### Problem Statement**Objective:**To determine the volume of hydrogen gas produced when 35.3 grams of iron reacts completely according to the following reaction at 25°C and 1 atm:\[\text{iron(s)} + \text{hydrochloric acid(aq)} \rightarrow \text{iron(II) chloride(aq)} + \text{hydrogen(g)}\]**Required Calculation:**Volume of hydrogen gas produced, \( \text{Volume} = \) \_\_\_\_ L (liters).**Chemical Reaction Explanation:**When iron reacts with hydrochloric acid, iron(II) chloride and hydrogen gas are produced. The reaction can be written as follows:\[\text{Fe(s)} + 2\text{HCl(aq)} \rightarrow \text{FeCl}_2\text{(aq)} + \text{H}_2\text{(g)}\]In this reaction, solid iron (Fe) reacts with aqueous hydrochloric acid (HCl) to form aqueous iron(II) chloride (FeCl₂) and hydrogen gas (H₂).### Calculations (Not Provided in Image):To find the volume of hydrogen gas produced, you need to:1. **Determine Moles of Iron:** - Calculate the molar mass of iron (Fe), which is approximately 55.85 g/mol. - Determine the moles of iron in 35.3 g. \[ \text{Moles of Fe} = \frac{35.3 \text{ g}}{55.85 \text{ g/mol}} \approx 0.632 \text{ moles} \]2. **Stoichiometry of the Reaction:** - According to the balanced chemical equation, 1 mole of Fe produces 1 mole of H₂ gas. - Therefore, 0.632 moles of Fe will produce 0.632 moles of H₂ gas.3. **Using Ideal Gas Law:** - The volume of a gas at standard temperature and pressure (STP, which is 0°C and 1 atm) is 22.4 L per mole. However, the conditions given are 25°C and 1 atm. - Use the ideal gas law \( PV = nRT \), where: - \(P\) is the pressure (1 atm), - ### Reaction of Iron with Chlorine Gas**Problem Statement:**- **Question:** How many grams of **iron** are needed to completely consume **40.0 L** of **chlorine gas** according to the following reaction at **25°C** and **1 atm**?**Chemical Equation:**\[ \text{iron (s) + chlorine (g) → iron(III) chloride (s)} \]- **Answer Placeholder:** \_\_\_\_ grams **iron**Students are expected to determine the mass of iron required to react with 40.0 liters of chlorine gas under the given conditions by using stoichiometric principles and the ideal gas law.**Note:**This question requires knowledge of the ideal gas law, stoichiometry, and molar masses of the reactants and products. The calculations will involve:1. Determining the moles of chlorine gas using the ideal gas law.2. Using the stoichiometric coefficients from the balanced chemical equation to find the corresponding moles of iron.3. Calculating the mass of iron needed using its molar mass. Be sure to apply accurate unit conversions and theoretical principles for precise calculations.

Ideal gas equation: PV = nRT P = pressureV = volumen = moles R = gas constantT = temperatureBalanced…

What volume of hydrogen gas is produced when 35.3 g of iron reacts completely according to the following reaction at 25 °C and 1 atm? iron(s) + hydrochloric acid (aq) → iron (II) chloride (aq) + hydrogen (g) L Volume =

What volume of hydrogen gas is produced when 35.3 g of iron reacts completely according to the following reaction at 25 °C and 1 atm? iron(s) + hydrochloric acid (aq) → iron (II) chloride (aq) + hydrogen (g) L Volume =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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