ratio in the

Practice this on app