In the reaction:
n2(g) + 3H2(g) -> 2NH3(g), nitrogen is
A. electrolyzed
B. synthesized
C. oxidized
D. reduced
e. None of these
Well, let's analyze the situation and find out what's going on here. We have nitrogen (N2) combining with hydrogen (H2) to form ammonia (NH3). Now, let's think about the changes that are happening.
In the reaction, nitrogen is going from being a neutral molecule (N2) to being part of a compound (NH3). So, we can say that nitrogen is being reduced. It's like nitrogen is putting on a fancy suit and becoming part of a new compound. So, the answer is D. Reduced.
But hey, don't feel bad for nitrogen. It's just going through a little transformation, like a caterpillar turning into a butterfly. It's all part of the circle of life, or in this case, the circle of chemistry.
In the given reaction: n2(g) + 3H2(g) -> 2NH3(g), nitrogen (N2) undergoes a change in its oxidation state from 0 to -3 in ammonia (NH3). Since the oxidation state of nitrogen decreases from 0 to -3, nitrogen is being reduced. Therefore, the correct answer is D. reduced.
To determine which option best describes the role of nitrogen in the given reaction (N2(g) + 3H2(g) -> 2NH3(g)), we need to understand the concept of oxidation and reduction reactions.
Oxidation refers to the loss of electrons or an increase in oxidation state, while reduction refers to the gain of electrons or a decrease in oxidation state.
In the reaction, nitrogen (N2) combines with hydrogen (H2) to form ammonia (NH3). To identify whether nitrogen is being oxidized or reduced, we need to compare the oxidation states of nitrogen before and after the reaction.
In its elemental form, nitrogen (N2) has an oxidation state of 0. In ammonia (NH3), the oxidation state of nitrogen is -3, since hydrogen has an oxidation state of +1. Therefore, we conclude that nitrogen is being reduced from an oxidation state of 0 to -3.
Among the options provided, the correct answer is D. Reduced.