Answered: Chemistry Question

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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Expert Solution

Step 1 Introduction

Consider the pressure be atmospheric pressure which is 1 atm.

Let us consider the gas equation PV=nRT

Here $n = \frac{M a s s (m)}{M o l a r M a s s (M)}$

So, $P V = (\frac{m}{M}) R T$

Density(d) is defined as the mass of the substance per unit volume.

Therefore, PM=dRT

Density (d) = $\frac{P M}{R T}$

where P-Pressure = 1atm

M-Molar Mass = 28.02g/mol for N₂

R-Gas constant = 0.08205 L atm mol^-1 K^-1

T- Temperature = 370.4 K

Step 2 Solution

$\begin{array}{rcl} D e n s i t y o f N 2 a t 370.4 K & = & \frac{1 a t m \times 28.02 g / m o l}{0.08025 L a t m m o l^{- 1} K^{- 1} \times 370.4 K K} \\ = & \frac{28.02}{30.39} g / L \\ = & 0.922 g / L \end{array}$

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