{"id":220285,"date":"2025-05-28T05:37:10","date_gmt":"2025-05-28T05:37:10","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=220285"},"modified":"2025-05-28T05:37:14","modified_gmt":"2025-05-28T05:37:14","slug":"calcium-carbide-reacts-with-water-to-produce-acetylene-gas-c2h2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/28\/calcium-carbide-reacts-with-water-to-produce-acetylene-gas-c2h2\/","title":{"rendered":"Calcium carbide reacts with water to produce acetylene gas, C2H2."},"content":{"rendered":"\n<p>Calcium carbide reacts with water to produce acetylene gas, C2H2. Calculate the volume (in liters) of acetylene produced at 25.0 \u00b0C and 685 mmHg from 0.0750 mol CaC2 and excess H2O. Given that R = 0.0821 L-atm\/(mol-K). CaC2(s) + 2H2O(l) -> Ca(OH)2(aq) + C2H2(g) a. 4.75 L. b. 2.04 L. c. 3.39 L. d. 2.72 L. e. 4.07 L.<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To determine the volume of acetylene gas (C\u2082H\u2082) produced, we use the <strong>Ideal Gas Law<\/strong>: PV=nRTPV = nRT<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>PP = pressure in atm<\/li>\n\n\n\n<li>VV = volume in liters<\/li>\n\n\n\n<li>nn = moles of gas<\/li>\n\n\n\n<li>RR = ideal gas constant = 0.0821 L\u00b7atm\/(mol\u00b7K)<\/li>\n\n\n\n<li>TT = temperature in Kelvin<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 1: Identify the amount of gas produced<\/strong><\/h3>\n\n\n\n<p>From the balanced equation: CaC2(s)+2H2O(l)\u2192Ca(OH)2(aq)+C2H2(g)\\text{CaC}_2(s) + 2\\text{H}_2\\text{O}(l) \\rightarrow \\text{Ca(OH)}_2(aq) + \\text{C}_2\\text{H}_2(g)<\/p>\n\n\n\n<p>1 mole of <strong>CaC\u2082<\/strong> produces 1 mole of <strong>C\u2082H\u2082<\/strong> gas.<br>Given: 0.0750 mol CaC\u2082 \u2192 produces <strong>0.0750 mol of C\u2082H\u2082<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 2: Convert pressure to atm<\/strong><\/h3>\n\n\n\n<p>685&nbsp;mmHg\u00d71&nbsp;atm760&nbsp;mmHg=0.901atm685 \\text{ mmHg} \\times \\frac{1 \\text{ atm}}{760 \\text{ mmHg}} = 0.901 atm<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 3: Convert temperature to Kelvin<\/strong><\/h3>\n\n\n\n<p>T=25.0\u00b0C+273.15=298.15KT = 25.0\u00b0C + 273.15 = 298.15 K<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 4: Plug values into the Ideal Gas Law<\/strong><\/h3>\n\n\n\n<p>V=nRTP=(0.0750&nbsp;mol)(0.0821\u2009L\\cdotpatm\/mol\\cdotpK)(298.15&nbsp;K)0.901&nbsp;atmV = \\frac{nRT}{P} = \\frac{(0.0750 \\text{ mol}) (0.0821 \\, \\text{L\u00b7atm\/mol\u00b7K}) (298.15 \\text{ K})}{0.901 \\text{ atm}} V=1.834\u2009L\\cdotpatm0.901\u2009atm\u22482.04\u2009LV = \\frac{1.834 \\, \\text{L\u00b7atm}}{0.901 \\, \\text{atm}} \\approx 2.04 \\, \\text{L}<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">\u2705 <strong>Correct Answer: b. 2.04 L<\/strong><\/h3>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation<\/strong><\/h3>\n\n\n\n<p>In this problem, we calculate the volume of acetylene gas (C\u2082H\u2082) produced from a chemical reaction between calcium carbide (CaC\u2082) and water. The balanced chemical reaction shows that one mole of calcium carbide produces one mole of acetylene gas, assuming excess water is present.<\/p>\n\n\n\n<p>We start with 0.0750 mol of CaC\u2082. This directly gives 0.0750 mol of C\u2082H\u2082 since the mole ratio is 1:1. Next, we apply the Ideal Gas Law equation PV=nRTPV = nRT, which relates pressure (P), volume (V), temperature (T), and the number of moles (n) for an ideal gas.<\/p>\n\n\n\n<p>To use this formula, the pressure must be in atmospheres (atm), and the temperature must be in Kelvin (K). The pressure is given in mmHg, so we convert 685 mmHg to atm using the conversion factor 1&nbsp;atm=760&nbsp;mmHg1 \\text{ atm} = 760 \\text{ mmHg}, which results in 0.901 atm. Similarly, the temperature is converted from Celsius to Kelvin by adding 273.15, resulting in 298.15 K.<\/p>\n\n\n\n<p>Substituting these values into the Ideal Gas Law formula with the gas constant R=0.0821&nbsp;L\\cdotpatm\/(mol\\cdotpK)R = 0.0821 \\text{ L\u00b7atm\/(mol\u00b7K)}, we solve for volume VV. After calculations, the result is approximately 2.04 liters.<\/p>\n\n\n\n<p>This calculation assumes ideal gas behavior, which is a good approximation under many standard conditions like 25\u00b0C and around 1 atm pressure. The final volume reflects how much space 0.0750 mol of acetylene gas occupies under those conditions.<\/p>\n\n\n\n<p>Thus, the correct answer is <strong>b. 2.04 L<\/strong>.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/learnexams-banner10-26.jpeg\" alt=\"\" class=\"wp-image-220286\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Calcium carbide reacts with water to produce acetylene gas, C2H2. Calculate the volume (in liters) of acetylene produced at 25.0 \u00b0C and 685 mmHg from 0.0750 mol CaC2 and excess H2O. Given that R = 0.0821 L-atm\/(mol-K). CaC2(s) + 2H2O(l) -> Ca(OH)2(aq) + C2H2(g) a. 4.75 L. b. 2.04 L. c. 3.39 L. d. 2.72 [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-220285","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/220285","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=220285"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/220285\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=220285"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=220285"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=220285"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}