Recent questions in Chemical reactions

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A chemistry student needs to prepare a buffer solution with a pH of 7.2 using acetic acid (CH3COOH) and sodium acetate (CH3COONa). The student has 100 mL of 0.1 M acetic acid and 100 mL of 0.1 M sodium acetate. What volume of each solution do they need to mix to prepare the desired buffer solution with a total volume of 500 mL?

asked Jan 22 in Chemical reactions by DomingoMarce (750 points)

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1 answer 52 views

A chemistry student needs to prepare a buffer solution with a pH of 5.2 using acetic acid (CH3COOH) and sodium acetate (NaC2H3O2). The student has 10 mL of 0.15 M acetic acid and 15 mL of 0.20 M sodium acetate. What volume of water should the student add to make the desired buffer solution?

asked Jan 22 in Chemical reactions by EarnestineGo (590 points)

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1 answer 77 views

A chemistry student needs to prepare a buffer solution of pH 5.0 using acetic acid and acetate ions. If the student has 0.3 M acetic acid and 0.2 M acetate ions, what volume of acetic acid and acetate ions should he/she mix to prepare a solution with a total volume of 500 mL?

asked Jan 22 in Chemical reactions by EileenRubin0 (690 points)

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1 answer 48 views

A chemistry student needs to find the rate of a chemical reaction for a given set of concentrations and time, given the following reaction: 2H2 (g) + O2 (g) -> 2H2O (g)If the initial concentrations of H2 and O2 are 0.5 M and 0.2 M, and the reaction rate is 0.12 M/s, what is the concentration of H2O after 10 seconds?

asked Jan 22 in Chemical reactions by PatriceBayle (370 points)

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1 answer 67 views

A chemistry student needs to determine the precipitate formed when 50 mL of 0.2 M silver nitrate solution is mixed with 75 mL of 0.1 M potassium chloride solution. What is the mass of the precipitate formed and what is the percent yield of the reaction?

asked Jan 22 in Chemical reactions by AnnabelleHed (550 points)

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1 answer 65 views

A chemistry student needs to determine the enthalpy change for the reaction of nitrogen gas reacting with hydrogen gas to form ammonia gas, given that they have the following information:N2(g) + 3H2(g) --> 2NH3(g) ΔH1 = -92.4 kJ/mol2H2(g) + O2(g) --> 2H2O(l) ΔH2 = -572.0 kJ/molN2(g) + O2(g) --> 2NO(g) ΔH3 = +180.6 kJ/molUse Hess's law to calculate the enthalpy change for the reaction:2NH3(g) + 5O2(g) --> 2HNO3(aq) + 2H2O(l)

asked Jan 22 in Chemical reactions by LeandroOxley (410 points)

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1 answer 47 views

A chemistry student needs to determine the effect on the equilibrium position of a chemical reaction when the concentration of a reactant is decreased. The student is given the balanced equation: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + heatIf the concentration of H₂ is decreased by removing 50% of its concentration, what would be the effect on the concentration of N₂, NH₃, and the position of equilibrium?

asked Jan 22 in Chemical reactions by KieraSeton95 (530 points)

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1 answer 67 views

A chemistry student needs to determine the effect of increasing temperature on the equilibrium position of a chemical reaction in which an exothermic reaction is taking place. Given the balanced chemical equation A + B ⇌ C + heat, the student needs to determine how the concentration of products and reactants will change as the temperature is increased, and explain the observed changes using Le Chatelier's principle.

asked Jan 22 in Chemical reactions by AnnieJohnsto (290 points)

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1 answer 57 views

A chemistry student needs to determine the direction in which equilibrium will shift when the concentration of reactants in a reversible reaction is changed using Le Chatelier's principle. Given the reaction equation: 2SO2(g) + O2(g) ⇄ 2SO3(g), if the concentration of SO2 is increased, will the reaction shift to the left or right?

asked Jan 22 in Chemical reactions by DarciPok795 (530 points)

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1 answer 76 views

A chemistry student needs to determine the concentration of a sulfuric acid solution by titrating 25.0 mL of the acid with 0.1000 M sodium hydroxide. The reaction between the two substances is H2SO4 + 2NaOH → Na2SO4 + 2H2O. If it takes 35.0 mL of the sodium hydroxide solution to fully neutralize the sulfuric acid, what is the concentration of the sulfuric acid solution in moles per liter (M)?

asked Jan 22 in Chemical reactions by BlakeSalaam (450 points)

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1 answer 46 views

A chemistry student needs to determine how the equilibrium concentration of products and reactants change when the temperature is increased in the reaction: 2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g) Given the initial concentrations of 0.15 M SO2, 0.025 M O2, and 0 M SO3, and a temperature increase of 50°C, calculate the new equilibrium concentration of each compound using Le Chatelier's Principle.

asked Jan 22 in Chemical reactions by Cynthia53529 (450 points)

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1 answer 59 views

A chemistry student needs to calculate the equilibrium constant for the following reaction:2 H2O(g) ⇌ 2 H2(g) + O2(g)The student has the initial concentration of H2 and O2 as 0.25 M and the initial concentration of H2O as 1.00 M. After the system reaches equilibrium, the student measures the concentration of H2 as 0.10 M. Using this information, what is the value of the equilibrium constant, Kc, for the above reaction?

asked Jan 22 in Chemical reactions by WillianHowto (510 points)

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1 answer 38 views

A chemistry student is studying the equilibrium reaction between nitrogen dioxide (NO2) and dinitrogen tetroxide (N2O4) and wants to test Le Chatelier's principle. They have a mixture of NO2 and N2O4 in a container. The student wants to determine the effect of temperature on the equilibrium position of the reaction. What temperature should the student use to shift the equilibrium towards the side with more NO2 gas?

asked Jan 22 in Chemical reactions by AntonyMahuri (800 points)

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1 answer 70 views

A chemistry student is required to calculate the activation energy of a chemical reaction. Given the rate constant of a reaction at two different temperatures, what is the activation energy?

asked Jan 22 in Chemical reactions by VioletConsta (490 points)

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1 answer 91 views

A chemistry student is provided with 10 grams of copper oxide and 5 grams of magnesium. The student reacts the two substances to form copper and magnesium oxide. What is the limiting reactant in this reaction and how many grams of copper can be produced?

asked Jan 22 in Chemical reactions by ChelseyB4436 (430 points)

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1 answer 59 views

A chemistry student is given a solution of iron(III) sulfate and potassium iodide. The student is asked to predict the products and balance the chemical equation for the redox reaction that occurs when the two solutions are mixed. What is the balanced chemical equation for the redox reaction that occurs between iron(III) sulfate and potassium iodide?

asked Jan 22 in Chemical reactions by EmilioMarcan (690 points)

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1 answer 39 views

A chemistry student is given a piece of copper and asked to react it with dilute hydrochloric acid. Will the reaction occur and if so, what product (if any) will be produced? Use your knowledge of single replacement reactions to explain your answer.

asked Jan 22 in Chemical reactions by AudreaPickar (540 points)

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1 answer 75 views

A chemistry student is experimenting with the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g). They want to investigate the effect of pressure on the yield of ammonia. Write a problem for the student to solve using Le Chatelier's principle that will help them predict the effect of changes in pressure on the equilibrium position of the reaction.

asked Jan 22 in Chemical reactions by JudyCottee50 (630 points)

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1 answer 35 views

A chemistry student is conducting an experiment in a closed container where nitrogen dioxide is being converted into nitrogen oxide and oxygen gas. If the student increases the concentration of the nitrogen dioxide in the container, how will it affect the equilibrium position of the reaction and what can be done to restore the equilibrium position? Use Le Chatelier's principle to explain your answer.

asked Jan 22 in Chemical reactions by CarolineLami (470 points)

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1 answer 41 views

A chemistry student is asked to determine the effect of temperature and pressure on the equilibrium of the reaction: 2NO2(g) ⇋ N2O4(g) using Le Chatelier’s principle. The initial concentration of NO2(g) is 0.5 mol/L and the reaction is carried out at 25°C. How will the equilibrium shift if the temperature is increased to 100°C and the pressure is decreased to 0.5 atm?

asked Jan 22 in Chemical reactions by BuckForro541 (490 points)

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