Achemist has 2.0 mol of methanol (ch₃oh). the molar mass of methanol is 32.0 g/mol. what is the mass, in grams, of the sample?
16
30
32
64

64

Explanation:

Mole of a compound = mass of a compound / molar mass of a compound

Mass of a compound = mole of a compound x molar mass of a compound

Given,

Mole of methanol = 2 mol

Molar mass of methanol = 32 g/mol

Mass of methanol = Mole of methanol x Molar mass of methanol  

                               = 2 mol x 32 g/mol = 64 g

Therefore, the mass, in grams, of the sample = 64

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24