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The vapor pressure of substance X is higher than that of substance Y at 298 K.  This observation means that A. X has stronger intermolecular forces than Y. B. Y has stronger intermolecular forces than X. C. X and Y have intermolecular forces of the same strength. D. The relative strength of the intermolecular forces cannot be determined.

How many moles of Carbon atoms are present in 2.50 g of Glucose (C6H12O6). MW C6H12O6 = 180.18 g/mol A. 0.0138 mol C B. 0.0416 mol C C. 0.0833 mol C D. 12.0 mol C

An equilibrium mixture contains 0.200 moles CH3OH, 0.400 moles CO and 0.500 moles H2 in a 2.0 L container.  What is the equilibrium constant (Kc) for the reaction?   A. 2.00 B. 0.500 C. 1.00 D. 0.125

Element X reacts with Sodium to form the ionic compound Na2X.  What is element X if its anion has 18 electrons? A. S B. Ar C. Se D. Br    

A photon of infrared light has a ____________________________ wavelength and ______________________ energy than a photon of ultraviolet radiation.   A. Shorter, lower B. Longer, lower C. Shorter, higher D. Longer, higher

What is the oxidation state of manganese in MnO4-? A.  +1 B.  +3 C.  +5 D.  +7

What is the hydroxide ion concentration, [OH-], in a solution with a pH of 8.472 at 25

What is the mass of 0.1000 mole of AlCl3

The pH of a 0.25 M aqueous solution of acetic acid, CH3CO2H, is 2.67 at 25

The equilibrium constant, K, is 2.4 x 103 at a certain temperature for the reaction: 2NO(g) ⇌ N2(g) + O2(g) For which of the following sets of conditions is the system at equilibrium? A.  1.0-L flask contains 0.024 mol NO, 2.0 mol N2, and 2.6 mol O2. B.  2.0-L flask contains 0.032 mol NO, 0.62 mol N2, and 4.0 mol O2. C.  3.0-L flask contains 0.060 mol NO, 2.4 mol N2, and 1.7 mol O2. D. None of these conditions are at equilibrium