Heptane (C7H16) gas reacts with oxygen gas to give carbon dioxide gas and water vapor.  If you mix heptane and oxygen in the correct stoichiometric ratio to make the reaction go to completion without any excess reagent, and if the total pressure of the mixture is 705 mmHg, what is the partial pressure of heptane? Enter your answer in units of mmHg.

How many moles of oxygen are consumed in burning 1.6 moles of Benzene, C6H6?

(Record your answer with rounded answer to proper significant digits and the proper units.) 1.How many moles of butane (C4H10(g)) were combusted in the presence of excess oxygen gas if 55.8 L of water vapour at STP is collected?Hint: Write a balanced chemical reaction equation first. 2.One of the steps to sweeten sour gas using the Claus process is reacting hydrogen sulfide gas with sulfur dioxide gas to produce water vapour and sulfur. 16H2S(g)+8SO2(g)----->16H2O(g)+3S8(s)  8.75 kL of hydrogen sulfide at 175 kPa and 250 °C reacts with excess sulfur dioxide. Calculate the mass, in kg, of sulfur produced.

Solid potassium chlorate, KCIO3, decomposes upon heating to form potassium chloride and oxygen gas. Write a balanced chemical equation for the reaction. The volume of oxygen that would form at standard temperature and pressure if 0.456 g KCIO3 decomposes is mL. Answer must be verified.

Given the following balanced equation, what volume of hydrogen gas (in liters) would be produced under conditions of STP from the reaction of 0.082 grams of magnesium solid reacting with excess hydrochloric acid solution?  Please report your answer WITH the correct number of significant figures, and WITHOUT units. Mg  +  2 HCl  →  MgCl2  +  H2

What is the volume @ STP of 3.29x10^25 molecules of CO2? Round to 2 decimal places.

The human body burns glucose (C6H12O6) for energy according to this chemical reaction: C6H12O6+6O2→ 6CO2+6H2O The products of the reaction are carbon dioxide CO2 and water H2O Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500.mL of air, which is typically enriched to 4% CO2 and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 0.50kg  of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO2 is 2.0 kg/m^3 .

Three bulbs are connected by tubing, and the tubing is evacuated. The volume of the tubing is 49.0 mL The first bulb has a volume of 58.0 ml and contains 6.07 atm of argon, the second bulb has a volume of 250 ml. and contains 1.62 atm of neon, and the third bulb has a volume of 27.0 ml. and contains 7.72 atm of hydrogen. If the stopcocks (valves) that isolate all three bulbs are opened, what is the final pressure of the whole system in atm? Answer:

The U.S. proven natural gas reserves in 2013 were 323 trillion  ft3 . How long will these reserves last if there are no imports or exports and if the U.S. annual rate of use of 24.5 trillion  ft3  continues?

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.