General Questions and Answers

Gaseous ethane (CH3CH3) will react with gaseous oxygen (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). Suppose 1.5 g of ethane is mixed with 9.91 g of oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 2 significant digits.

The following chemical reaction takes place in aqueous solution: Zn(NO3)2(aq) + (NH4)₂S (aq) → ZnS (s) + 2NH4NO3(aq) Write the net ionic equation for this reaction.

According to the following reaction: 3KOH(aq) + H₂PO4 (aq) - → K3PO4 (aq) + 3H₂O (1) What would you multiply "grams of potassium hydroxide" by to convert to the units "moles of phosphoric acid" ?

A 0.225 M solution of a weak monoprotic acid (HA) has a pH of 4.34. What is the value of K of this acid? K = Percent Ionization What is the percent ionization of this acid? = %

A 66.0 mL portion of a 1.50 M solution is diluted to a total volume of 248 mL. A 124 mL portion of that solution is diluted by adding 135 mL of water. What is the final concentration? Assume the volumes are additive.

How many unpaired electrons are found in a ground state atom of Fe?

Calories are used as a nutritional measurement for food. Based on your findings for energy content per gram, which snack foods give the maximum calories? Does this support your prediction?

20 g of magnesium reacts with hydrochloric acid, generating hydrogen gas according to the reaction below. The hydrogen gas is collected over water. Mg(s) + 2HCl(aq) → MgCl2 (aq) + H₂(g) If 2.97 L of hydrogen gas is collected at 760.0 mmHg and 20°C, what was the percent yield of the reaction?

A fixed container containing an ideal gas is heated. The pressure of the gas increases because A) the gas molecules move faster and strike the walls of the container more often and with more force. B) the gas molecules slow down, striking the walls of the container less often and with less force. C) the gas molecules begin sticking together other and strike the walls of the container with twice the force. D) the gas molecules will melt and fall to the bottom of the container. E) the gas molecules will no longer behave ideally.

How many moles of NH, gas form when 32.4 L of H₂ gas completely reacts at STP according to the following reaction? Remember 1 mol of an ideal gas has a volume of 22.4 L at STP. N₂(g) + 3 H₂(g)---> 2 NH3(9)

What is the volume (in L) of carbon dioxide at 1.00 atm and 298.15 K are released from a car's engine upon consumption of a 60.0 L LIQUID tank gasoline? (Gasoline density: 0.770 kg/L, Molar mass of C8H18: 114.2 g/mol) C8H18 (1) +2^5 i2 O₂ (g) → 8 CO₂ (g) + 9 H₂O (g)

15.0 L of an ideal gas at 298 K and 3.36 atm are heated to 383 K with a new pressure of 6.00 atm. What is the new volume in liters?

When chromium metal is added to nitric acid, the following reaction takes place Cr (s) + 6 HNO3(aq) → Cr(NO3)3 (aq) + 3 H₂O (1) + 3 NO₂ (g) Calculate the volume of NO₂ gas (in L) collected over water at 40.0 °C when 11.1 g of chromium is added to excess nitric acid if the total pressure is 675.0 torr. The vapor pressure of water at 40.0 °C is 55.3 torr.

Convert 532 torr to kPa. Remember that multiple steps may be required in the conversion.

At STP, 10.00 mol of gas occupies approximately what volume in litres? R= 0.08314 L bar/mol.K.

A house is designed to have passive solar energy features. Brickwork is to be incorporated into the interior of the house to act as a heat absorber. Each brick weighs approximately 1.8 kg. The specific heat of the brick is 0.85 J/g. K. How many bricks must be incorporated into the interior of the house to provide the same total heat capacity as 1500 gal of water? Express your answer using two significant figures.

Calcium carbonate, CaCO3, decomposes when heated to calcium oxide (CaO) and carbon dioxide (CO₂). If 100 g of calcium carbonate is allowed to decompose, 56 g of calcium oxide is produced. What mass of carbon dioxide is produced by the decomposition?

What is the molarity (M) of a solution that is made with 35.7 grams (g) of NaOH with a final volume of 480.0 mL?

A 0.279 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H₂SO4 (aq) → MSO4 (aq) + H₂(g) A volume of 291 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal.

What pressure in mmHg is equivalent to 1.350 atm?

Enter a balanced equation for the reaction of NaCH3COO (so written as NaC₂ H₂O₂) and HCl.

Predict the products and enter a balanced equation for each of the following. Combination: Ca(s) + Br2 (g)→

Draw the Lewis structure of acetic acid (CH3COOH) and then choose the appropriate set hybridization states for the three central atoms. Your answer choice is independent of the orientation of your drawn structure.

Write a balanced equation for reaction: Solid copper (II) oxide and solid aluminium metal react to form copper metal and solid aluminium oxide.

+ Draw the Lewis structure of CH3NCO and then choose the appropriate set of hybridization states for the three central atoms. Your answer choice is independent of the orientation of your drawn structure. Click to draw a new structure A) sp³ / sp² / sp B) sp³ / sp² / sp² C) sp³ / sp³ / sp³ D) sp / sp² / sp E) sp³/sp/sp

How many grams of aluminum oxide (Al2O3) can be roduced from 22 grams of oxygen in the reaction below? 4 Al+30₂ - 2 Al₂O3

You may want to reference (Page) Section 8.3 while completing this problem. Predict the products and enter a balanced equation for each of the following. Part A Decomposition: NaCl(s)→→____+.

In the following diagram, if red spheres are the element A, white spheres are the element B, and green spheres are the element C: Write a balanced equation for the reaction.

Balance each of the following chemical equations, and identify the type of reaction: Mg(s) + N₂(g) → Mg3N2 (s) Express your answer as a chemical equation. Identify all of the phases in your answer. Submit AΣO A chemical reaction does not occur for this question. Part D Request Answer Identify the type of the reaction from part C. combination ? O decomposition O single replacement O double replacement O combustion Review | Constar

Write the correct formulas for the products for reaction: Solid copper (II) nitrate is heated and forms solid copper (II) oxide, gaseous nitrogen (IV) oxide, and oxygen gas.

An ionic isotope has 49 protons, 50 electrons, and 55 neutrons. ▪ What is the name of the element? What is the isotope symbol in the one-line format (e.g., hydrogen-2)? Is this a cation or is this an anion? Explain how you know. ■

When 1.00-gram sample of baking soda is heated, a gas is formed. The solid that remains weighs less than 1.00 g and does not have the same properties as the original sample. Is baking soda an element or compound? Justify your answer from the description given.

Write a balanced equation for reaction: Propene gas (C3H6) reacts with oxygen gas to form two gaseous products: carbon dioxide and water. Express your answer as a chemical equation. Identify all of the phases in your answer. A chemical reaction does not occur for this question. Part L Request Answer Identify the type of reaction above. combustion combination decomposition single replacement double replacement

The following equation is balanced. State the number of atoms of each element in each side. 2Na(s) + Cl₂ (g)→2NaCl(s)

A chemist adds 38.9 g of magnesium bromide to 1.50 L of a solution that has a concentration of 0.209 M bromide ions. What is the final concentration of bromide ions? Assume the volume does not change when the solid magnesium bromide is added.

Prelaboratory Assignment 1. a. What is the law of definite proportions, and how does it apply to this experiment? b. What is a mole and what is a molar mass? What are the molar masses of magnesium and atomic oxygen? C. Why is magnesium the limiting reactant (Ebbing/Gammon, Section 3.8) in this experiment?

A 25 mL solution of 0.15 M NaCl is mixed with a 40 mL solution of 0.1 M Mg(ClO4)₂ What is the sodium ion concentration in the mixture? A) 0.15 M B) 0.25 M OC) 0.115 M D) 0.058 M E) 0.038 M

Many chemical reactions can be classified according to what the atoms or groups of atoms do during the reaction. The four types of classifications include synthesis (also called combination) reactions, decomposition reactions, single-displacement reactions, and double-displacement reactions. Classify the following reactions as synthesis, decomposition, single-displacement, or doubledisplacement reactions.

The amount of 2.00 g of NaCl and 4.00 g of AgNO3 are used in this experiment. According to the chemical equation NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) - a) Which one of the two compounds is the limiting reagent? NaCl b) What is the theoretical yield (to 2 decimal places in grams) of the previous question? c) If only 3.12 g of AgCl is collected from the experiment described in previous question, what is the percent yield (2 decimal places) of the experiment?

Given the compound of AuCI, where gold has only one isotope, 197 Au, and chlorine has two isotopes, 35Cl and 37 Cl. How many lines will be shown in the mass spectrum of this compound and what are the mass numbers for each of fragments? O2 lines of masses 232 and 234 4 lines masses 35, 37, 232, and 234 3 lines of masses 35, 37, and 197 5 lines of masses 35. 37, 197, 232, and 234 6 lines 35, 37.73, 197, 232, and 234

Decide how the sketches below would be listed, if they were listed in order of decreasing force between the charges. That is, select "1" beside the sketch with the strongest force between the charges, select "2" beside the sketch with the next strongest force between the charges, and so on. Note for advanced students: since the units of each charge are not written, you may assume any convenient and reasonable unit, for example coulombs or multiples of e.

Given the following combustion reaction: C6H12O6(s) + 6O2(g) → 6 CO₂(g) + 6 H₂O(g) and the enthalpy of formations in kJ/mol for each species are: C6H12O6(s) = -1273.3, CO₂(g) = -393.5, and H₂O(g) = -286.0 Determine the heat exchange (in kJ) when 43.1 g of C6H12O6(s) (molar mass = 180.16 g/mol) is burned in excess oxygen.

Suppose 5.41 g of potassium bromide is dissolved in 350. mL of a 65.0 m M aqueous solution of silver nitrate. Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the potassium bromide is dissolved in it. Round your answer to 3 significant digits.

If a sample had an absorbance of 0.333, what would be the concentration? If a sample had a concentration of 0.40 mg/ml, what would be the absorbance?

If the average 10-mL of the pipet is calculated to be 9.963 ± 0.034 mL, what is the average mass [in g] of water delivered by the pipet at each 10-mL increment at 30°C. Given the density of water at 30°C is 0.9956 g/mL.

How many atoms of hydrogen are in 35 g of C₂H6? 6.3 x 10^26 4.2x 10^24 7.0x10^23 12x10^23 11x10^26

How many moles of compound would be in 4.5 g Xe(CN), if this compound could form? 20.5 69.9 0.0682 0.0245 489 4.50 825

A 55.8 ml sample of a 0.103 M potassium sulfate solution is mixed with 37.8 mL of a 0.113 M lead (II) acetate solution and this precipitation reaction occurs. K₂SO4 (aq) + Pb(C₂H30₂)2 (aq)->2 KC ₂H3O₂ (aq) + PbSO4(s) The solid PbSO4 (molar mass=303 26 g/mol) is collected, dried, and found to have a mass of 1.10 g. Determine the theoretical yield in grams

A student was given the hydrate of potassium sulfide (K₂S). Following the procedure of the experiment the following data were recorded: Mass of sample before heating, g Mass of sample after heating, g Calculate the mass of the water lost during the heating. Calculate the moles of water lost during heating. Its Molecular Weight is 18.00 g/mol. Calculate the moles of anhydrous salt present. The formula weight of K₂S is 110.27 g/mol. Calculate the number of moles of water per mole of anhydrous salt in the hydrate. Write the formula of the hydrated salt:

If a compound is composed of 24.68 % N and 75.32 % F, then what is its empirical formula? Calculate the moles of N= Calculate the moles of F = What number must you multiply each ratio by in order to convert all decimals to whole numbers and get the empirical formula? Calculate the empirical formula. Put only whole numbers in the blanks.