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A chemistry student is given a sample of a compound containing sulfur, oxygen, and carbon. The student needs to determine the mass percentages of each element in the compound using mass balance calculations. The sample has a total mass of 5.00 grams, and the student devises an experiment to isolate each of the three elements by chemical reactions, and the mass of each element is recorded as follows: 1.20 g sulfur, 1.80 g oxygen, and 2.00 g carbon. What are the mass percentages of sulfur, oxygen, and carbon in the compound?

asked Jan 22 in Analytical Chemistry by SterlingElki (3.1k points)

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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 JeanetteShar (2.2k points)

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A chemistry student is given a chemical equation for the reaction between calcium chloride and sodium carbonate. The equation is unbalanced and the student must balance it, while ensuring that the correct stoichiometric coefficients for each compound are used. The student must then calculate the mass of product formed when 5.0 grams of calcium chloride react completely with excess sodium carbonate. What is the mass of the product formed?

asked Jan 22 in Inorganic Chemistry by MoseSiler86 (2.6k points)

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A chemistry student is given a 25 mL sample of a solution containing an unknown amount of sodium chloride. After adding excess silver nitrate solution to the sample, the student records the mass of the resulting precipitate to be 2.655 grams. Using mass balance calculations, determine the mass percentage of sodium chloride in the original solution.

asked Jan 22 in Analytical Chemistry by KristoferAck (2.1k points)

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A chemistry student is given a 10 mL sample of a solution containing chloride ions and sulfate ions, and is asked to determine the mass of each ion present in the sample. The student knows that the total mass of the solution is 12.25 g, and that the density of the solution is 1.225 g/mL. The student also knows that the mass percent of chloride ions in the solution is 5%, and the mass percent of sulfate ions is 10%. Using mass balance calculations, what is the mass of chloride ions and sulfate ions present in the sample?

asked Jan 22 in Analytical Chemistry by ChanteStroh (2.5k points)

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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 NoellaEtx177 (2.1k points)

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1 answer 55 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 RodolfoKello (2.4k points)

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1 answer 84 views

A chemistry student is asked to find the standard cell potential for the redox reaction: Mg(s) | Mg²⁺(aq, 0.1 M) || Cu²⁺(aq, 0.01 M) | Cu(s) Given that the standard potential for the reduction of Mg²⁺ is -2.37 V and for the reduction of Cu²⁺ is +0.34 V. The student should show how to calculate the cell potential and determine if the reaction will proceed spontaneously or not.

asked Jan 22 in ElectroChemistry by DeneseSteinm (2.6k points)

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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 Murray05Y450 (2.2k points)

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1 answer 50 views

A chemistry student is asked to determine the concentration of copper ions in a 500 mL solution of copper sulfate. The student has access to a balance, a pipette, and standard solutions of sodium hydroxide and sulfuric acid. Using the mass balance calculations, what is the concentration of copper ions in the solution?

asked Jan 22 in Analytical Chemistry by LeighBwb6800 (2.4k points)

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1 answer 53 views

A chemistry student is asked to determine the concentration of a particular compound in a sample of drinking water. The student collects a 100 mL water sample and adds a known amount of a standard solution containing the compound. After allowing the solution to equilibrate, the student measures the concentration of the compound in the new solution using a spectrophotometer, to be 0.0125 M. Assuming mass balance, calculate the concentration of the compound in the original drinking water sample.

asked Jan 22 in Analytical Chemistry by JodieGartrel (2.1k points)

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1 answer 51 views

A chemistry student has two containers, one with 25 grams of hydrogen gas and the other with 35 grams of oxygen gas. What mass of water can be produced when these two gases undergo a reaction and which gas is the limiting reactant?

asked Jan 22 in Chemical reactions by CesarForlong (2.7k points)

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1 answer 86 views

A chemistry student has mixed 0.1 mol of hydrochloric acid (HCl) with 0.2 mol of sodium hydroxide (NaOH). What is the pH of the resulting solution?

asked Jan 22 in Inorganic Chemistry by LaunaRxf8120 (2.0k points)

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1 answer 93 views

A chemistry student has a sample of an unknown compound containing carbon, hydrogen, and oxygen. The mass of the sample is 2.50 g. After combustion, the student finds that 1.80 g of carbon dioxide, 0.75 g of water, and 0.20 g of oxygen are produced. Using mass balance calculations, determine the empirical formula of the unknown compound.

asked Jan 22 in Analytical Chemistry by Hulda4183859 (2.3k points)

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1 answer 63 views

A chemistry student has 5 g of magnesium (Mg) and 10 g of hydrochloric acid (HCl) to react. What mass of magnesium chloride (MgCl2) will be produced? (Assuming the reaction goes to completion and all the reactants are used up)

asked Jan 22 in Chemical reactions by LorenzaOrell (2.8k points)

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1 answer 51 views

A chemistry student has 25g of sulfur and 30g of oxygen to produce sulfur dioxide. If the equation for the reaction is: S + O2 → SO2, what is the limiting reactant and how much sulfur dioxide will be produced?

asked Jan 22 in Chemical reactions by ElisabethWeo (2.6k points)

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1 answer 103 views

A chemistry student has 20 grams of sodium hydroxide and 25 grams of hydrochloric acid. What is the limiting reactant in the reaction and how much product can be formed? (Assuming the balanced equation is NaOH + HCl → NaCl + H2O)

asked Jan 22 in Chemical reactions by SherriBorell (2.1k points)

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1 answer 59 views

A chemistry student has 100 grams of ammonia and 50 grams of oxygen. What is the limiting reactant in the reaction if the balanced equation is:4NH3 + 3O2 → 2N2 + 6H2O And how much of the other reactant will be left over after the reaction is complete?

asked Jan 22 in Chemical reactions by MaynardErb58 (2.1k points)

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1 answer 54 views

A chemistry student has 10 grams of sulfur and 15 grams of oxygen. Given the balanced equation for sulfur dioxide formation, how much sulfur dioxide can they produce? Which reactant will be the limiting reactant and what is the amount of the excess reactant?

asked Jan 22 in Chemical reactions by ElidaHaskins (2.1k points)

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1 answer 85 views

A chemistry student has 10 grams of magnesium and 15 grams of oxygen gas to produce magnesium oxide. What is the limiting reactant and how much magnesium oxide can be produced?

asked Jan 22 in Chemical reactions by CedricNicker (3.3k points)

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