If methane gas reacts with copper (II) oxide, it produces copper metal, carbon dioxide and water vapor. CH.p + CuO „ → Cu „ + CO:» + H,O » If 23.4 g of methane is treated with 18.5 g of copper (II) oxide, what volume of carbon dioxide and water vapor would be collected at 25.0°C and 790 mmHg. Write your final answer/s HERE! a) Balanced chemical equation b) Limiting reactant Volume of CO; |(write your answer here) |(write your answer here) (write your answer here) (write your answer here) c) Volume of water vapor

If methane gas reacts with copper (II) oxide, it produces copper metal, carbon dioxide and water vapor. CH.p + CuO „ → Cu „ + CO:» + H,O » If 23.4 g of methane is treated with 18.5 g of copper (II) oxide, what volume of carbon dioxide and water vapor would be collected at 25.0°C and 790 mmHg. Write your final answer/s HERE! a) Balanced chemical equation b) Limiting reactant Volume of CO; |(write your answer here) |(write your answer here) (write your answer here) (write your answer here) c) Volume of water vapor

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Gas jar Gas collects here Trough of water |Bee hive shelf Reaction mixture 2 NaCiO, > 2 Naci 3(s) 30 2(g) (s), A sample of NaCIO3 is partially decomposed by heating, producing O2 gas that is collected safely over water. The volume of total gas collected is 2.50 x 104 m³ at 26 °C, giving 102 kPa total pressure. How many grams of NaCIO3 were decomposed? What atom was oxidized? What atom was reduced? The pressure of water vapor at 26 °C is 25 torr. SHOW ALL WORK!
Could I have help with this chemistry question
Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. Suppose the O2 gas evolved by a certain chemical reaction taking place at 50.0°C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 76.9mL. Sketch of a gas-collection apparatus Calculate the mass of O2 that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. = g
a 2.802g sample of an unknown pure metal (M) is added to a 0.2 L solution of 2 mol/L H2SO4(aq). The metal reacts with the acid until the metal is completely gone to form M3+(aq) ion in the solution and produces hydrogen gas that is collected. The hydrogen gas that is collected over water that is isolated from the reaction has a volume of 0.82 L at 25 degrees Celsius and a total pressure of 704.0 mmHg. How many moles of H2(g) are produced? Write a balanced equation for the reaction of M with H2SO4(aq). What is the identity of metal M?
A 0.158-g sample of unknown metal, X, reacted with hydrochloric acid according to the following balanced reaction: 2 X (s) + 6HCl (aq) -> 2 XCl3 (aq) + 3 H2 (g) The volume of the hydrogen gas collected over water was 216 mL at 22 degress C and a barometer reading of 764 mm Hg (VP of water at 22 degrees C is 20. mm Hg) (a) Determine the molar mass of "X" knowing that the molar mass is grams per mole: 1) atomic mass of metal 2) identiy of unknown metal
Ethane burns in air to give h2o and o2 . 2c6h6+ 7o2= 4co2+ 6h2o What volume of o2 (L) is required for complete reaction with 6.8 L of c6h6 ? Assume all gases are measured at the same temperature and pressure. Volume = __L What volume of h2o vapor (L) is produced in the complete reaction of 6.8 L of c6h6 ? Assume all gases are measured at the same temperature and pressure. Volume =___ L
Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. Suppose the O2 gas evolved by a certain chemical reaction taking place at 35.0°C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 48.7mL. Sketch of a gas-collection apparatus Calculate the mass of O2 that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. = g
The compound Mg(ClO3)2 decomposes when heated according to the equation below. Mg(ClO3)2 (s) ➝ MgCl2 (s) + 3 O2 (g) An impure sample of material contains a small amount of Mg(ClO3)2 . The sample is heated and the gas produced collected by downward displacement of water. A total of 377.1 ml of gas is collected at a temperature of 20.0ºC when the atmospheric pressure is 740.0 torr. [The vapor pressure of water at 20.0ºC is 17.54 torr.]Calculate the number of grams of Mg(ClO3)2 present in the impure sample. Grams of Mg(ClO3)2 : Answer in grams
STP (standard temperature and pressure) is used as a reference point for the molar volume of an ideal gas. In the USA, most chemists, most general chemistry texts, and OWL use STP = 0°C, 1 atm, where the molar volume = 22.4 L/mol. If the reference pressure is chosen to be 1 bar, the molar volume is 22.7 L/mol. Do not confuse the two. A 0.580 mol sample of xenon gas occupies a volume of L at STP.
A piece of sodium metal reacts completely with water according to the reaction: 2Na(s) + 2H20(1) > 2NaOH(ag) + H2(8) The hydrogen gas is collected over water at 25°C. The volume of the gas generated is 246 mL at 760.0 mmHg. Calculate the volume of dry hydrogen gas that would be collected at STP. __ mL H2
Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCI(aq) ZnClą(aq) +H2(g) The product gas, H,, is collected over water at a temperature of 20 °C and a pressure of 755 mm Hg. If the wet H, gas formed occupies a volume of 6.66 L, the number of moles of Zn reacted was mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.
The combustion of octane, C, H g8, proceeds according to the reaction shown. 2C,H1g(1) + 25 0,(g) 16 CO, (g) + 18 H,O(1) If 562 mol of octane combusts, what volume of carbon dioxide is produced at 14.0 °C and 0.995 atm? V = L