{"id":13153,"date":"2020-11-30T06:19:11","date_gmt":"2020-11-30T00:49:11","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=13153"},"modified":"2020-11-30T17:16:45","modified_gmt":"2020-11-30T11:46:45","slug":"stoichiometry-used-chemistry","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/stoichiometry-used-chemistry\/","title":{"rendered":"What is stoichiometry and why is it used in chemistry?"},"content":{"rendered":"
People also ask<\/strong><\/p>\n 1.<\/strong>\u00a0How many moles of potassium are needed to react with 0.5 mole of bromine gas? 2. <\/strong>Ethene gas burns in excessive oxygen according to the following equation. 3. <\/strong>What is the mass of zinc needed to produce 2.4 dm3\u00a0<\/sup>of hydrogen gas at room conditions? 4. <\/strong>Aluminium reacts with copper(II) oxide to produce aluminium oxide and copper. If 2.0 g of excess aluminium is reacted with 0.06 mole of copper(II) oxide, find the mass of aluminium left after the reaction. 5.<\/strong> Excess sodium chloride is added to 50.0 cm3<\/sup> of silver nitrate solution. 2.87 g of silver chloride is precipitated. Calculate the concentration of the silver nitrate solution in mol dm-3<\/sup>. 6.<\/strong> In the preparation of copper(II) sulphate, a student added 4.0 g of copper(II) oxide to 1.25 mol dm-3<\/sup> sulphuric acid. Calculate the volume of the acid needed to react completely with the copper(II) oxide. [Relative atomic mass: O, 16; Cu, 64] 7.<\/strong> Excess aluminium powder is added to 300 cm3<\/sup> of 2.0 mol dm-3<\/sup> hydrochloric acid. The mixture is then warmed to speed up the reaction. Calculate the mass of the salt formed. [Relative atomic mass: Al, 27; Cl, 35.5] 8.<\/strong> 150 cm3<\/sup> of 1.0 mol dm-3<\/sup> ammonia solution is completely neutralised with phosphoric acid using a titration method. Calculate the mass of ammonium phosphate formed. [Relative atomic mass: H, 1; N, 14; O, 16; P, 31] 9.<\/strong> 6.20 g of copper(II) carbonate is added to 100 cm3<\/sup> of 14.6 g dm-3<\/sup> hydrochloric acid. Calculate the mass of copper(II) chloride produced. [Relative atomic mass: H, 1; C, 12; O, 16; Cl, 35.5; Cu, 64] What is stoichiometry and why is it used in chemistry? Stoichiometry is a study of quantitative composition of substances involved in the chemical reactions. A balanced chemical equation can be used to calculate number of moles, number of particles and mass or volume of a reactant or product. By using the information obtained from a […]<\/p>\n","protected":false},"author":3,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_genesis_hide_title":false,"_genesis_hide_breadcrumbs":false,"_genesis_hide_singular_image":false,"_genesis_hide_footer_widgets":false,"_genesis_custom_body_class":"","_genesis_custom_post_class":"","_genesis_layout":"","footnotes":""},"categories":[84],"tags":[4734,4732,4737,4382,4381,4735,4736,4731,4730,4733],"yoast_head":"\n\n
Stoichiometry Problems with Answers<\/h2>\n
\n2K(s) + Br2<\/sub>(g) \u27f6\u00a02KBr(s)
\nSolution:<\/strong>
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\nC2<\/sub>H4<\/sub>(g) + 3O2<\/sub>(g)\u00a0\u00a0\u27f6\u00a0 2CO2<\/sub>(g) + 2H2<\/sub>O(l)
\nFind the volume of carbon dioxide released at STP if 42 g of ethene is burnt completely. [Relative atomic mass: H, 1; C, 12. Molar volume: 22.4 dm3<\/sup> mol-1<\/sup> at STP]
\nSolution:<\/strong>
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\nZn(s) + 2HNO3<\/sub>(aq) \u27f6 \u00a0Zn(NO3<\/sub>)2<\/sub>(aq) + H2<\/sub>(g)
\n[Relative atomic mass: Zn, 65. Molar volume: 24 dm3<\/sup> mol-1<\/sup>\u00a0at room conditions]
\nSolution:<\/strong>
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\n[Relative atomic mass: Al, 27]
\nSolution:<\/strong>
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\n[Relative atomic mass: Cl, 35.5; Ag, 108]
\nSolution:
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