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13C decays with a rate constant of 2.31 x 10-10/min. What is the activity of a 5.21 g sample in curies.
Draw the structure of the tripeptide, which is composed of Phe+Lys+Cys and answer additional questions .
1.1. specify the value of the isoelectric point
1.2 select the indicator and determine the pH of the aqueous solution by indicator's color 1.3 specify the hydrophilic-hydrophobic balance
1.4 draw the structures of the tripeptide that correspond to the pH values 0, pl, 7, 14. Specify the charge of the tripeptide in each pH
2. Construct the Fişcher's formula for the D-mannose [2(L),3(L),4(D),5(D),6- pentahydroxyhexan-1-al] and draw all the tautomers: oxo, and pyranoses, furanoses. 3.Give the formula of the nucleic base cytosine, nucleoside cytidine, nucleotide cytidine-3-phosphate
A sample of carbon dioxide occupies a volume of 3.50 Liters at 125 kPa pressure. What pressure would the gas exert if the volume was decreased to 2.00 liters?
1.If heat is observed as products were formed means that the reaction is ___.
a.endothermic
b. endergonic
c. exothermic
d. both b and c are correct
2.If a substance that would increase the reaction’s rate would have been added instead, what will happen to the equilibrium?
a.shift to the left
b. shift to the right
c. none of the given options
d. no shift
3.Will the equilibrium re-established after one of your groupmates added an increment in the temperature?
a. yes
b. no
c. more information required
d. none of the given options
4.What equation relates the expression of the equilibrium constant in terms of pressure and concentration?
a.ideal gas equation
b. van’t Hoff equation
c. Arrhenius equation
d. Molarity
5.If the coefficients for a reaction are all multiplied by 2, the equilibrium constant will be
a.equal to Kc x 2
b. equal to Kc over 2
c. unchanged
d. equal to Kc2
4.A reaction that is spontaneous as written __________.
a.is very rapid
b.will proceed without outside intervention
c.is also spontaneous in the reverse direction
d.has an equilibrium position that lies far to the left
e.is very slow
5.For an isothermal process, ΔS = __________.
a.q
b.qrev/T
c.qrev
d.Tqrev
e.q + w
1.The entropy will usually increase when;
I.a molecule is broken into two or more smaller molecules.
II.a reaction occurs that results in an increase in the number of moles of gas.
III.a solid changes to a liquid.
IV.a liquid changes to a gas.
a. I only
b.II only
c.III only
d.IV only
e.I, II, III, and IV
2.For the reaction, A + B → C, ΔHo = +30 kJ; ΔSo = +50 J/K. Therefore the reaction is:
a.spontaneous at all temperatures.
b.nonspontaneous at all temperatures.
c.spontaneous at temperatures less than 600 K.
d.spontaneous at temperatures greater than 600 K.
e.spontaneous only at 25oC.
3.The thermodynamic quantity that expresses the degree of disorder in a system is __________.
a.enthalpy
b.internal energy
c.bond energy
d.entropy
e.heat flow
Silver metal reacts with sulfur to form silver sulfide according to the following balanced equation: (5 points)2Ag(𝑠) + S(𝑠) → 𝐴𝑔2S(𝑠)What is the limiting reactant when 50.0 g Ag is reacted with 10.0 g S?
The titration of a 10.0ml sample of vinegar requires 30.0ml of 0.20 M NaOH solution. Calculate
i. The molarity
ii. The mass /mass percent concentration of acetic acid.
Given that the density of acetic acid is 1.01g/cm3
Find the formal charge of each atom in the given compounds/polyatomic ion.
a. HBr
b. N₂0
c. SO₄²⁻
A sample of carbon dioxide gas, CO2, occupies a volume of 5.0L at STP. What is the volume of carbon dioxide at 780 torrs and 25 degrees celsius?
