Octane reacts with oxygen in a combustion reaction described by the unbalanced equation C,H 18(e) + Pates + H2O). What is the mole ratio of octane and water vapour?

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.

contains 0.550 bar H2(g)0.550 bar H2(g) , 0.491 bar N2(g)0.491 bar N2(g) , and 0.121 bar Ar(g)0.121 bar Ar(g) . Calculate the mole fraction, ?χ , of each of these gases.

The internal pressure of a gas, π = au dv)T' is a measure of intermolecular forces, because it indicates a change in internal energy as the molecules get closer or further apart, without temperature changing. = a Calculate the change in internal 1 Vm T energy, AU, when 1.5 mols of acetone (a = 16 l² atm/mo1²), expands from 2 liters to 5 liters at a constant temperature. ii) Would this change in internal energy be greater or smaller for an ideal gas? Why? i) Using the van der Waals equation of state, T = au

using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔHsoln. Was the dissolution of this salt exothermic or endothermic?

Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance A B с D H :0: H | || | H с C -C-H 174 H H H chemical symbol, chemical formula or Lewis structure H H H | | C I 1 I H H H (II | Ag - Ar - :O: -O-H boiling point (Choose one) (Choose one) ✓ (Choose one) (Choose one) ✓

When air expands adiabatically (without gaining or losing heat), its pressure P and volume V are related by the equation PV14 = C where C is a constant. Suppose that at a certain instant the volume is 310 cubic centimeters and the pressure is 87 kPa and is decreasing at a rate of 8 kPa/minute. At what rate in cubic centimeters per minute is the volume increasing at this instant? cm3 min (Pa stands for Pascal it is equivalent to one Newton/(meter squared); kPa is a kiloPascal or 1000 Pascals.

Xenon and helium are both ideal, monatomic gases, but they have very different molar masses (Mxenon = 33*Mhelium). If you have 1 mole of each gas and the gases are at the same temperature, which one of the following statements is true?     They both have the same internal energy, but xenon has a lower root-mean-square speed than helium.    They both have the same internal energy and root-mean-square speed.    They both have the same root-mean-square speed, but xenon has a greater internal energy than helium.    They both have the same internal energy, but helium has a lower root-mean-square speed than xenon.    They both have the same root-mean-square speed, but helium has a greater internal energy than xenon.