What factors control the rate of a chemical reaction? Why do each contribute to the speed of the reaction? Be sure to describe the behavior of the particles involved in reaction as part of your explanation.

Two chemicals A and B are combined to form a chemical C. The rate, or velocity, of the reaction is proportional to the product of the instantaneous amounts of A and B not converted to chemical C. Initially, there are 100 grams of A and 50 grams of B, and for each gram of B, 2 grams of A is used. It is observed that 15 grams of C is formed in 10 minutes. How much is formed in 40 minutes? (Round your answer to one decimal place.) 46.15 grams What is the limiting amount of C after a long time? 150 grams How much of chemicals A and B remains after a long time? A grams В grams At what time is chemical C half-formed? t = 13.8 X min

(1 Try Again Your answer is incorrect. • Row 3: Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. Here is a graph of the molarity of formic acid (HCO₂H) in a reaction vessel during a certain chemical reaction. Use this graph to answer the questions in the table below. 3 0.030 0.025 0.020 0.0187 0.015 0.010- 0.005 0 y 500 1000 1500 seconds 2000 2500 3000 × Ś

The rate of a reaction is how quickly the reaction goes to completion. If two reactions have the same amount of reactant, increasing the rate does not increase the amount of product produced, it simply reduces the time that it takes to make the product.    Using the internet , research the four factors below that affect the rate of a chemical reaction.    1. Reactant concentration (  explained with details and add graphs to explain what you wrote for each one of them) 2. pressure  (  explained with details and add graphs to explain what you wrote for each one of them) 3. Temperature  (  explained with details and add graphs to explain what you wrote for each one of them) 4. Presence of a catalyst.    (  explained with details and add graphs to explain what you wrote for each one of them)          Your work should be written in complete sentences, and assume your audience is grade 11 chemistry students who do not understand this unit. Make sure all research is put into your own words!

Consider the same reaction carried out two more times, both at the same condition(including concentration and temperature), but where the volume of the reaction is doubled in the second reaction. Since the concentrations are the same in both cases, the 2nd has twice the quantity of gases. How do those two rates of reaction compare to each other? Please compare using units of moles/(L•min) and separately using units of moles/min.

Nitrous oxide decomposes to nitrogen and oxygen in the following reaction:2N2​O(g)2N2​(g)+O2​(g)Using this concentration versus time plot, answer the following questions.   The green curve in the concentration versus time diagram is associated with which chemical in the balanced reaction?      The blue curve in the concentration versus time diagram is associated with which chemical in the balanced reaction?

A chemistry graduate student is studying the rate of this reaction: She fills a reaction vessel with and measures its concentration as the reaction proceeds: time (seconds) Use this data to answer the following questions. Write the rate law for this reaction. rate Calculate the value of the rate constant . Round your answer to significant digits. Also be sure your answer has the correct unit symbol.

Consider the following reaction: 2H₂O₂(aq)→ 2H₂O(1) + O₂(g) Concentration (M) 1.2 1.0 0.8- 0.6- 0.4- 0.2- 0 0 10 Show Transcribed Text 20 [H₂O₂] 30 c 40 50 Time (s) 60 70 80 The graph shows the concentration of H₂O₂ as a function of time. Use the graph to calculate the following. a.) Calculate the average rate of the reaction between 10 and 20 s. b.) Calculate the instantaneous rate of the reaction at 30 s. c.) Calculate the instantaneous rate of formation of O₂ at 50 s. d.) If the initial volume of the H₂O₂ solution is 1.5 L, what total amount of O₂ (in moles) is formed in the first 50 s of reaction?

0.003 ? 0.00218 0.002 - M 0.001 5 10 15 20 25 30 seconds created x10 Is H,0, being created or destroyed by the chemical destroyed reaction? neither created nor destroyed If f H,O, is being created or destroyed, what is the rate at which it is being created or destroyed 7 seconds after the reaction starts? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. If H,O, is being created or destroyed, what is the average rate at which it is being created or destroyed during the first 7 seconds of the reaction? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. 미

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.