Camels store a fat called tristearin (C7H1006) in their humps. The breakdown of tristearin provides both energy and water. The reaction is shown below: 2 _C57H1006(S) + 163_0₂(g) → 114 CO₂(g) + 110 H₂O(l) How many moles of 0₂ gas would be required to react with 17.00 moles tristearin?

peact Baking soda is often included in recipes to make food rise. When heated, it will produce sodium carbonate, water vapor, and carbon dioxide. Which of the five types of chemical reactions does the equation represent? Provide evidence and reasoning

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

A sample of 49.0 g of tetraphosphorous decoxide (P,O10) reacts with 49.0 g of water to produce phosphoric acid (H, PO,) according to the following balanced equation. P,010 + 6 H,O → 4H,PO, Determine the limiting reactant for the reaction. H,PO, O H,0 O P,O10 Calculate the mass of H, PO, produced in the reaction. mass of H, PO4: Calculate the percent yield of H, PO, if 37.5 g of H, PO, is isolated after carrying out the reaction. percent yield:

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.

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?

For the following reaction, 5.82 grams of water are mixed with excess chlorine gas. The reaction yields 14.0 grams of hydrochloric acid. chlorine (g) + water (1) →→→hydrochloric acid (aq) + chloric acid (HCIO3) (aq) What is the theoretical yield of hydrochloric acid ? What is the percent yield of hydrochloric acid ? grams %

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 5.4 kgkg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)

Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P,(s) + 50,(g) 2 P,0; (g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid (H,PO,): P,0;(g) + 3H,0(1) 2 H;PO, (1) Suppose the yield of the first step is 77.% and the yield of the second step is 67.%. Calculate the mass of phosphorus required to make 6.0 kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

When exposed to air, aluminum metal, AlAl, reacts with oxygen, O2O2, to produce a protective coating of aluminum oxide, Al2O3Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here: 4Al+3O2→2Al2O3 a) What is the theoretical yield of aluminum oxide if 3.00 molmol of aluminum metal is exposed to 2.55 molmol of oxygen? Express your answer with the appropriate units.