Chem 110 Homework set 3-Cyanogen is a gas which contains 46.2% C and 53.8% N by mass.

Chem 110Homework set 3Name:…………………………………………………section:……………….Q1) Cyanogen is a gas which contains 46.2% C and 53.8% N by mass. At a temperature of 25°Cand a pressure of 750 mm Hg, 1.50 g of cyanogen occupies 0.714 L. What is the molecularformula of cyanogen?Q2) What is the density of fluorine gas at STP?Q3) Given three cylinders containing O2 gas at the same volume and pressure. Cylinder A is at 20°C, cylinder B is at -15°F, cylinder C is at 260 K. Which cylinder contains the largest mass ofoxygen?Q4) A lungful of air (500 mL) contains 4.1% CO2 by volume. How many grams of KO2(s) isneeded to remove the CO2 from a lungful of air at STP according to the following reaction?4 KO2(s) + 2 CO2(g) → 2 K2CO3(s) + 3 O2(g)Q5) An unknown gas contains 83% C and 17% H by mass. If effuses at 0.87 times the rate ofCO2 gas under the same conditions. What is the molecular formula of the unknown gas?Q6) An ideal gas expands into a vacuum (external pressure = 0) without gaining or losing heat.For this expansionA) ΔE increases.B) ΔE does not change.C) ΔE decreases.D) ΔE = TΔSQ7) Find ΔE° for the reaction below if the process is carried out at a constant pressure of 1.00atm and ΔV (the volume change) = -24.5 L. (1 L ∙ atm = 101 J)2 CO(g) + O2 (g) → 2 CO2(g) ΔH° = -566. kJQ8) At constant pressure, the combustion of 5.00 g of C2H6(g) releases 259 kJ of heat. What isΔH for the reaction given below?2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(l)Q9) When 0.455 g of anthracene, C14H10, is combusted in a bomb calorimeter that has a waterjacket containing 500. g of water, the temperature of the water increases by 8.63°C. Assumingthat the specific heat of water is 4.18 J/(g ∙ °C), and that the heat absorption by the calorimeter isnegligible, estimate the enthalpy of combustion per mole of anthracene.Q10) Coal gasification can be represented by the equation:2 C(s) + 2 H2O(g) → CH4(g) + CO2(g) ΔH = ?Use the following information to find ΔH for the reaction above.CO(g) + H2(g) → C(s) + H2O(g)ΔH = -131 kJCO(g) + H2O(g) → CO2(g) + H2(g)ΔH = -41 kJCO(g) + 3 H2(g) → CH4(g) + H2O(g) ΔH = -206 kJ