Measurements taken during the following reaction showed a concentration of carbon monoxide (CO) of 196.9 mol/L at 13.9 min and of 122.7 mol/L at 29.5 min. CO (g) + NO2 (g) --> CO2 (g) + NO (g) Calculate the average rate of the gain of carbon dioxide (CO2) in M/sec. Write the answer in scientific notation with 3 sig.dig.

Measurements taken during the following reaction showed a concentration of carbon monoxide (CO) of 196.9 mol/L at 13.9 min and of 122.7 mol/L at 29.5 min. CO (g) + NO2 (g) --> CO2 (g) + NO (g) Calculate the average rate of the gain of carbon dioxide (CO2) in M/sec. Write the answer in scientific notation with 3 sig.dig.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section: Chapter Questions

Problem 113QRT

See similar textbooks

QUESTION 10

Measurements taken during the following reaction showed a concentration of carbon monoxide (CO) of 196.9 mol/L at 13.9 min and of 122.7 mol/L at 29.5 min.

CO (g) + NO₂ (g) --> CO₂ (g) + NO (g)

Calculate the average rate of the gain of carbon dioxide (CO₂) in M/sec.

Write the answer in scientific notation with 3 sig.dig.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Calcium oxide (CaO), an important ingredient in cement, is produced by decomposing calcium carbonate (CaCO3) at high temperature: CaCO3(s) → CaO(s) + CO2(g) In one particular reaction, 70 g of CaCO3 is heated at 450°C in a 5.0 L vessel. The pressure of CO2 is 0.24 atm after 4.0 minutes. What is the average rate of CO2 production in moles per minute during the 4 minutes? (Enter in mol/min.) If you assume this rate of decomposition remains constant, how many minutes will it take for the entire sample of CaCO3 to decompose?
Calcium oxide, an important ingredient in cement, is produced by decomposing calcium carbonate at high temperature: CaCO3(s) → CaO(s) + CO2(g) In one reaction, 3.9 kg of calcium carbonate is heated at 589 °C in a 20.0-L vessel. The pressure of CO2 is 0.18 bar after 6.5 minutes. question 1. What is the average rate of CO2 production in mol/min during the 6.5-minute interval? question 2. How many moles of calcium carbonate consumed in the 6.5-minute interval?
If Δ[Br2]ΔtΔ[Br2]Δ� = 4.7×10−6 M/sM/s , what is the value of Δ[ClO−2]ΔtΔ[ClO2−]Δ� during the same time interval? Express your answer to two significant figures and include the appropriate units. What is the average rate of consumption of Br−Br− during the same time interval? Express your answer to two significant figures and include the appropriate units.
A gas, AB, decomposes and the volume of B2 produced is measured as a function of time. The data obtained are as follows: Time (min): 0, 8.3, 15.4, 19 Volume (L): 0, 4.2, 8.6, 11.5 What is the average rate of production of B2 for the first 19 min? Round your answer to 2 decimal places.
An unknown gas, D, reacts with fluorine gas to form the compound DF4 (g), as represented by the following equation: D(g) + 2F 2 (g) --> DF4 (g) B. What is the initial rate of disappearance of F2 (g) in trial 1. Justify.
Propane combustion results in the production of carbon dioxide and water vapor according to the following balanced chemical equation: C3H8 (g) + 5 O2 (g) --> 3 CO2 (g) + 4 H2O (g) If the concentration of carbon dioxide increases from 0.773 M to 0.961 M in the first 17.2 seconds, what is the rate of reaction (in M/s)? (answer in 3 significant figures)
The enzyme urease is widely used for determining urea concentration in blood. The Michaelis constant for urease at room temperature is 2.0 mM and k2 = 2.5 × 10^3 s^-1 at pH = 7.5. Based on the kinetic experiment, when 4.76 mM urease was used, the initial rate of the reaction was determined to be 8.1 M/sec. What is the concentration in unit of mM of urea in blood? Please keep your answer to two decimal place. Please convert all concentration unit to mM in calculation. The answer is 4.26 (I would need help getting this answer)
What is the average rate from t1= 50 s to t2= 100 s
In the following reaction represented by the net ionic equation, the rate of reaction of CN– is 0.312 mol/L·min. What is the rate of reaction of MnO4– (mol/L·min)? Report your answer to the thousandths place and do not include units. 2 MnO4– + 3 CN– + H2O → 2 MnO2 + 3 CNO– + 2 OH–
In a study of the gas phase decomposition of sulfuryl chloride at 600 KSO2Cl2(g)SO2(g) + Cl2(g)the concentration of SO2Cl2 was followed as a function of time.It was found that a graph of ln[SO2Cl2] versus time in minutes gave a straight line with a slope of -4.28×10-3 min-1 and a y-intercept of -6.95 . Based on this plot, the reaction is________. (firest, zero, or second) order in SO2Cl2 and the rate constant for the reaction is min-1.
The decomposition of H2O2 was studied and the concentration (in moles per liter) as a function of time was determined. a. Create a spreadsheet in Excel with the following columns and values. Calculate values for the natural logarithm of [H2O2] using an appropriate formula. Time H2O2(M) LN [H2O2] 0 0.862 120 0.556 240 0.394 360 0.246 480 0.149 b. Create a graph of [H2O2] versus time. Use the Scatter chart type and use the subtype that connect the points with a line. c. Create a graph of LN(H2O2) versus time. Use the scatter chart type and use the subtype that does not connect the points with a line. Instead, insert a trendline (linear fit) and display the equation of the line on the graph. d. Using the trendline equation, calculate the natural log of concentration (LN[H2O2] corresponding to a time elapsed of 200 seconds. From that value, calculate the molar concentration of H2O2 at 200 seconds
Here is a graph of the molarity of bromine Br2 in a reaction vessel during a certain chemical reaction. If Br2 is being created or destroyed, what is the rate at which it is being created or destroyed 10 seconds after the reaction starts? Round your answer to 2 significant digits. If Br2 is being created or destroyed, what is the average rate at which it is being created or destroyed during the first 10 seconds of the reaction? Round to 2 significant digits.