A 5.00-g sample of solid BaCI2 •2H2O was heated such that the water turned to steam and was driven off. Assuming ideal behavior, what volume would that steam occupy at 1.00 atm and 100.0 C?
The combustion of octane, C6H15, proceeds according to the reaction 2 C8H18 (l) + 25 O2 (g) --> 12CO2 (g) + 18 H2O (l)If 5.70 x 10^2 mol of octane combusts, what volume of carbon dioxide is produced at 36.0 c and 0.995 atm?
Part AIf 50.0 L of hydrogen chloride gas reacts with 10.0 L of oxygen gas, what is the volume of chlorine gas produced? Assume all gases are at the same temperature and pressure. HCl (g) + O2 (g) → Cl2 (g) + H2O (g) Express your answer with the appropriate units.
A baker uses sodium hydrogen carbonate (baking soda) as the agent in a banana-nut quickbread. The baking soda decomposes according to two possible reactions. Reaction 1: 2NaHCO3(s) → Na2CO3(s) + H2O(l) + CO2(g) Reaction 2: NaHCO3(s) + H+(aq) → H2O(l) + CO2(g) + Na+(aq) Calculate the volume (in mL) of CO2 that forms at 220 °C and 0.906 atm per gram of NaHCO 3 by each of the reaction processes.
Enter your answer in the provided box.Xenon hexafluoride was one of the first noble gas compounds synthesized. The solid reacts rapidly with the silicon dioxide in glass or quartz containers to form liquid XeOF4 and gaseous silicon tetrafluoride. What is the pressure in a 0.500-L container at 25°C after 3.05 g of xenon hexafluoride reacts? (Assume that silicon tetrafluoride is the only gas present and that it occupies the entire volume.)
A mixture of oxygen and nitrogen gases is maintained in a 9.63 L flask at a pressure of 137 atm and a temperature of 15 C. If the gas mixture contains 6.66 grams of oxygen, the number of grams of nitrogen in the mixture is g.
How many milliliters of oxygen gas at STP are released from heating 2.90 g of mercuric oxide?2HgO(s) → 2 Hg (l) + O2 (g)Express your answer with the appropriate units.
Calculate the mass in grams of hydrochloride produced when 5.35 L of molecular hydrogen measured at STP reacts with an excess of molecular chlorine gas.H2(g) + Cl2(g) → 2HCl(g) g
A 2.95 - g sample of an unknown chlorofluorocarbon is decomposed and produces 583 mL of chlorine gas at a pressure of 750 mm Hg and a temperature of 298 K. What is the percent chlorine (by mass) in the unknown chlorofluorocarbon?
Consider the following reaction:2SO2(g) + O2(g) → 2SO_s(g)If 285.3 mL of SO2 is allowed to react with 167.3 mL of O2 (both measured al 321 K and 53.2 mmHg), what is the limiting reactant?What is the theoretical yield of SO3?If 174.2 mL of SO3 is collected (measured at 321 K and 53.2 mmHg), what is the percent yield for the reaction?
Consider the following reaction. H2 (g) + I2 (s) → 2HI (g) If the cylinder with a movable piston below contains 1 mol H2(g) and 1 mol I2(s), which represents the cylinder after the reaction is complete?
The ideal gas law PV = nRT relates pressure P, volume V, temperature T, and number of moles of a gas, n. The gas constant R equals 0.08208 L middot atm/(K • mol) or 8.3145 J/(K • mol). The equation can be rearranged as follows to for n: n = PV/RT This equation is useful when dealing with gaseous because calculations involve mole ratios. Part AWhen heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3 → CaO + CO2 What is the mass of calcium carbonate needed to produce 63.0 L of carbon dioxide at STP? Express your answer with the appropriate units.
Assume that a single cylinder of an automobile engine has a volume of 524 cm2.Part AIf the cylinder is full of air at 72 °C and 0.990 atm, how many moles of O2 are present? (The mole fraction of O2 in dry is 0.2095)Part BHow many grams of C8 H18 could be combusted by this quantity of O2, assuming combustion with formation of CO2 and H2O?
Hydrogen and iodine gases react to form hydrogen iodide gas as follows: H2 (g) + I2 (g) → 2HI (g) At a certain temperature and pressure 1.4 L of H 2 reacts with 1.4 L of I 2. If all the H2 and I2 are consumed, what volume of HI, at the same temperature and pressure, will be produced?
Enter your answer in the provided box. Ammonium nitrate, a common fertilizer, is used as an explosive in fireworks and by terrorists. It was the material used in the tragic explosion at the Oklahoma City federal building in 1995. How many liters of gas at 307°C and 1.00 atm are formed by the explosive decomposition of 20.7 kg of ammonium nitrate to nitrogen, oxygen, and water vapor?
Three moles of glyceryl trioleate (triolein) are completely hydrogenated. How many moles of hydrogen are required?
Lithium reacts with nitrogen gas according to the following reaction: 6Li(s)+ N2 (g) → 2Li3N(s) What mass of lithium is required to react completely with 58.6 mL of N2 gas at STP?Express your answer in grams.
Chlorine gas is collected from the following reaction of MnO2(s) with HCl:MnO2(s) + 4HCl(aq) → MnCl2(aq) + Cl2(g) + 2H2O(l) Calculate the volume of HCl solution (1.0 M) needed to produce 5.0 x 103 mL of Cl2 at 1.0 atm and 300K. a. 203 mL b. 51 mL c. 812 mL d. 102 mL e. none of the above
What is the total volume of all gases that are produced when 32.0 mL of C3H5(NO3)3 reacts as shown in the reaction below. Assume standard temp and pressure. (d = 1.60 g/mL, molar mass 227.10 g/mol) 4C3H5(NO3)3 (I) → 6N2(g) + O2(g) + 12CO2(g) + 10H2 (g).
When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2AI (s) + 6HCI(aq) → 2AICI3(aq) + 3H3(g) What volume of H2(g) is produced when 5.40 g of Al(s) reacts at STP?
Ammonium carbonate decomposes upon heating according to the following balanced equation: (NH4)2CO3 (s) → 2 NH3 (g) + CO2 (g) + H2O (g) Calculate the total volume of gas produced at 20.0°C and 1.03 atm by the complete decomposition of 11.8 g of ammonium carbonate.
Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al (s) + 3O2 (g) → 2Al2O3 (s) What volume of O2 gas (in L) measured at 795 mmHg and 27°C, is required to completely react with 53.5 g of Al?
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO2 (s) + 4HCl (aq) → MnCl2 (aq) + 2 H2O (l) + Cl2 (g) How much MnO2(s) should be added to excess HCl(aq) to obtain 225 mL of Cl2(g) at 25° and 715 Torr?
Limestone (CaCO3) reacts with hydrochloric acid according to the equation: CaCO 3 + 2HCl → CaCl2 + H2O + CO2 If 1.00 mol of CO2 has a volume of 22.4 L under the reaction conditions, how many liters of gas can be formed by reaction of 2.30 g of CaCO3 with 2.30 g of HCl? Which reactant is limiting? a. limestoneb. hydrochloric acid
How many grams of carbon disulfide are needed to completely consume 53.3 L of chlorine gas according to the following reaction at 25°C and 1 atm? carbon disulfide (s) + chlorine (g) → carbon tetrachloride (l) + sulfur dichloride (s)
For each of these equations, determine the change in the number of moles of gas, Δngas. (a) (NH4)2CO3 (s) → 2NH3 (g) + CO2 (g) + H2O (g) (b) H2 (g) + Cl2 (g) → 2HCl (g) (c) 2H2 (g) + O2 (g) → 2 H2O(l) (d) 2Na (s) + Cl2 (g) → 2NaCl (s)
The combustion of octane, C8H18, proceeds according to the reaction 2C8H18 (l) + 25O2 (g) → 16CO2 (g) + 18H2O (l)lf 546 mol of octane combusts, what volume of carbon dioxide is produced at 16 0°C and 0.935 atm?
The combustion of octane, C8H18 proceeds according to the reaction 2C8H18 (l) + 25O2 (g) → 16CO2 (g) + 18H2O (l) If 313 mol of octane combusts, what volume of carbon dioxide is produced at 39.0°C and 0.995 atm?
When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2 Al (s) + 6HCl (aq) → 2 AICI3 (aq) + 3H2 (g) What volume of H2 (g) is produced when 8.40 g of Al (s) reacts at STP?
When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2AI (s) + 6HCl (aq) → 2AICl3 (aq) + 3H2 (g) What volume of H2(g) is produced when 7.10 g of Al(s) reacts at STP?
Oxygen gas reacts with powdered aluminum according to the following reaction 4Al(s) + 3O2(g) → 2Al2O3(s)What volume of O2 gas, measured at 765 mmHg and 22°C, is required to completely react with 53.0 g of Al? Express the volume in liters to three significant figures.
The total volume of hydrogen gas needed to fill the Hinderburg was 2.00 x 108 L at 1.00 atm and 25.0°C. How much energy was evolved when it burned?Hint-Use the Ideal Gas Law to obtain the moles of hydrogen gas. 2H2 (g) + O2 (g) → 2H2O (l) ΔH = -572 kJa. 2.86 x 104 kJb. 5.72 x 1010 kJc. 8.18 x 106 kJd. 35 x 1011 kJ e. 2.34 x 109 kJ
Part AWhat is the volume occupied by 14.1 g of argon gas at a pressure of 1.20 atm and a temperature of 400 K? Express your answer with the appropriate units. Part B Compare the volume of 14.1 g of helium to 14.1 g of argon gas (under identical conditions). • The volume would be the same for helium gas. • The volume would be greater for helium gas. • The volume would be lower for helium gas.
Part AWhat volume of O2 at 836 mmHg and 41°C is required to synthesize 13.5 mol of NO? Express your answer numerically in liters.
The combustion of octane, C8H18, proceeds according to the reaction 2C8H18 (l) + 25O2 (g) → 16CO2 (g) + 18H2O (l) If 579 mol of octane combusts, what volume of carbon dioxide is produced at 34.0°C and 0.995 atm?
Reaction vessel contains 6.1 g of CO and 6.1 g of O2. How many grams of CO2 could be produced according to the following reaction?2 CO + O2 → 2 CO2
A miniature volcano can be made in the laboratory with ammonium dichromate. When ignited, it decomposes in a fiery display. (NH4)2Cr2O7 (s) → N2 (g) + 4H2O (g) + Cr2O3 (s) If 0.76 g of ammonium dichromate is used, and the gases from this reaction are trapped in a 15.1 L flask at 29°C, what is the total pressure of the gas in the flask? What are the partial pressures of N2 and H2O?
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2 (g) + 3F2 (g) → 2CIF3 (g) A 2.05 L reaction vessel, initially at 298 K, contain chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 811 mmHg.Identify the limiting reactant and determine the theoretical yield of CIF3 in grams. Express your answer with the appropriate units.