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.

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

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?

What is the easiest process to get to the result?

Commercial drain cleaners contain sodium hydroxide and aluminum. When water is added to this mixture, the heat that is generated will melt grease and the gas that is created will stir up the particles that are clogging the drain. If the process proceeds according to the following reaction: 2 Al (s) + 2 NaOH (aq) + 6 H2O (l) → 2 NaAl(OH)­4 (aq) + 3 H2 (g)   If you use 5.6 g of Al (s) and excess sodium hydroxide, how many liters of H2 (g) at 742 mm Hg and 22.0 ˚C are produced?

Soda ash (sodium carbonate) is widely used in the manufacture of glass.  Prior to the environmental movement much of it was produced by the following reaction.   CaCO3 + 2 NaCl → Na2CO3 + CaCl2   Unfortunately, the byproduct calcium chloride is of little use and was dumped into rivers, creating a pollution problem.  As a result of the environmental movement, all of these plants closed.  Assume that 125g of calcium carbonate (100.09 g/mol) and 125 g of sodium chloride (58.44 g/mol) are allowed to react.   Determine how many grams of useful sodium carbonate (105.99 g/mol) will be produced.  How many grams of useless calcium chloride (110.98 g/mol) will be produced?  You should also determine how many grams of excess reactants are left (indicate which one is the limiting reactant)