Complete the equation by inserting the state symbols for the products. $\text{CuCO}_3(s) + 2\text{HCl}(aq) \rightarrow \text{CuCl}_2(\ldots) + \text{H}_2\text{O}(\ldots) + \text{CO}_2(\ldots)$
In a different experiment, powdered copper(II) carbonate is used rather than large pieces of copper(II) carbonate. Every other condition and the mass of copper(II) carbonate remain unchanged. Draw a line on the grid in Fig. 5.1 to show how the mass of the reaction mixture changes with time.
The initial experiment is carried out again using large pieces of copper(II) carbonate and hydrochloric acid at a higher concentration. All other conditions stay the same. Describe and explain the change in rate of reaction when hydrochloric acid of a higher concentration is used.
Excess copper(II) carbonate is mixed with $22.0\,\text{cm}^3$ of $0.500\,\text{mol dm}^{-3}$ hydrochloric acid. Calculate the volume of carbon dioxide produced at room temperature and pressure. Give your answer to two significant figures.
Describe the observations seen when: • a few drops of aqueous ammonia are added to an aqueous solution containing copper(II) ions • excess aqueous ammonia is added to an aqueous solution containing copper(II) ions.
A copper ionic compound has the formula $\text{Cu}_2\text{O}$. Deduce the oxidation number of copper in $\text{Cu}_2\text{O}$.
Describe the method for preparing crystals of ammonium chloride from aqueous ammonia and dilute hydrochloric acid.