Metal compound a reacts with dilute hydrochloric acid to produce effervescence. the gas evolved extinguishes a burning candle. write a balanced chemical equation for the reaction if one of the compounds formed is calcium chloride.

When a mineral (A) is boiled with N a 2 ​ C O 3 ​ . A white precipitate (B) is formed. The precipitate is filtered and C O 2 ​ is passed through the filtrate, then a compound (C) sparingly soluble in cold water is formed. The compound (C) on strong heating gave two compounds D and E on heating with cobalt oxide produces blue coloured substance (F). Identify A to F and give balanced chemical reactions

Gujarat Board Gujarat Board Textbook Solutions Class 10 Science Chapter 2 Acids, Bases and Salts Gujarat Board Class 10 Science Acids, Bases and Salts InText Questions and Answers Question 1. You have been provided with three test tubes, one of them contains distilled water and the other two contain an acidic solution and a basic solution respectively. If you are given only red litmus paper, how will you identify the contents of each test tube? Answer: Add few drops of solution from all three test tubes on the red litmus paper separately. The solution which turns red litmus to blue contains basic solution. Use this blue litmus paper to test the solutions in other two test tubes. The solution from the test tube which turns blue litmus paper to red will be the acidic solution and solution of the test tube which do not change either red or blue litmus paper contains water. Question 2. Why should curd and sour substances not be kept in brass and copper vessels? Answer: Curd and sour substances contain acids which can react with copper vessels and brass to form toxic compounds. Question 3. Which gas is usually liberated when an acid reacts with a metal? Illustrate with an example. How will you test for the presence of this gas? Answer: When an acid react with a metal it liberates hydrogen gas. Example: Zn(s) + 2HCl(aq) → ZnCl 2(aq)+ H 2(g) To test the presence of H 2 gas, bring a burning match stick near the mouth of the test tube where H 2 gas is released, the match stick burn...

Reaction of zinc granules with dilute sulphuric acid and testing hydrogen. Take about 5 ml of dilute sulphuric acid in a test tube and add a few pieces of zinc granutes to it. Pass the gas being evolved through the soap solution. Bubbles are formed in the soap solution, because in soap solution there is hydrogen gas. H 2 ​ SO 4 ​ + Zn → ZnSO 4 ​ + H 2 ​ ↑ If we take a burning candle near a gas filled bubble, it burns with a pop sound. Views: 5,535 (a) What is the common name of the compound CaOCl 2? (b) Name the raw material used for the preparation of plaster of Paris. (c) Which property of plaster of Paris is utilised in making casts for broken limbs in hospitals? (d) Explain why chlorine is used for sterilising drinking water supply. Metal compound A reacts with dilute hydrochloric acid produce effervescence. The gas evolved extinguishes a burning candle. Write a balanced chemical equation for the reaction If one of the compounds formed is calcium chloride. Updated On May 10, 2023 Topic Acid,Bases and Salts Subject Science Class Class 10 Answer Type Text solution:1 Video solution: 11 Upvotes 1271 Avg. Video Duration 4 min

The gas the extinguishes a burning candle is carbon dioxide. It is formed by the action of dilute hydrochloric acid on metal carbonate or metal hydrogencarbonate and produces effervescence . Since one of the compounds formed is calcium chloride, this shows that the metal compound is calcium carbonate. It cannotbe calcium hydrogencarbonate because calcium hydrogencarbonate is found in solution . Thus , the metal compound A is calcium carbonate ( C a C O 3 ) . Calcium carbonate reacts with dilute hydrochloric acid to form calcium chloride. carbon dioxide and water . C a C O 3 ( s ) + 2 H C l ( a q ) → C a C l 2 ( a q ) + C O 2 ( g ) + H 2 O ( l )

Metal compound A reacts with dilute hydrochloric acid to produce effervescence. The gas evolved to extinguish a burning candle. Write a balanced chemical equation for the reaction if one of the compounds formed is calcium chloride. a) \\[CaC\\] Metal compound A reacts with dilute hydrochloric acid to produce effervescence. The gas evolved to extinguish a burning candle. Write a balanced chemical equation for the reaction if one of the compounds formed is calcium chloride. a) \[CaC\] Hint: According to the question, the gas produced as a result of this reaction produces effervescence. There is one particular gas which has this property. The same gas also turns limewater milky. Complete step by step answer: Let us try and solve this question by going through the options and eliminating the wrong ones. According to the question, the gas produced by reaction of metal with dilute hydrochloric acid produces effervescence. The same gas also extinguishes a burning candle. Carbon dioxide is a gas which has this property. From this, we can say that the product side must contain carbon dioxide. We can, therefore, eliminate the options which do not have carbon dioxide in its products, i.e., option (b) and (d). Now, the options left with us are option (a) and option (c). As the base equation is the same in both the options, we can check the equations for its stoichiometric coefficients. Look at the equation in option (c), we can see that Hydrogen is not balanced on both sides. On the r...

The explanation for the answer: • As the gas formed is an effervescent carbon dioxide gas, it happens when Calcium Carbonate ( CaCO 3 ) . reacts with hydrochloric acid (HCl). • The carbon dioxide gas also acts as an extinguisher for fires. • So, the burning candle is extinguished. • The metal compound A, therefore, constitutes calcium carbonate. • Thus metal compound A is CaCO 3 • The Gas B evolved is CO 2 • The balanced equation of the reaction is: CaCO 3 ( s ) Calcium Carbonate + 2 HCl ( aq ) Hydrochloric acid → CaCl 2 ( s ) Calcium chloride + CO 2 ( g ) Carbon dioxide + H 2 O ( l ) water or Oxygen hydride . Final Answer: • Metal compound A is Calcium Carbonate ( CaCO 3 ) . • The Gas B evolved is Carbon dioxide ( CO 2 )

(a) Brisk effervescence with an acid is produced due to the evolution of Carbon dioxide ( CO 2 ) gas which is colourless and odourless gas on reaction of an acid with carbonate ore. Example: • ZnCO 3 ( s ) ( Zinc carbonate ) + HCl ( aq ) ( Dil . Hydrochloric acid ) → ZnCl 2 ( s ) ( Zinc chloride ) + CO 2 ( g ) ( Carbon dioxide ) • So the ore is a carbonate ore. (b) The process of calcination followed by reduction is required to obtain a metal from its carbonate ore. Step-1: Calcination When a carbonate ore is heated in the limited supply or absence of air, the carbonate ore gets converted into its oxide ore after releasing carbon dioxide. • Hence, by the calcination process the metal carbonate ore are converted to their metal oxides a shown below. • ZnCO 3 ( Zinc carbonate ) → ∆ ZnO ( s ) ( Zinc oxide ) + CO 2 ( g ) ( Carbon dioxide ) Step-2: Reduction with carbon Oxide ore is heated with carbon which acts as a reducing agent and helps to extract the metal i.e.; Zinc. • ZnO ( s ) ( Zinc ) + C ( s ) ( Carbon ) → Zn ( s ) ( Zinc ) + CO ( g ) ( Carbon moonoxide ) Q. One of the forms of a naturally occurring solid compound P is usually used for making the floors of houses. On adding a few drops of dilute hydrochloric acid to P, brisk effervescence are produced. When 50 g of reactant P was heated strongly, than 22 g of a gas Q and 28 g of a solid R were produced as products. Gas Q is the same which produced brisk effervescence on adding dilute HCl to P. Gas Q is said to...