Name: Date: Period: Course: CHEM 510 Ideal Law Practice Set 2.0 Directions: Solve the following problems on a separate sheet of paper using the 5-step method to show your work. All answers must be in proper SIG FIGs. Use the Ideal Gas Law (PV=nRT) to solve each of the following. R = 8.31 (L•kPa)/(K•mol) or 0.082 (L•atm)/(K•mol) 1. Calculate the volume 3.00 moles of a gas will occupy at 24.0 °C and 101.3 kPa.
a) Write the equation for the reaction. b) Calculate the number of moles of Fe2+ present in 1.0 dm3 of the solution. c) Calculate the molar mass of hydrate iron(II) sulphate. Hence calculate the value of x. 4.
IB HL Chemistry Energetics - End of Topic Test 35 min 37 marks Answer all the questions in the spaces provided 1. What energy changes occur when chemical bonds are formed and broken? A. Energy is absorbed when bonds are formed and when they are broken. B.
Repeat the titration until there are two titres within 0.1cm3 of each other. Record results in a suitable table. Results: Rough Titre: 7.653 First Run: 6.553 Second Run: 6.453 Third Run: 6.553 Calculations: During the titration, iron(II) ions are oxidised to iron(III) ions and manganate(VII) ions are reduced to manganese(II) ions. The equation is as follows: 5Fe2+(aq) + MnO4-(aq) + 8H+(aq) ? 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) The above equation shows that one mole of manganate(VII) ions reacts with 5 moles of iron(II) ions in acid solution.
Read each question carefully The Final is 2 and 1/2 hours long or 150 minutes Homework and Quizzes: 150 pts Midterms: 550 pts Final Exam : 300 pts Final Grade over 1000 Letter Grade Note that you need at least 600/1000 to make a grade of C − . 1 Exercise 1. (30 points) If u = i − j + k and v = i + j + k • Find the cosine of the angle between the vectors u and v • For what values of the constant b are the vectors v orthogonal? and w = i + b j • Find the area of the parallelepiped spanned by the vectors u and v 2 Exercise 2. (30 points) • Find the vector equation of the line through P (2, 1, 3) perpendicular to the plane 3x − 4y + z − 5 = 0 • Two particles P1 and P2 have position vector r1 (t) =< 1, t + 3, −t > and r2 (t) =< 2t − 1, 1 + 3t2 , t3 − 2 > respectively at time t. Do the particles collide?
When the temperature falls below temperature of 980K, the structure is trigonal and posses the lattice boundaries a=b=c, α= β= γ ≠ 90°. The structure will transform from a α-model to the β-model and become a hexagonal unit cell. This then portrays the difference between the symmetries of the two different structures. According to Table 2, it shows the changes in cell parameters as well as volume in relation to the temperature of the metal. It therefore shows us that when temperature rises, the crystal forms will change as they are affected by changes in temperature.
4. Results and Discussion Specific heat capacity refers to the amount of heat needed to raise or lower the temperature of a substance. This amount of heat is directly proportional to the mass of the material. In the first activity, the specific heat of a metal, in our case aluminum, was calculated (Table 1). The following formula was used: cm=mwcwT3-T1+mcccT3-T1 mmT2-T3 Where cw is the specific heat capacity of water and cc is the specific heat capacity of calorimeter.
Which way will the following equilibrium shift if the total pressure on the system is decreased? 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g) Answer________________ 4. Hydrogen peroxide is decomposed as follows: H2O2(l) → H2(g) + O2(g) H = +187 kJ Predict the direction of equilibrium shift by each of the following imposed changes: a) Increase the [H2] ........................................Answer ______________________ b) Decrease the [O2] .......................................Answer ______________________ c) Decrease the total pressure ........................Answer ______________________ d) Increase the temperature............................Answer ______________________ e) Add MnO2 as a catalyst.............................. Answer ______________________ 5. Consider the following reaction at equilibrium: H2(g) + I2(g) → 2HI(g) a) Addition of more H2 gas to the container will do what to the rate of the forward reaction? Answer ________________________ b) If, for a while, the rate of the forward reaction is greater than the rate of the reverse
First, when determining the mass of 100 mL solution, it is necessary to assume that the density of all the solutions is 1.00 g/mL. Secondly, to calculate the heat released by each reaction the following equation will be used: · Q = Cp * m * ∆t (Cp = 4.18 J/goC). Finally, it is necessary to know how to find ∆H. This can be found with the following formula: · ∆H = -q. Additivity of Heats of Reaction: Hess’s Law relates to the concepts being studied in several ways. This experiment mainly relates to
Record the volume of gas in burette in every 30 seconds for 5 minutes. 8. Tabulate the reading obtained from the reaction. 9. Repeat the experiment by using 0.2 g magnesium powder.