During the production of ammonia, hydrogen is produced from the steam reforming of methane. In the reformer methane gas is reacted with excess water and the resulting mixture is found to contain 12 kg of hydrogen and 15 kg water. Assuming all the methane is reacted calculate the amount of water used.

During the production of ammonia, hydrogen is produced from the steam reforming of methane. In the reformer methane gas is reacted with excess water and the resulting mixture is found to contain 12 kg of hydrogen and 15 kg water. Assuming all the methane is reacted calculate the amount of water used.

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

Which of the following is the formation reaction for Na2CO3 (s)? A. 2 Na(s) + C(s, graphite) + 3 O(g) → Na2CO3(s) B. 4 Na(s) + 2 C(s, graphite) + 3 O2(g) → 2 Na2CO3(s) C. 2 Na(s) + C(s, graphite) + 1.5 O2(g) → Na2CO3(s) D. Na2(s) + C(s, graphite) + 1.5 O2(g) → Na2CO3(s) E. 2 Na(g) + C(g) + 1.5 O2(g) → Na2CO3(s)
packets of the anhydrous form of a hydrate are sometimes used to keep cellars from being damp. Is there a limit to how long a packet could be used?
2. An experiment to determine the carbon-sequestration capacity of a poui tree determined that in 1 year, the mature tree could remove 11,455 L (measured at room temperature and pressure) of carbon dioxide from the air, using the process in Q.1(d) to produce glucose. What mass of glucose would the poui tree have produced doing this?
The zinc inside the penny reacts with acetic acid (CH3COOH). The products are zinc acetate and hydrogen gas. Write out the balanced chemical reaction of zinc with acetic acid using states (i.e. s, g, l, and aq).
Hydrogen sulfide, H2S, is produced during decomposition of organic matter. When 0.4190 mol H2S burns to produce SO2 (9) and H20(g), -217.0 kJ of heat is released. What is this heat in kilocalories? Heat = kcal
Hh.81.
Combustion of hydrocarbons such as pentane (C5H₁2) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid pentane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.440 kg of pentane are burned in air at a pressure of exactly 1 atm and a temperature of 18.0 °C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits. ローロ X 00 0°
Combustion of hydrocarbons such as hexane (C6H₁4) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid hexane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.320 kg of hexane are burned in air at a pressure of exactly 1 atm and a temperature of 15.0 °C. Calculate the volume of carbon dioxide gas that is produced. Be sure your answer has the correct number of significant digits. OL X x10 Ś 18 Ar
A household water heater containing 50 gallons (227 L) of water is heated burning natural gas (methane, molar mass = 16.043 g mol-1) via the following reaction: CH4(g) + O2(g) CO2(g) + H20(O A,H = -891 kJ mol-1 What mass of methane, in units of g, is needed to heat the 227 L of water in the heater from 25.0°C to 44.0°C? Assume: • the heater is 100% efficient in its use of heat energy • no heat is lost to the surroundings specific heat of water is: 4.184 Jg-1 °C-1 density of water is: 0.9970 g mL¯1
4
There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(I) oxide and sulfur dioxide: →+2Cu2Ss 3O2g + 2Cu2Os 2SO2g In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: →+Cu2Os Cs + 2Cus COg Suppose the yield of the first step is 86.% and the yield of the second step is 64.% . Calculate the mass of copper(I) sulfide required to make 2.0kg of copper. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
Certain salts of benzoic acid have been used as food additives for decades. The potassium salt of benzoic acid, potassium benzoate, can be made by the action of potassium permanganate on toluene according to the following reaction (unbalanced): C7H8 + KMnO4 ® KC7H5O2 + MnO2 + KOH + H2O toluene potassium benzoate Balance the equation. What is the limiting reactant when 10.750 g of toluene react with 14.750 g of potassium permanganate? How much of the excess reactant remains after all of the limiting reactant is consumed? In an experiment using the masses of reactants listed above, 7.042 g of potassium benzoate was produced. What is the percent yield of that experiment? If the yield of potassium benzoate cannot realistically be expected to be more than 72.15%, what is the minimum number of grams of toluene needed to achieve this yield while producing 10.00 g of KC7H5O2?