All categories

2 years ago

What is the general formula for cycloalkenes.

Chemistry

2 answers:

maria [59]2 years ago

3 0

C( n)H(2n) is the general formula, eg: Cyclohexane is C6H12

dexar [7]2 years ago

3 0

$\tt \huge { \red{\colorbox{lime}{Answer}}}$

$\tt \bf \: \implies C_{n}H_{2}n$

Cycloalkenes have the general formula

$\\ \tt \: \: \: C_{n} H_{2} \: _{n - m}$

The letter m represents the number of double bonds. Thus, cyclopropene has the formula C3H4 while that of cyclobutene is C4H6. The properties of alkanes and alkenes are very similiar.

You might be interested in

In the following reaction, how many grams of oxygen will react with 10.47 grams of benzene (C6H6)? 2C6H6 + 1502 12CO2 + 6H2O The

goldfiish [28.3K]

Can you follow me and like me please?

8 0

3 years ago

How many electrons can be held in sub level I=3?

Zinaida [17]

2 is your answer hope you get it right

6 0

3 years ago

How many significant figures are there in this expression 0.001050

WITCHER [35]

4 sig fig in that expression

4 0

3 years ago

Read 2 more answers

You have 50 ml of a complex mixture of weak acids that contains some HF (pKa = 3.18) and some HCN (pKa = 9.21). Which is larger,

bonufazy [111]

Answer:

$\frac{[F^{-}]}{[HF]}$ is larger

Explanation:

$pK_{a}=-logK_{a}$ , where $K_{a}$ is the acid dissociation constant.

For a monoprotic acid e.g. HA, $K_{a}=\frac{[H^{+}][A^{-}]}{[HA]}$ and $\frac{[A^{-}]}{[HA]}=\frac{K_{a}}{[H^{+}]}$

So, clearly, higher the $K_{a}$ value , lower will the the $pK_{a}$

In this mixture, at equilibrium, $[H^{+}]$ will be constant.

$K_{a}$ of HF is grater than $K_{a}$ of HCN

Hence, $(\frac{F^{-}}{[HF]}=\frac{K_{a}(HF)}{[H^{+}]})>(\frac{CN^{-}}{[HCN]}=\frac{K_{a}(HCN)}{[H^{+}]})$

So, $\frac{[F^{-}]}{[HF]}$ is larger

5 0

3 years ago

Consider the reaction 2NO(g) 1 O2(g) ¡ 2NO2(g) Suppose that at a particular moment during the reaction nitric oxide (NO) is reac

GalinKa [24]

<h2>a) The rate at which $NO_2$ is formed is 0.066 M/s</h2><h2>b) The rate at which molecular oxygen $O_2$ is reacting is 0.033 M/s</h2>

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$2NO(g)+O_2(g)\rightarrow 2NO_2(g)$

The rate in terms of reactants is given as negative as the concentration of reactants is decreasing with time whereas the rate in terms of products is given as positive as the concentration of products is increasing with time.

Rate in terms of disappearance of $NO$ = $-\frac{1d[NO]}{2dt}$ = 0.066 M/s