A reaction produced 37.5 L of oxygen gas at 307 K and 1.25 atm. How many moles of oxygen were produced?

Chemistry

1 answer:

MariettaO [177]3 years ago

3 0

On the basis of the given data:

Volume (V) is 37.5 L

Temperature (T) is 307 K

Pressure (P) is 1.25 atm

In order to calculate the number of moles, the formula to be used is PV = nRT, Here R is 0.0821 Latm/mol/K

n = PV / RT

n = 1.25 atm × 37.5 L / 0.0821 Latm/mol/K × 307 K

n = 1.85 mol

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Compound a reacts with one equivalent of h2 in the presence of a catalyst to give methylcyclohexane. Compound a can be formed up

V125BC [204]

Answer:

The compound a is 1-methyl cyclohexene (see attachment for structure).

Explanation:

The reaction of 1-Bromo-1-methylcyclohexane with sodium methoxide is a second-order reaction since the methoxide ion is a strong base and also a strong nucleophile. This ion attacks the alkyl halide faster than the alkyl halide can ionize to produce a first-order reaction. However, we can not see the product of nucleophilic substitution. The SN₂ mechanism is blocked due to the impediment of the 1-Bromo-1-methylcyclohexane. The main product, according to the Zaitsev rule, is the 1-methyl cyclohexene, thus forming a double bond.

Then, this cyclohexene is hydrogenated to form the cyclohexane.