For the following reaction, 6.65 grams of oxygen gas are mixed with excess hydrogen sulfide. The reaction yields 2.19 grams of water. hydrogen sulfide (g) + oxygen (g) →→→→water (1) + sulfur dioxide (g) What is the theoretical yield of water? What is the percent yield of water? grams %

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**Chemical Reaction Analysis**

For the following reaction, **6.65 grams** of **oxygen gas** are mixed with excess **hydrogen sulfide**. The reaction yields **2.19 grams** of **water**.

\[ \text{hydrogen sulfide (g)} + \text{oxygen (g)} \rightarrow \text{water (l)} + \text{sulfur dioxide (g)} \]

- **What is the theoretical yield of water?** ___ grams
- **What is the percent yield of water?** ___%

This setup involves determining the theoretical and percent yield of water based on the given amounts of oxygen and the product obtained.
Transcribed Image Text:**Chemical Reaction Analysis** For the following reaction, **6.65 grams** of **oxygen gas** are mixed with excess **hydrogen sulfide**. The reaction yields **2.19 grams** of **water**. \[ \text{hydrogen sulfide (g)} + \text{oxygen (g)} \rightarrow \text{water (l)} + \text{sulfur dioxide (g)} \] - **What is the theoretical yield of water?** ___ grams - **What is the percent yield of water?** ___% This setup involves determining the theoretical and percent yield of water based on the given amounts of oxygen and the product obtained.
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