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Li and Raj are playing football. They take turns trying to run past each other with the football. Li weighs 125 pound and Raj weighs 175 pounds. Li discovers that if he changes direction quickly when running, he can always dodge out of the way before Raj can tackle him.
Why is Li able to avoid Raj’s tackle? Choose the best description.
Raj has more mass and therefore more inertia, so he can change his motion more easily than Li.
Raj has more mass and therefore less inertia, so he can change his motion more easily than Li.
Li has less mass and therefore more inertia, so he can change his motion more easily than Raj.
Li has less mass and therefore less inertia, so he can change his motion more easily than Raj.
Calculate the lattice energy of rubidium flouride from the following data:
Heat of sublimation=+86kjmol
Standard heat of formation of RbF =-548kjmol
Dissociation energy of F²(g)=+155kjmol
Ionization energy of Rb(g)=+402kjmol
Electron affinity of F(g)= -346kjmol
2. Calculate the lattice energy of calcium chloride from the following data:
Heat of sublimation Ca(g)=+193kjmol
Standard heat of formation of CaCl2(g) =-794kjmol
Dissociation energy of Cl2(g)=+242kjmol
Ionization energy of Ca(g) to Ca²+(g)=+1725kjmol
Electron affinity of Cl(g)= -364kjmol
A system containing 5 moles of an ideal monotomic gas was heated from temperature T1 = 210 K to temperature T2 = 410 K. The internal energy of the gas increased by ∆E = 5000 J. Calculate the change in enthalpy,▲H.
The heat of combustion of benzene is -3268jmol and cyclohexane is -3920kjmol.
Calculate:
(a) The heat of hydrogenation of benzene to cyclohexane
(b)The heat required to hydrogenate a double bond of benzene
Use the thermal power table to calculate the mass of water that can be brought from 20 ° C to 100 ° C by burning 1 kg of butane.
on the combustion of alkanes: To increase the temperature of 1 kg of water from 20 ° C to 100 ° C, an energy of 330 kJ is required.
Predict the structure from following Spectroscopy data: Vapor Density: 54 IR: 3420, 3250, 850 cm-1
Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2 (g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.920 mol N2 and 0.700 mol O2 are mixed in a 3.00-L reaction vessel. What will be the concentrations of N2, O2, and NO when equilibrium is established? (Hint: assume that the amounts of N2 and O2 that react are small—less than 10% of the starting amounts—and check your assumption when you have solved the equation.)
Consider the following reaction: N2O4 (g) → 2 NO2 (g) Assume that an experiment is carried out in which the starting concentration of N2O4 (g) is 0.100 mol/L. No products are present at the beginning of the reaction. When equilibrium is established, the concentration of NO2 (g) is 2.43 x 10-2 mol/L. Calculate the equilibrium constant for the above reaction.
I-Butanol and chlorobenzene form a minimum-boiling azeotropic system. The mole fraction of I-butanol in the liquid (x) and vapour (y) phases at 1.000 atm is given below for a variety of boiling temperatures (H. Artigas, C.
Lafuente, P. Cea, F.M. Royo, and J.S. Urieta,J. Chem. Eng. Data 42,132 (1997))
T/K 396.57 393.94 391.60 390.15 389.03 388.66 388.57
X 0.1065 0.1700 0.2646 0.3687 0.5017 0.6091 0.7171
Y 0.2859 0.3691 0.4505 0.5138 0.5840 0.6409 0.7070
Pure chlorobenzene boils at 404.86 K.
(a) Construct the chlorobenzene-rich portion of the phase diagram from the data.
(b) Estimate the temperature at which a solution whose mole fraction of I-butanol is 0.300 begins to boil.
(c) State the compositions and relative proportions of the two phases present after a solution initially 0.300 l-butanol is heated to 393.94 K
