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Ch.10 - Gases
All textbooksBrown 14th EditionCh.10 - GasesProblem 119
Chapter 10, Problem 119

Consider the combustion reaction between 1.00 L of liquid methanol (density = 0.850 g/mL) and 500 L of oxygen gas measured at STP. The products of the reaction are CO2(g) and H2O(g). Calculate the volume of liquid H2O formed if the reaction goes to completion and you condense the water vapor.

Verified step by step guidance
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Step 1: Write the balanced chemical equation for the combustion of methanol (CH3OH). The reaction is: \[ 2 \text{CH}_3\text{OH} (l) + 3 \text{O}_2 (g) \rightarrow 2 \text{CO}_2 (g) + 4 \text{H}_2\text{O} (g) \].
Step 2: Calculate the mass of methanol using its volume and density. Use the formula: \[ \text{mass} = \text{density} \times \text{volume} \]. Convert the volume from liters to milliliters first.
Step 3: Convert the mass of methanol to moles using its molar mass. The molar mass of methanol (CH3OH) is approximately 32.04 g/mol. Use the formula: \[ \text{moles} = \frac{\text{mass}}{\text{molar mass}} \].
Step 4: Determine the limiting reactant by comparing the mole ratio of methanol to oxygen gas. At STP, 1 mole of gas occupies 22.4 L. Calculate the moles of oxygen gas using its volume and compare it to the stoichiometric ratio from the balanced equation.
Step 5: Calculate the moles of water produced using the stoichiometry of the balanced equation. Then, convert the moles of water to volume using the density of water (1 g/mL) and the molar mass of water (18.02 g/mol). Use the formula: \[ \text{volume} = \frac{\text{moles} \times \text{molar mass}}{\text{density}} \].
Related Practice
Textbook Question
It turns out that the van der Waals constant b equals four times the total volume actually occupied by the molecules of a mole of gas. Using this figure, calculate the fraction of the volume in a container actually occupied by Ar atoms (b) at 20.27 MPa pressure and 0 °C. (Assume for simplicity that the ideal-gas equation still holds.)
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Textbook Question

Large amounts of nitrogen gas are used in the manufacture of ammonia, principally for use in fertilizers. Suppose 120.00 kg of N21g2 is stored in a 1100.0-L metal cylinder at 280 °C. (b) By using the data in Table 10.3, calculate the pressure of the gas according to the van der Waals equation.

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Textbook Question

Cyclopropane, a gas used with oxygen as a general anesthetic, is composed of 85.7% C and 14.3% H by mass. (a) If 1.56 g of cyclopropane has a volume of 1.00 L at 99.7 kPa and 50.0 °C, what is the molecular formula of cyclopropane?

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Textbook Question

An herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor expressed at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl. (b) Calculate its empirical formula.

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Textbook Question

An herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor expressed at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl. (c) What other information would you need to know about this compound to calculate its true molecular formula?

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Textbook Question

A 4.00-g sample of a mixture of CaO and BaO is placed in a 1.00-L vessel containing CO2 gas at a pressure of 97.33 kPa and a temperature of 25 °C. The CO2 reacts with the CaO and BaO, forming CaCO3 and BaCO3. When the reaction is complete, the pressure of the remaining CO2 is 20.0 kPa. (b) Calculate the mass percentage of CaO in the mixture.

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