A 10.0 gram rock sample at 85.0°C was dropped into a 30.0g Al calorimeterwhich contains 50.0g water. The final temperature of the mixture is 45.0°C.Find the initial temperature of the calorimeter and water in Celsius. *AlwaterrockSpecific heat J/g C0.9004.1862.00O 34.7O 22.5O 41.6O 36.8 In the following chemical reaction, the initial concentration of H2O2 is0.2546 M and the initial rate of reaction is 9.32 x 10^-4 M/s. What will be theconcentration of H2O2 at t = 35 s? *2H202 → 2H20 + 020.2220 M0.3220 M0.50000 M0.4300 M

Given that: Initial concentration of H2O2 = 0.2546 M Initial rate of reaction = 9.32×10-4 M/s…

In the following chemical reaction, the initial concentration of H2O2 is 0.2546 M and the initial rate of reaction is 9.32 x 10^-4 M/s. What will be the concentration of H2O2 at t = 35 s? * 2H202 → 2H20 + 02 0.2220 M 0.3220 M

In the following chemical reaction, the initial concentration of H2O2 is 0.2546 M and the initial rate of reaction is 9.32 x 10^-4 M/s. What will be the concentration of H2O2 at t = 35 s? * 2H202 → 2H20 + 02 0.2220 M 0.3220 M

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

A chemistry graduate student is studying the rate of this reaction: 2C1,0, (g)- 2C1, (g) +50, (g) He fills a reaction vessel with Cl,0, and measures its concentration as the reaction proceeds: time [C,0,] (seconds) 0| 0.0900 M 10. 0.0579 M 20. 0.0372 M 30. 0.0239 M 40. 0.0154 M Use this data to answer the following questions. Write the rate law for this reaction. rate Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
Consider the given reaction : 2HgC2(ag) + C204²(ag) – 2CH(ag) + 2CO2(g) + Hg2Cl2(s) Experiment [HgCl2] [C2O42] Initial rate 1 0.0836 M 0.202 M 5.2 x10-5 0.0836 M 0.404 M 2.08 x10-4 0.0418 M 0.404 M 1.04 x104 4 0.0627 M 0.606 M ? Calculate the initial rate for experiment 4. 3.50 x 10-4 M min-1 8.75 x 103 M min-1 1.20 x 10-4 M min-1 O 6.00 x 104 M min 1
17. SHOW ALL YOUR WORK OGiven the following data, determine the order of the reaction with respect to NO(g). 2 NO(g) + Cl2(g)→ 2 NOCI(g) Experiment 1 [C2] (M) 0.0100 [NO] (M) Rate (M/s) 3.4 x 104 1.36 x 103 3.4 x 104 0.0300 0.0150 0.0150 0.0100 3 0.0400
Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A]2 where k= 1.45 ×10-2 M-1s-1 at a particular temperature. If the initial [A] = 0.300 M, what will be the concentration of A remaining after 3.00 minutes? 0.168 M 0.0221 M 0.296 M 0.287 M
Consider the following balanced chemical reaction: A + B → C The following table shows initial reaction rates obtained using different initial concentration of A and B: Initial [A] (mol L-) Initial [B] (mol L-1) Initial Rate (mol L-1 s-1) 0.202 0.350 0.138 0.202 0.701 0.277 0.604 0.350 0.413 0.604 0.701 0.827 If rate = k[A]"[B]" , then m = • and n =
Reaction of nitrogen monoxide and hydrogen A student collects the data below for the reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) Trial [NO]i [H2]i Initial Rate (M/s) 1 0.050 M 0.050 M 0.0917 2 0.10 M 0.050 M 0.367 3 0.10 M 0.10 M 0.734 Write 2-3 sentences to describe how you determined the rate law for the reaction.
A chemistry graduate student is studying the rate of this reaction: H₂CO3 (aq) → H₂O (aq) + CO₂ (aq) He fills a reaction vessel with H₂CO3 and measures its concentration as the reaction proceeds: time (seconds) 0 10. 0.0334M 20. [H₂CO3] 0.100M 30. 0.0200M 0.0143 M 40. 0.0111 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X
A chemistry graduate student is studying the rate of this reaction: 2C1₂O5 (g) → 2Cl₂ (g) +50₂ (g) He fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [C₁₂05] 0.600M 0.215M 0.20 00. 0.131M 0.30 0.0941 M 0.40 0.0734M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate k = - k 0 ☐x10 X Ś
The reaction A+B → C was investigated in a series of experiments with different initial concentrations of the two reactants. The following initial rates were observed. What is the overall reaction order? O 0 05 02 0 1 O 3 04 Experiment 1 Experiment 2 Experiment 3 Initial [A] 0.10 M 0.20 M 0.20 M Initial [B] 0.10 M 0.10 M 0.20 M Initial rate 1.60 x 10-2 mol L-1 s-1 3.20 x 10-2 mol L-1 5-1 3.20 x 10-2 mol L-1 5-1
1. Given the following data, determine the orders (m and n) with respect to the concentrations of A and B in the reaction Orders: [A] 0.020 M 0.020 M 0.010 M 0.010 M m= A+B products Rate = k[A][B]" [B] 0.020 M 0.010 M 0.020 M 0.010 M n = Time for reaction 19 sec 19 sec 76 sec 76 sec What time would you predict if both concentrations of A and B were made to be 0.040 M?
What is the rate of the reaction when A=0.43M and B=0.31M?
Consider the balanced chemical equation. H₂O₂ (aq) +31 (aq) + 2H+(aq) → I3¯¯(aq) + 2H₂O(1) In the first 11.0 s of the reaction, the concentration of I drops from 1.000 M to 0.752 M. Part A Predict the rate of change in the concentration of H₂O2 (A[H₂O2]/At). Express the rate to three significant figures and include the appropriate units. A[H₂O₂]/At = Submit Request Answer Part B Value μÀ HÅ Δ[13]/Δt = Value Predict the rate of change in the concentration of I3 (A[13¯]/At). Express the rate to three significant figures and include the appropriate units. Submit Request Answer Units Units ? www. ?