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What is the pressure (in bar) of a sample of N2H4 gas with a density of 2.15 g/L at 298 K?

What is the pressure (in bar) of a sample of N2H4 gas with a density of 2.15 g/L at 298 K?

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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**Question 2** What is the pressure (in bar) of a sample of \(N_2H_4\) gas with a density of 2.15 g/L at 298 K? *Explanation for Educational Website:* This question involves calculating the pressure of a gas using the ideal gas law equation or a variation that incorporates density. The parameters given are: - **Density:** 2.15 g/L - **Temperature:** 298 K - **Molar mass of \(N_2H_4\):** This would be needed for calculations, calculated as follows: \( (2 \times \text{Atomic mass of N}) + (4 \times \text{Atomic mass of H}) = \text{molar mass of } N_2H_4 \). Tools or formulas you might need: 1. Ideal Gas Law: \( PV = nRT \) 2. Modification involving density: \( P = \frac{dRT}{M} \) Where: - \( P \) = pressure, - \( V \) = volume, - \( n \) = moles of gas, - \( R \) = ideal gas constant (R = 0.0821 L atm K\(^{-1}\) mol\(^{-1}\) or adjusted for different units), - \( T \) = temperature in Kelvin, - \( d \) = density, - \( M \) = molar mass. To solve the problem, determine the molar mass of hydrazine (\(N_2H_4\)), then apply the formula \( P = \frac{dRT}{M} \) to find the pressure in bar.
Transcribed Image Text:**Question 2** What is the pressure (in bar) of a sample of \(N_2H_4\) gas with a density of 2.15 g/L at 298 K? *Explanation for Educational Website:* This question involves calculating the pressure of a gas using the ideal gas law equation or a variation that incorporates density. The parameters given are: - **Density:** 2.15 g/L - **Temperature:** 298 K - **Molar mass of \(N_2H_4\):** This would be needed for calculations, calculated as follows: \( (2 \times \text{Atomic mass of N}) + (4 \times \text{Atomic mass of H}) = \text{molar mass of } N_2H_4 \). Tools or formulas you might need: 1. Ideal Gas Law: \( PV = nRT \) 2. Modification involving density: \( P = \frac{dRT}{M} \) Where: - \( P \) = pressure, - \( V \) = volume, - \( n \) = moles of gas, - \( R \) = ideal gas constant (R = 0.0821 L atm K\(^{-1}\) mol\(^{-1}\) or adjusted for different units), - \( T \) = temperature in Kelvin, - \( d \) = density, - \( M \) = molar mass. To solve the problem, determine the molar mass of hydrazine (\(N_2H_4\)), then apply the formula \( P = \frac{dRT}{M} \) to find the pressure in bar.
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