97.3 g of ZNO3 is mixed with 59.1 g of XCI. How many grams of NO2 will be produced from the balanced reaction shown below?

\[ \text{ZNO}_3 (s) + 2 \text{XCI} (aq) \rightarrow \text{ZCl}_2 (aq) + \text{NO}_2 (g) + \text{X}_2\text{O} (l) \]

You may not need all of the information below:

- Molar Mass of XCI = 36.46 g/mol
- Molar Mass of ZNO3 = 233.43 g/mol
- Molar Mass of ZCl2 = 208.23 g/mol
- Molar Mass of NO2 = 46.01 g/mol
- Molar Mass of X2O = 18.02 g/mol

For full credit, your answer must:
- Contain the correct number of significant figures
- Include the proper abbreviation for units

Your Answer:

The chemical reaction of 97.3 g ZNO3 with 59.1 g XCI intends to produce NO2. According to stoichiometry, the balanced equation indicates that 19.2 g of NO2 will be produced.

This question explores the concept of stoichiometry, which uses balanced chemical equations to predict the mass of products formed in a chemical reaction.

Given you have 97.3 g ZNO3 and 59.1 g XCI and the balanced equation

ZNO3 + 2XCI --> ZCl2 + NO2 + X20,

we first convert the known mass of the reactants to moles using their molar masses.

The molar mass of ZNO3 is 233.43 g/mol and XCI is 36.46 g/mol.

So, we have (97.3 g)/(233.43 g/mol) = 0.417 moles of ZNO3 and

(59.1 g)/(36.46 g/mol) = 1.62 moles of XCI.

According to stoichiometry, one mole of ZNO3 will produce one mole of NO2.

Therefore, only 0.417 moles of NO2 will be produced from the given amount of ZNO3. We then convert the moles of NO2 back to grams using the molar mass of NO2 which is 46.01 g/mol, giving an output (0.417 mol)*(46.01 g/mol) = 19.2 g of NO2.

In conclusion, from the balanced chemical reaction of 97.3 g ZNO3 with 59.1 g XCI, 19.2 g of NO2 is produced.

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