Posted: March 14th, 2023

Factors Affecting the Rate of a Reaction

The aim of this experiment is to investigate whether changing the concentration of a solution will have any effect on the rate of the reaction. We are trying to prove that increasing the concentration will speed up the rate of the reaction.

What Citation Styles Can You Use for My Essay?

Students often ask, “Can you write my essay in APA or MLA?”—and the answer’s a big yes! Our writers are experts in every style imaginable: APA, MLA, Chicago, Harvard, you name it. Just tell us what you need, and we’ll deliver a perfectly formatted paper that matches your requirements, hassle-free.

The rate of a chemical reaction is the rate at which reactants are used up or products are produced. In order to measure the rate of reaction we measure the amount of reactants used or products produced over a certain period of time. In our experiment we have chosen to use sodium thiosulphate and hydrochloric acid. This is because this reaction would be the easiest for us to note the rate of the reaction.

According to Le Chatelier’s Principle; “if a system that is in equilibrium is disturbed, the equilibrium position will change in order to oppose the disturbing influence and re-establish equilibrium” (1). Therefore if the concentration of a substance is increased then the reaction that removes that substance will be favoured in order to re-establish equilibrium in the system. So if we are increasing the concentration of the reactants then the forward reaction will speed up. Based on this information we can predict that the rate of the reaction of sodium thiosulphate and hydrochloric acid will speed up with increased concentration.

Since increasing the concentration will increase the amount of molecules we can predict that there will be more effective collisions taking place. The more effective collisions taking place, the quicker the rate of the reaction will be.

Increasing the concentration of a substance will increase the rate of the reaction.

Is It Legal to Use Your Writing Service?

Absolutely, it’s 100% legal! Our service provides sample essays and papers to guide your own work—think of it as a study tool. Used responsibly, it’s a legit way to improve your skills, understand tough topics, and boost your grades, all while staying within academic rules.

• 5 Equal Volume conical flasks
• One 500cm³ measuring cylinder
• Two 100cm³ measuring cylinder
• One 10cm³ measuring cylinder
• 8g of sodium thiosulphate
• 35cm³ concentrate hydrochloric acid
• 1 electronic scale
• 1 filter paper
• 1 stopwatch
• 1 piece of white paper with black cross

Flask	Sodium Thiosulphate concentration (cm³)	Time (s) How Much Does It Cost to Get a Paper Written? Our pricing starts at $10 per page for undergrad work, $16 for bachelor-level, and $21 for advanced stuff. Urgency and extras like top writers or plagiarism reports tweak the cost—deadlines range from 14 days to 3 hours. Order early for the best rates, and enjoy discounts on big orders: 5% off over $500, 10% over $1,000! (experiment 1)	Time (s) (experiment 2)
1 Will My Use of This Service Stay Private? Yes, totally! We lock down your info with top-notch encryption—your school, friends, no one will know. Every paper’s custom-made to blend with your style, and we check it for originality, so it’s all yours, all discreet.	50	32.72	24.16
2 Do You Use AI to Write Papers? No way—our papers are 100% human-crafted. Our writers are real pros with degrees, bringing creativity and expertise AI can’t match. Every piece is original, checked for plagiarism, and tailored to your needs by a skilled human, not a machine.	40	33.80	27.90
3 Why Choose You for Research Papers? We’re the best because our writers are degree-holding experts—Bachelor’s to Ph.D.—who nail any topic. We obsess over quality, using tools to ensure perfection, and offer free revisions to guarantee you’re thrilled with the result, even on tight deadlines.	30	54.60	43.01
4 Who’s Writing My College Essays? Our writers are top-tier—university grads, many with Master’s degrees, who’ve passed tough tests to join us. They’re ready for any essay, working with you to hit your deadlines and grading standards with ease and professionalism.	20	84.92	71.01
5 Are Your Papers Original? Always! We start from scratch—no copying, no AI—just pure, human-written work with solid research and citations. You can even get a plagiarism report to confirm it’s 95%+ unique, ready for worry-free submission.	10	197.40	158.19

From the above tables and graphs we can see that our hypothesis is correct. Increasing the concentration of a solution will increase the rate of the reaction. We can also see from the table and the graphs that the rate of the reaction differed in experiment 2. The reason for this could be that when we prepared the dilute solution of hydrochloric acid we did not mix it properly with the water. This lead to there being a stronger dilute in the bottom of the measuring cylinder compared to that at the top of the measuring cylinder. This would have affected the results as it means that in experiment 1 there was a weaker solution of hydrochloric acid used, when it came to experiment 2 we were using the solution at the bottom of the cylinder and that part of the solution is stronger and more concentrated.

Can You Match Any Citation Style?

You bet! From APA to IEEE, our writers nail every style with precision. Give us your guidelines, and we’ll craft a paper that fits your academic standards perfectly, no sweat.

This actually helped prove our hypothesis as we can see that in experiment 2 the rate of the reaction was shorter. This is because there was a higher concentration of hydrochloric acid being added to the solution.

In the graph concentration vs. 1/time we can see that a straight line is formed. This means that there is an inverse relationship between concentration and the rate of a reaction. As the concentration of a substance is increased then the time for the reaction to take place is decreased.

From all of the above results from the experiment conducted we can conclude that the rate of a reaction is affected by the concentration of a substance. As there is a higher concentration of molecules in the substance then there will be more effective collisions taking place which means that the reaction will take place much faster.

Chemistry Practical Investigation Preparation

Can I Update Instructions Mid-Order?

Yep! Use our chat feature to tweak instructions or add details anytime—even after your writer’s started. They’ll adjust on the fly to keep your essay on point.

In this practical investigation we are going to investigate the effect that concentration has on the rate of a reaction. In order to do this we are going to conduct an experiment which involves adding different concentrations of a substance to another substance and then take note of the different rates of reaction, if any difference is to be seen. If a difference is seen then we can come to the conclusion that concentration does have an effect on the rate of a reaction.

According to Le Chatelier’s Principle; “if a system that is in equilibrium is disturbed, the equilibrium position will change in order to oppose the disturbing influence and re-establish equilibrium” (1). Therefore if the concentration of a substance is increased then the reaction that removes that substance will be favoured in order to re-establish equilibrium in the system. So if we are increasing the concentration of the reactants then the forward reaction will speed up. Based on this information we can predict that the rate of the reaction of sodium thiosulphate and hydrochloric acid will speed up with increased concentration.

Since increasing the concentration will increase the amount of molecules we can predict that there will be more effective collisions taking place. The more effective collisions taking place, the quicker the rate of the reaction will be. Thus we can conclude in our hypothesis that increasing the concentration of a substance will increase the rate of the reaction.

The rate of a chemical reaction is the rate at which reactants are used up or products are produced. In order to measure the rate of reaction we measure the amount of reactants used or products produced over a certain period of time. In our experiment we have chosen to use sodium thiosulphate and hydrochloric acid. This is because this reaction would be the easiest for us to note the rate of the reaction. Other reactions that we could’ve used include the reaction that is represented in the following equation; 2 NO + O2 = 2 NO2. The reason that we did not chose this reaction is because it would be to complicated for us to monitor the rate of the reaction. It is for this reason that we chose to use the reaction between hydrochloric acid and sodium thiosulphate.

How Do I Get an Essay Written?

Easy—place your order online, and your writer dives in. Check drafts or updates as you go, then download the final paper from your account. Pay only when you’re happy—simple and affordable!

In this experiment we are going to prepare five measuring cylinders each with different concentrations of sodium thiosulphate in. This is to test what effect the different concentrations have on the rate of the reaction. In order to make sure that each flask has an equal total volume we will add water to the each measuring cylinder. The next step of the process is to draw a cross on a piece of paper and place it under the measuring cylinder. Once that has been done we will add a dilute solution of hydrochloric acid to each of the measuring cylinders. Since we know that this reaction produces a creamy yellow precipitate it will not be hard to measure the rate of the reaction. Once the hydrochloric acid has been added we will time how long it takes until we cannot see the cross on the paper, this means until the creamy yellow precipitate is formed and the solution becomes turbid.

If our hypothesis is correct then we will find that the measuring cylinders with a higher concentration of sodium thiosulphate will take quicker to form a creamy-yellow precipitate, thus proving that increasing concentration increases the rate of the reaction.

Bibliography:

1. M. Mann: Physical Science 12 textbook and workbook October 2007: page 16-1

1. http://www.azete.com/view/48253

1. http://www.science.uwaterloo.ca/~cchieh/cact/c123/coneffec.html