Question
Complete the following reactions:
  1. $NH_3+ 3Cl_2($excess$) →$
  2. $XeF_6 + 2H_2O →$

Answer

  1. $NH_3 + 3Cl_2 ($excess$) → NCl_3 + 3HCl$
  2. $XeF_6 + 2H_2O → XeO_2F_2 + 4HF$

Need a full question paper?

Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.

Start Generating Free

Similar questions

What is the repeating unit in the condensation polymer obtained by combining $HO_2CCH_2CH_2CO_2H$ (succinic acid) and $H_2NCH_2CH_2NH_2$ (ethylene diamine).
Consider the decomposition of hydrogen peroxide in alkaline medium which is catalysed by iodide ions.
$\text{2H}_2\text{O}_2\xrightarrow{\text{OH}^-}2\text{H}_2\text{O}+\text{O}_2$
This reaction takes place in two step as given below:
Step-I $\text{H}_2\text{O}_2+\text{I}^-\rightarrow\text{H}_2\text{O}_2+\text{IO}^-\text{ (slow)}$
Step-II $\text{H}_2\text{O}_2+\text{IO}^-\rightarrow\text{H}_2\text{O}_2+\text{I}+\text{O}_2\text{ (fast})$
  1. Write the rate law expression and determine the order of reaction w.r.t. $H_2O_2.$
  2. What is the molecularity of each individual step?
Why the boiling points of aldehydes and ketones are higher than the hydrocarbons and ethers of comparable molecular masses but lower than alcohols?
Explain the following term with suitable examples:
Interstitials.
Explain reaction of carboxylic acids with metals and alkalies. ### Write the equations for the reactions showing that carboxylic acids are acidic in nature and state theusefulness of this reactions.
Give the examples of chain and position isomerism in carboxylic acids.
In a reaction between $A$ and $B$, the initial rate of reaction $(r_0)$ was measured for different initial concentrations of $A$ and $B$ as given below:
$A/mol\ L^{-1}$ $0.20$ $0.20$ $0.40$
$B/mol\ L^{-1}$ $0.30$ $0.10$ $0.05$
$r_0/mol\ L^{-1}\ s^{-1}$ $5.07 \times 10^{-5}$ $5.07 \times 10^{-5}​$​​​​​​ $1.43 \times 10^{-4}$
What is the order of the reaction with respect to $A$ and $B?$
Phenols do not undergo substitution of the -OH group like alcohols.
Nitric oxide, $NO$, reacts with oxygen to produce nitrogen dioxide.
$\text{2NO(g)+O}_2(\text{g)}\rightarrow\text{2NO}_2\text{(g)}$
The rate law for this reaction is:
$\text{Rate = k}[\text{NO]}^2[\text{O]}_2$
Propose a machanism for the reaction.
The rate constant for the first order decomposition of $H_2O_2$ is given by the following equation:$\log{k}=14.2-\frac{\text{1.0}\times\text{10}^{4}}{\text{T}}K$
Calculate $E_a$ for this reaction and rate constant k if its half-life period be $200$ minutes.
$($Given: $R = 8.314\ J\ K^{–1}\ mol^{–1})$