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How many moles of helium is in a 250. L balloon at STP ? first: This is a problem a. missing variable b. change in conditions C. 22.414 L/1 mol d. density = molar mass/22.414 L e. partial P second: we need to solve for using the equation f. P g. P1 h. P2 i. V j. V1 (not V) k. V2 (not V) I. n m. n1 (not n) n. n2 (not n) o. T p. T1 (not T) q. T2 (not T) r. R= 8.205 x 10-² L atm/K mol s. 22.414 L/1 mol t. Ptotal = P1 + P2 + .. u. PV = nRT v. P¡V1 P2V2 n2T2 finally: The answer is V. 68300 mol w. 62.5 mol X. 5600 mol V. 11.2 mol

How many moles of helium is in a 250. L balloon at STP ? first: This is a problem a. missing variable b. change in conditions C. 22.414 L/1 mol d. density = molar mass/22.414 L e. partial P second: we need to solve for using the equation f. P g. P1 h. P2 i. V j. V1 (not V) k. V2 (not V) I. n m. n1 (not n) n. n2 (not n) o. T p. T1 (not T) q. T2 (not T) r. R= 8.205 x 10-² L atm/K mol s. 22.414 L/1 mol t. Ptotal = P1 + P2 + .. u. PV = nRT v. P¡V1 P2V2 n2T2 finally: The answer is V. 68300 mol w. 62.5 mol X. 5600 mol V. 11.2 mol

Chemistry
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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### Problem Analysis: Moles of Helium in a Balloon at STP **Problem Statement:** How many moles of helium is in a 250 L balloon at STP (Standard Temperature and Pressure)? **Steps to Solve:** **First: Identify the Type of Problem** - This is a **missing variable** problem related to gases. **Options:** a. missing variable b. change in conditions c. 22.414 L/1 mol d. density = molar mass/22.414 L e. partial P **Second: Determine What to Solve For and the Equation to Use** - Solve for **n** (moles) using the equation **PV = nRT**. **Variables to Consider:** f. P (Pressure) g. P₁ h. P₂ i. V (Volume) j. V₁ (not V) k. V₂ (not V) l. n (desired variable) m. n₁ (not n) n. n₂ (not n) o. T (Temperature) p. T₁ (not T) q. T₂ (not T) r. R = 8.205 x 10⁻² L atm/K mol (Ideal Gas Constant) s. 22.414 L/1 mol (Molar Volume at STP) **Equations:** t. \( P_{\text{total}} = P_1 + P_2 + \ldots \) u. \( PV = nRT \) v. \(\frac{P_1V_1}{n_1T_1} = \frac{P_2V_2}{n_2T_2}\) **Finally: Determine the Answer** - The answer is **11.2 mol**. **Options:** v. 68300 mol w. 62.5 mol x. 5600 mol y. 11.2 mol This analysis walks through the process of solving for the moles of a gas using the Ideal Gas Law, ensuring the identification of right variables and recognizing the conditions at Standard Temperature and Pressure.
Transcribed Image Text:### Problem Analysis: Moles of Helium in a Balloon at STP **Problem Statement:** How many moles of helium is in a 250 L balloon at STP (Standard Temperature and Pressure)? **Steps to Solve:** **First: Identify the Type of Problem** - This is a **missing variable** problem related to gases. **Options:** a. missing variable b. change in conditions c. 22.414 L/1 mol d. density = molar mass/22.414 L e. partial P **Second: Determine What to Solve For and the Equation to Use** - Solve for **n** (moles) using the equation **PV = nRT**. **Variables to Consider:** f. P (Pressure) g. P₁ h. P₂ i. V (Volume) j. V₁ (not V) k. V₂ (not V) l. n (desired variable) m. n₁ (not n) n. n₂ (not n) o. T (Temperature) p. T₁ (not T) q. T₂ (not T) r. R = 8.205 x 10⁻² L atm/K mol (Ideal Gas Constant) s. 22.414 L/1 mol (Molar Volume at STP) **Equations:** t. \( P_{\text{total}} = P_1 + P_2 + \ldots \) u. \( PV = nRT \) v. \(\frac{P_1V_1}{n_1T_1} = \frac{P_2V_2}{n_2T_2}\) **Finally: Determine the Answer** - The answer is **11.2 mol**. **Options:** v. 68300 mol w. 62.5 mol x. 5600 mol y. 11.2 mol This analysis walks through the process of solving for the moles of a gas using the Ideal Gas Law, ensuring the identification of right variables and recognizing the conditions at Standard Temperature and Pressure.
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