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A solution of 0.1 M AgNO3 was electrolyzed using a current of 0.5 A for 150 seconds. If 0.15 g of silver was deposited, what is the value of the Faraday constant?

asked Jan 22 in ElectroChemistry by FranY1408156 (2.2k points)

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A solution contains 0.1 M of an unknown ion X. The electrode potential of this ion X is measured to be +0.60 V versus the standard hydrogen electrode (SHE). Calculate the concentration of ion X in the solution using electrochemical methods.

asked Jan 22 in ElectroChemistry by VickeyBatema (1.9k points)

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A solution contains 0.05 mol of Cu^2+ ions. If a current of 0.5 A is passed through this solution for 15 minutes, what is the value of the Faraday constant?

asked Jan 22 in ElectroChemistry by TiaMuirden46 (2.3k points)

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A solution contains 0.05 M AgNO3 and 0.10 M KCl. A silver electrode is dipped in the solution and a potential of 0.53 V is measured against a standard hydrogen electrode. Calculate the concentration of Ag+ ions in the solution.

asked Jan 22 in ElectroChemistry by AntonyKnotts (1.8k points)

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1 answer 103 views

A solution containing two different dye molecules of different sizes (methyl blue and eosin) is kept in a glass tube. Using the knowledge of diffusion and transport phenomena, calculate the time required for the eosin molecules to diffuse to a distance of 10 cm from the source of the solution, if the diffusion coefficient of eosin is known to be 2.5 x 10^-10 m^2/s.

asked Jan 22 in Physical Chemistry by FinleyConsta (2.4k points)

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A solution containing 0.5 moles of potassium dichromate was electrolyzed with a current of 1.5 Amperes for 30 minutes. During the process, the final volume of the solution was found to be 250 mL. Calculate the value of the Faraday constant using this information.

asked Jan 22 in ElectroChemistry by CorneliusChi (1.6k points)

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1 answer 103 views

A solution containing 0.5 M of iron(III) ions and 0.5 M of thiocyanate ions is allowed to reach equilibrium. If the equilibrium constant of the formation of the FeSCN2+ complex ion is 3.0 x 10^3, calculate the concentration of FeSCN2+ complex ion at equilibrium when the initial concentration of thiocyanate ions is doubled.

asked Jan 22 in Chemical equilibrium by BoydHaynes98 (1.9k points)

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A solution containing 0.1 M acetic acid and 0.1 M sodium acetate has a pH of 4.5. If 0.02 moles of hydrochloric acid is added to the solution, what will be the pH of the solution after equilibrium is reached? (Given pKa of acetic acid = 4.76)

asked Jan 22 in Chemical equilibrium by RoderickKyle (2.4k points)

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1 answer 117 views

A small metal block is placed in a beaker containing boiling water. The block initially weighs 50 grams and its temperature is 25°C. After 5 minutes, its weight is 49 grams and its temperature is 80°C. Determine the entropy change of the metal block during this process assuming it to be irreversible.

asked Jan 22 in Physical Chemistry by DelorasGaise (1.9k points)

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A sealed vessel contains a mixture of nitrogen dioxide and dinitrogen tetraoxide gases in equilibrium. If the volume of the container is increased, would the equilibrium shift towards more or less NO2? Calculate the new equilibrium constant at the new volume assuming the pressure and temperature remain constant.

asked Jan 22 in Chemical equilibrium by KreogMoore5 (6.4k points)

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A sample problem for a chemistry student to solve from the subtopic Calculating the effect of changing the temperature on the equilibrium constant could be: What would be the new equilibrium constant (Kc) for the reaction 2NOCl (g) ↔ 2NO (g) + Cl2 (g) at 400 K, if the initial equilibrium constant at 300 K is 2.50 x 10^-3? Given that the enthalpy change of the reaction (∆H) is -91.84 kJ/mol and the entropy change of the reaction (∆S) is -188.8 J/mol K.

asked Jan 22 in Chemical equilibrium by WalterC19362 (2.4k points)

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1 answer 97 views

A sample of unknown concentration of iron (Fe) is being analyzed using spectrophotometry. The absorbance values obtained from the analysis are: 0.3, 0.6, and 0.9. Using Beer's law, determine the concentration of iron in the sample.

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

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A sample of nitrogen dioxide is placed in a container at 250°C and 1 atm, where it decomposes according to the following equation: 2NO2(g) ↔ 2NO(g) + O2(g)The initial concentration of NO2 is 0.10 M, and the equilibrium constant (Kc) at this temperature is 4.0 x 10^-3. If the volume of the container is suddenly decreased to one-half of its original volume, causing the pressure to double, what will happen to the amount of NO and O2 present at equilibrium? Calculate the new equilibrium concentrations of NO and O2.

asked Jan 22 in Chemical equilibrium by MarcellaMack (1.7k points)

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A sample of gas at 25°C and 2 atm is expanded suddenly against a constant external pressure of 1 atm. Calculate the change in entropy of the gas as it expands irreversibly.

asked Jan 22 in Physical Chemistry by SommerBartos (1.8k points)

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1 answer 165 views

A sample of drinking water from a local source was analyzed for its composition using mass balance calculations. The sample was found to contain 100 mg/L of calcium ions, 50 mg/L of magnesium ions, 20 mg/L of chloride ions, and 10 mg/L of sulfate ions. If the total volume of the sample was measured to be 50 mL, what is the mass of each ion present in the sample?

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

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1 answer 203 views

A sample of argon gas is contained in a container kept at constant volume. The temperature of the gas is slowly increased by step-wise increments. The energy absorbed by the sample at each increment is recorded, and the average energy of the gas at each temperature is calculated. Using this data, the student is asked to determine the heat capacity of the gas at constant volume and explain why this value only depends on the temperature of the system.

asked Jan 22 in Physical Chemistry by MarianCocket (2.0k points)

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1 answer 97 views

A sample of an unknown inorganic compound weighing 6.25 grams was analyzed to determine its empirical and molecular formulas. After combustion, the sample produced 9.375 grams of carbon dioxide and 3.125 grams of water. What is the empirical and molecular formula of the inorganic compound?

asked Jan 22 in Inorganic Chemistry by IolaHolly818 (2.0k points)

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1 answer 143 views

A sample of an unknown inorganic compound contains 44.44% magnesium, 22.22% sulfur, and 33.33% oxygen by mass. Determine the empirical formula of the compound. If the molar mass of the compound is 120 g/mol, what is its molecular formula?

asked Jan 22 in Inorganic Chemistry by DeloresKuhn6 (2.1k points)

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1 answer 97 views

A sample of an unknown compound was analyzed using elemental analysis, and the results showed that the compound contains 12.8% hydrogen, 49.2% carbon, and 38.0% oxygen by mass. What is the empirical formula of the compound?

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

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1 answer 225 views

A sample of an inorganic compound contains 51.28% sodium, 21.44% sulfur, and 27.28% oxygen by mass. Determine the empirical formula of the compound.

asked Jan 22 in Inorganic Chemistry by YVMCinda4278 (2.3k points)

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