Atmospheric scientists often use mixing ratios to express the concentrations of trace compounds in air. Mixing ratios are often expressed as ppmv (parts per million volume):\[ \text{ppmv of } X = \frac{\text{vol of } X \text{ at STP}}{\text{total vol of air at STP}} \times 10^6 \]On a certain November day, the concentration of carbon monoxide in the air in downtown Denver, Colorado, reached \(3.2 \times 10^2\) ppmv. The atmospheric pressure at that time was 625 torr and the temperature was 0°C.a. What was the partial pressure of CO?Partial pressure = _______ torrb. What was the concentration of CO in molecules per cubic meter?Concentration = _______ molecules/m\(^3\)c. What was the concentration of CO in molecules per cubic centimeter?Concentration = _______ molecules/cm\(^3\)

Given data: Total pressure = 625 torr Temperature = 0 ℃ Concentration of CO = 3.2×102 ppmv

Atmospheric scientists often use mixing ratios to express the concentrations of trace compounds in air. Mixing ratios are often expressed as ppmv (parts per million volume): vol of X at STP ppmv of X = × 106 total vol of air at STP On a certain November day, the concentration of carbon monoxide in the air in downtown Denver, Colorado, reached 3.2 × 102 atmospheric pressure at that time was 625 torr and the temperature was 0°C. ppmv. The a. What was the partial pressure of CO? Partial pressure = torr b. What was the concentration of CO in molecules per cubic meter? Concentration = molecules/m3 c. What was the concentration of CO in molecules per cubic centimeter? Concentration = molecules/cm³

Atmospheric scientists often use mixing ratios to express the concentrations of trace compounds in air. Mixing ratios are often expressed as ppmv (parts per million volume): vol of X at STP ppmv of X = × 106 total vol of air at STP On a certain November day, the concentration of carbon monoxide in the air in downtown Denver, Colorado, reached 3.2 × 102 atmospheric pressure at that time was 625 torr and the temperature was 0°C. ppmv. The a. What was the partial pressure of CO? Partial pressure = torr b. What was the concentration of CO in molecules per cubic meter? Concentration = molecules/m3 c. What was the concentration of CO in molecules per cubic centimeter? Concentration = molecules/cm³

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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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

Atmospheric scientists often use mixing ratios to express the concentrations of trace compounds in air. Mixing ratios are often expressed as ppmv (parts per million volume):

\[ \text{ppmv of } X = \frac{\text{vol of } X \text{ at STP}}{\text{total vol of air at STP}} \times 10^6 \]

On a certain November day, the concentration of carbon monoxide in the air in downtown Denver, Colorado, reached \(3.2 \times 10^2\) ppmv. The atmospheric pressure at that time was 625 torr and the temperature was 0°C.

a. What was the partial pressure of CO?

Partial pressure = _______ torr

b. What was the concentration of CO in molecules per cubic meter?

Concentration = _______ molecules/m\(^3\)

c. What was the concentration of CO in molecules per cubic centimeter?

Concentration = _______ molecules/cm\(^3\)

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