**Chemical Reaction of Nitrogen Dioxide**In this example, nitrogen dioxide (NO₂) reacts to form nitrogen monoxide (NO) and oxygen gas (O₂). The chemical equation representing the reaction is:\[ 2NO_2(g) \rightarrow 2NO(g) + O_2(g) \]**Problem Statement:**A reaction container starts with an initial concentration of nitrogen dioxide, NO₂(g), at 0.350 M (molarity). The task is to determine the concentration of NO₂(g) after the reaction has proceeded for 30 seconds, given that the rate of NO₂(g) loss is \(1.20 \times 10^{-3}\) M/s.**Calculation Summary:**Given:- Initial concentration of NO₂(g): 0.350 M- Rate of reaction: \(1.20 \times 10^{-3}\) M/s- Reaction time: 30 secondsThe rate of reaction indicates how fast NO₂ is being consumed. To find the concentration after 30 seconds:\[ \text{Change in concentration} = \text{Rate} \times \text{Time} = 1.20 \times 10^{-3} \times 30 \]\[ \text{Change in concentration} = 0.036 \, \text{M} \]Subtract this change from the initial concentration to get the final concentration:\[ \text{Final concentration of NO}_2(g) = 0.350 \, \text{M} - 0.036 \, \text{M} = 0.314 \, \text{M} \]The concentration of NO₂(g) after 30 seconds is 0.314 M. This example demonstrates the calculation of reaction kinetics for a given chemical process.

Change in the concentration of compound per unit time is known as rate of a reaction.

Nitrogen dioxide will react to form nitrogen monoxide and oxygen gas according to the equation: 2NO2(g) → 2NO(g)+O2(g) A reaction container starts with an initial NO,(g) concentration of 0.350 M. What is the concentration of NO2(g) after the reactions processed for 30 seconds given the rate of NO;(g) loss 1.20× 10-3 M/s?

Nitrogen dioxide will react to form nitrogen monoxide and oxygen gas according to the equation: 2NO2(g) → 2NO(g)+O2(g) A reaction container starts with an initial NO,(g) concentration of 0.350 M. What is the concentration of NO2(g) after the reactions processed for 30 seconds given the rate of NO;(g) loss 1.20× 10-3 M/s?

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...

See similar textbooks

Similar questions

Can you help me correcting this questions in the picture with the notes below please? Notes: In question 1a, the rate law is fine but should have partial pressures, not concentrations. In 1b, the units of the answer are incorrect; they should have "atm" in it. Hint: in the denominator of the calculation is atm^3.
Consider the reaction: H2 (g) +I2 (g) → 2 HI (g) A chemist performed an experiment and monitored the concentration of I2 during the course of the reaction. The red line in the graph below represents the results obtained. Which line in the plot would best represent how the concentration of HI changes during the course of the reaction? Time (s) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a a b b d d е е Concentration (M)
Peroxynitric acid (HOONO2) is an unstable molecule that decomposes to nitric acid and oxygen: 2HOONO2(aq) → 2HNO3(aq) + O2(g)When the concentration of peroxynitic acid is graphed against time, the resulting plot is curved, but if the logarithm of this concentration is plotted, we instead get a straight line. Based on this, which statement is true? a) This decay is a second order in peroxynitric acid. b) The slope of the straight-line graph is the rate constant. c) One needs the concentration of peroxynitric acid to calculate its half-life. d) The rate law appears to be of the form -Δ[HOONO2]/Δt = k[HOONO2].
1a
Consider the reaction 2A --> A₂. If the initial concentration of A is 4 M, and after 10 minutes the reaction appears to stop when the concentration of [A] is 2.0 M
Enter your answer in the provided box. For the simple decomposition reaction AB(g)→ A(g) + B(g) rate = k[AB]2 and k = 0.10 L/mol·s. How long will it take for [AB] to reach 1/3 of its initial concentration of 1.50 M? t =_____s
(#28) Reaction Rates and time. A decomposition reaction in the first order has a rate constant of 1.26 x 10-4/sec. If the initial concentration of the reactant is 0.644 M. how much time will it take before 20% of the reactant has decomposed? 28a) In blank #1, type-in the working formula to solve for the time required. Enter the algebraic formula as a one-line equation and without spaces in between characters. Use lowercase for all fonts. 28b) In blank #2, type in your answer for the time it will take for 20% f the reactant to decompose. The answer is in seconds but do not include the unit. Enter your answer as a whole number with four significant figures.
5. Consider the following reaction: 2Fe(NO3)3(aq) + 3CuCl₂(aq) →→2FeCl3(s) + 3Cu(NO3)2 (aq) The concentration of Fe(NO3)3 (aq) at t = 19.4 s is 0.53 mol/L. At t = 59.8 s its concentration is 0.21 mol/L. a. Calculate the average rate of reaction with respect to Fe(NO3)3 (aq). b. Calculate the average rate at which Cu(NO3)2 (aq) is being formed. c. Calculate the average rate of reaction with respect to CuCl₂ (s). SHOW ALL YOUR WORK.
In the laboratory, hydrogen gas of good purity can most easily be obtained by the reaction of a strong acid, like sulfuric acid, on a reactive metal, such as zinc: Zn(s)+H,SO,(aq) ZnSO,(aq)+H, (g) Suppose an engineer decides to study the rate of this reaction. He prepares four reaction vessels by adding 160.9 g of solid zinc and 83. mL of 5.0 M sulfuric acid solution to each, and then filling the remainder of the vessel with distilled water. The volume and temperature of each vessel is shown in the table below. Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. alo Ar initial rate of vessel volume temperature reaction A 1.0 L 14.0 °C В 4.0 L 14.0 °C ? 2.0 L 14.0 °C 8.0 L 14.0 °C v ? 1 (highest) 2 4 (lowest) >