Inorganic Chemistry Questions

To make rust-resistant, a jewelry is electroplated by tin (Sn). Molar mass of Sn is 118.710 g/mol. The half-reaction related to this process is shown below: Sn2+ (aq) + 2e¯→ Sn(s) How much time in seconds would it take for 325 mg of Sn to be plated at a current of 4.7 A?

Consider the reactions 1. C(graphite) + O2(g) →> CO2(g) ΔHxn=-393.5 kJ 2. H2(g) + 1/2O2(g) -> H₂O(1) ΔHOrxn=-285.8 kJ 3. 2 C2H2(g) + 5 O2(g) -> 4 CO2(g) + 2 H₂O0) ΔHºrn = -2598.8 kJ Calculate the ΔHOrxn for the reaction: 2 C(graphite) + H2(g) -> C2H2(g) ΔHᵒrn = ???

Given that zinc reacts with iodine in the fixed mass ratio of 1 gram of zinc to 3.88 grams of iodine, how many grams of iodine are required to completely react with 4.2 grams of zinc? The unit conversion you will use here is: grams of Zinc/ grams of iodine Fill in the blanks to set up the problem mathematically: 4.2 g of zinc x grams of grams number of grams of zinc required= Type your answer here

Consider the following two cases: Case 1: 1 g of carbon + 1.33 g of oxygen = 1 mole of carbon monoxide Case 2: 1 g of carbon + 2.66 g of oxygen = 1 mole of carbon dioxide Why is that in the second case when we doubled the amount of oxygen we don't get double the amount of carbon monoxide and instead we make one mole of CO₂? To form one mole of CO2, we need to (keep/double) the C amount and you need to (keep/double) the amount of Owith respect to the amount of C and O in CO. To form two moles of CO, we need to (keep/double) the C amount and you need to (keep/double) the amount of O.

Calculate the pH of a 0.321 M solution of NaNO₂. The ionization constant, K₁, for the acid, HNO₂, is 4.60 × 10^-4.

In an experiment, magnesium sulfate heptahydrate, Epsom salt, is heated to a constant mass. What is the best representation of what happened in this experiment? 1. MgSO4 (byd) → MgSO4(gnhyd) 2. magnesium sulfate heptahydrate → anhydrous magnesium sulfate 3. MgSO.7H₂O → MgSO, + 7 H₂O 4. MgSO.H₂O(s) → MgSO.(s) + H₂O(g)

Upon combustion, an unknown compound containing only carbon and hydrogen produces 39.86 g carbon dioxide and 8.16 g water. Determine the empirical formula of the unknown compound. C3H2 CH C₂H CH₂ C3H

Consider the reaction. 2 CO(g) + Oz(g) -> 2 CO2(g) ΔH = -566.0 kJ a) Is the reaction exothermic of endothermic? b) 2.80 g of CO let to react with excess of O2. How much heat will be released or absorbed by the system?

150. mL of 0.350 M HCI was mixed with 150. mL of 0.350 M NaOH in a calorimeter (of negligible heat capacity). The initial temperature of the HCI and NaOH solutions was the same, 23.25°C, and the final temperature of the mixed solution was 25.60°C. Calculate the heat of neutralization for the reaction: NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O) dsol = 1.00 g/mL; S.H.sol = 4.184 J/g °C

The chemical formula for calcium hydroxide is: Ca(OH)₂ Calculate the molar mass of calcium hydroxide. Round your answer to 2 decimal places.

The chemical formula for beryllium sulfide is BeS. A chemist determined by measurements that 0.0200 moles of beryllium sulfide participate in a chemical reaction. Calculate the mass of beryllium sulfide that participates. Round your answer to 3 significant digits.

Calculate the mass of dinitrogen tetroxide (N₂O4) that contains a million (1.0 × 106) nitrogen atoms. Be sure your answer has a unit symbol if necessary, and round it to 2 significant digits.

The chemical formula for methanol is: CH3OH Calculate the molar mass of methanol. Round your answer to 2 decimal places.

A chemist determined by measurements that 0.040 moles of potassium participated in a chemical reaction. Calculate the mass of potassium that participated in the chemical reaction. Round your answer to 2 significant digits.

Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. C(s) + H₂(g) → C₂H6 (g)

The chemical formula for cesium chloride is CsCl. A chemist measured the amount of cesium chloride produced during an experiment. She finds that 97.9 g of cesium chloride is produced. Calculate the number of moles of cesium chloride produced. Round your answer to 3 significant digits.

While Bayer is often credited with the commercialization of Aspirin (an chemical modification of a compound found in the Willow Tree bark) as a pain reliever medication. Indigenous Americans actually discovered the pain relieving properties of the Willow Tree long before Bayer. A compound extracted from Willow Bark was subjected to Elemental Analysis and the following mass data were collected: C: 60.87% H: 4.38% O: 34.75% Based on this information, what is the empirical formula of this compound?

Fill in the systematic names of the following chemical compounds. Note: for compounds containing hydrogen, you may give the common name instead.

What is the balanced equation for the combustion of pentane when the equation is balanced with the smallest, whole numbers possible? 2 C5H12 +11 O2→ 10 CO + 12 H2O C5H12 +8O₂ --> 5 CO₂ + 6H₂O C5H1₂ →5C+ 6H₂ C5H12+5O2 → 5CO2+6H2 I DON'T KNOW YET

What is the correct structure for 3-fluoro-2,2-dimethylpentane?

This is the chemical formula for zinc bromate: Zn(BrO3)₂ Calculate the mass percent of oxygen in zinc bromate. Round your answer to the nearest percentage.

For each reaction in the table below, write the chemical formulae of any reactants that will be oxidized in second column of the table. Write the chemical formulae of any reactants that will be reduced in the third column.

100.0 mL of 1.35 M HCI solution is mixed with 650.0 mL of distilled water. What is the final solution's concentration? Hint: Don't forget to use the new solution's total volume. 0.208 M HCI 8.78 M 0.180 M 2.27 M

Determine the number of atoms that bear non-zero formal charges in the Lewis structure given below exactly as it is depicted.

Ammonia gas reacts with oxygen gas, O₂ (g), to produce nitrogen dioxide and water. When 32.4 g of ammonia gas reacts with 87.3 g of oxygen gas to produce 64.5 g of nitrogen dioxide, what is the percent yield for the reaction? For the hydrogen atom, H, you must use a molar mass of 1.008 g/mol in your calculations and for the nitrogen atom, N, use a molar mass of 14.01 g/mol in your calculations. Do NOT include units in your answer. Do not include "%" in your answer. If you round during your calculation, be sure to keep at least three (3) decimal places. Report your answer to one (1) decimal place.

Scientists can analyze metals using the emission spectrum produced when the sample is introduced into the flame of an emission spectrometer. The flame provides the energy to excite the electrons of the metal atoms to higher energy states. When the electrons return to the ground state, lines of characteristic wavelengths are produced. The lines in the emission spectrum are characteristic of the metal because each atom's ground-state electron configuration is unique. The emission line used for zinc determinations in atomic emission spectroscopy is 214 nm. If there are 9.00x10¹0 atoms of zinc emitting light in the instrument flame at any given instant, what energy (in joules) must the flame continuously supply to achieve this level of emission? Express your answer numerically in joules. During an emission, electrons move from a higher energy orbital to a lower energy orbital. Which of the following are valid transitions that produce lines in the emission spectrum of Zn?

How many non-bonding electrons are on the central atom in the optimized Lewis structure of OBr2, in which the formal charges are minimized?

By titration, it is found that 63.1 mL of 0.194 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.

What is the concentration of copper ions in an aqueous solution that is 2.0 M Cu₂SO4? (2 significant figures) Hint: How many copper ions does one formula unit produce? a. 1.0 M Cu b. 2.0 M Cut c. 4.0 M Cu+ d. 0.5 M Cu

The angle between the fluorines in PF3 are smaller than the angles between the fluorines in CF4, even thoughthey both have four pairs of electrons around the central atom. Explain why the fluorines are being pushed a little closer together in PF3 than they are in CF4

A stock solution containing Mn²+ ions was prepared by dissolving 1.861 g pure manganese metal in nitric acid and diluting to a final volume of 1.000 L. The following solutions were then prepared by dilution: For solution 4, 40.00 mL of stock solution was diluted to 1000.0 mL. For solution B, 20.00 mL of solution A was diluted to 250.0 mL. For solution C, 10.00 mL of solution B was diluted to 550.0 mL. Calculate the concentration of the stock solution.

Biphenyl, C₁2H10 , is a nonvolatile, nonionizing solute that is soluble in benzene, C6H6. At 25 °C, the vapor pressure of pure benzene is 100.84 Torr. What is the vapor pressure of a solution made from dissolving 12.1 g of biphenyl in 33.9 g of benzene?

One serving (25 grams) of sour cream and onion potato chips contains 9 g of fat, 14 g of carbohydrates, and 2 g of protein. Estimate the number of calories. [Hint: One gram of protein or one gram of carbohydrate typically releases about 4 Cal/g, while fat releases 9 Cal/g.] Report your answer to 1 significant figure.

8. Balance the following redox reaction if it occurs in neutral solution. What are the coefficients in front of Ti²+ (aq) and Fe2+ (aq) in the balanced reaction? Ti²+ (aq) +Fe³+ (aq) → Ti4+ (aq) + Fe²+ (aq) D) 3 and 1 A) 1 and 2 B) 2 and 1 C) 2 and 2 E) 1 and 3

How many milliliters of 9.39 M nitric acid solution should be used to prepare 3.50 L of 0.300 M HNO3?

In the laboratory you dissolve 20.8 g of lead(II) nitrate in a volumetric flask and add water to a total volume of 375 mL. What is the molarity of the solution? What is the concentration of the lead cation? What is the concentration of the nitrate anion?

Solid Mass: 2.51 g What is the volume of the solution, in liters? amount added: 0.0129 mol

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. a. 0.400 mole of Ca (NO3)2 in 300.0 mL of solution b. 1.5 moles of Na2SO4 in 2.00 L of solution c. 9.70 g of NH4Cl in 970.0 mL of solution d. 4.20 g of K3PO4 in 810.0 mL of solution

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. (Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit.) a. iron(III) chloride and sodium hydroxide b. silver nitrate and ammonium selenate c. copper(II) sulfate and barium nitrat d. calcium nitrate and cesium iodide

In the laboratory you dissolve 24.3 g of potassium carbonate in a volumetric flask and add water to a total volume of 250 mL. What is the molarity of the solution? What is the concentration of the potassium cation? What is the concentration of the carbonate anion?

When aqueous solutions of zinc iodide and potassium phosphate are combined, solid zinc phosphate and a solution of potassium iodide are formed. The net ionic equation for this reaction is:

You wish to make a 0.316 M perchloric acid solution from a stock solution of 6.00 M perchloric acid. How much concentrated acid must you add to obtain a total volume of 75.0 mL of the dilute solution?

The compound ammonium cyanide is a strong electrolyte. Write the reaction when solid ammonium cyanide is put into water. Include states of matter in your answer.

A chemist must dilute 91.4 mL of 445. mM aqueous potassium dichromate (K₂Cr₂O7) solution until the concentration falls to 57.0 mM . She'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Round your answer to 3 significant digits.

A chemist adds 275.0 mL of a 3.4M potassium iodide (KI) solution to a reaction flask. Calculate the mass in kilograms of potassium iodide the chemist has added to the flask. Round your answer to 2 significant digits.

Calculate the volume in liters of a 0.12M barium chlorate solution that contains 425. mmol of barium chlorate (Ba(CIO3)₂). Round your answer to 2 significant digits.

Iron concentrations greater than 6.30×10-6 M in water used for laundry purposes can cause staining. What [OH-] is required to reduce Fe2+ to this level by precipitation of Fe(OH)2? (Ksp = 8.0x10-16)

Diborane (B₂H6) is a gas at room temperature that forms explosive mixtures with air It reacts with oxygen according to the following equation B2H6(g) +302 (g) --> B2O3(s) + 3H₂O(l) How many grams of diborane will react with 8.0 mol of O₂? Express your answer to two significant figures and include the appropriate units.

A chemist prepares a solution of zinc nitrate (Zn(NO3)₂) by measuring out 113. μmol of zinc nitrate into a 300. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in μmol/L of the chemist's zinc nitrate solution. Round your answer to 3 significant digits.

A chemist prepares a solution of magnesium fluoride (MgF₂) by measuring out 0.00399 μmol of magnesium fluoride into a 100. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mmol/L of the chemist's magnesium fluoride solution. Round your answer to 3 significant digits.