a:5:{s:8:"template";s:8138:"<!DOCTYPE html>
<html lang="en-US">

<head>
<meta charset="utf-8"/>
<meta content="width=device-width" name="viewport"/>
<title>{{ keyword }}</title>
<link href="http://gmpg.org/xfn/11" rel="profile"/>


<link href="http://fonts.googleapis.com/css?family=Open+Sans:400italic,700italic,400,700&amp;subset=latin,latin-ext" id="twentytwelve-fonts-css" media="all" rel="stylesheet" type="text/css"/>
<style id="twentytwelve-style-css" media="all" rel="stylesheet" type="text/css">/*



/* =Reset
-------------------------------------------------------------- */

html, body, div, h1, h2, h3, a, ul, li, footer, header, hgroup, nav {
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	padding: 0;
	border: 0;
	font-size: 100%;
	vertical-align: baseline;
}
body {
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ul {
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h1,
h2,
h3 {
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}
html {
	overflow-y: scroll;
	font-size: 100%;
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	-ms-text-size-adjust: 100%;
}
a:focus {
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}
footer,
header,
hgroup,
nav {
	display: block;
}

/* Clearing floats */
.wrapper:after {
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}
.wrapper:before,
.wrapper:after {
	display: table;
	content: "";
}


.menu-toggle {
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	box-shadow: 0 1px 2px rgba(64, 64, 64, 0.1);
}
.menu-toggle {
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}
.menu-toggle:hover {
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.menu-toggle:active {
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}


/* Body, links, basics */
html {
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}
body {
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	font-family: Helvetica, Arial, sans-serif;
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}
body.custom-font-enabled {
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a {
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a:hover {
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}

/* Assistive text */
.assistive-text {
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.main-navigation .assistive-text:hover,
.main-navigation .assistive-text:active,
.main-navigation .assistive-text:focus {
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	border-radius: 3px;
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	display: block;
	font-size: 12px;
	padding: 12px;
	position: absolute;
	top: 5px;
	left: 5px;
	z-index: 100000; /* Above WP toolbar */
}

/* Page structure */
.site {
	padding: 0 24px;
	padding: 0 1.714285714rem;
	background-color: #fff;
}

/* Header */
.site-header {
	padding: 24px 0;
	padding: 1.714285714rem 0;
}
.site-header h1,
.site-header h2 {
	text-align: center;
}
.site-header h1 a {
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	display: inline-block;
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}
.site-header h1 a:hover {
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}
.site-header h1 {
	font-size: 24px;
	font-size: 1.714285714rem;
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.site-header h2 {
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	font-size: 0.928571429rem;
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/* Navigation Menu */
.main-navigation {
	margin-top: 24px;
	margin-top: 1.714285714rem;
	text-align: center;
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.main-navigation li {
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	margin-top: 1.714285714rem;
	font-size: 12px;
	font-size: 0.857142857rem;
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.main-navigation a {
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.main-navigation a:hover {
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}
.main-navigation div.nav-menu > ul {
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}
.menu-toggle {
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}

/* Banner */

/* Sidebar */

/* Footer */
footer[role="contentinfo"] {
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	clear: both;
	font-size: 12px;
	font-size: 0.857142857rem;
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	margin-top: 24px;
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footer[role="contentinfo"] a {
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footer[role="contentinfo"] a:hover {
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/* Minimum width of 600 pixels. */
@media screen and (min-width: 600px) {
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		max-width: 68.571428571rem;
		overflow: hidden;
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	.site-header h1,
	.site-header h2 {
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		line-height: 1.846153846;
		margin-bottom: 0;
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	.main-navigation div.nav-menu > ul {
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		border-top: 1px solid #ededed;
		display: inline-block !important;
		text-align: left;
		width: 100%;
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	.main-navigation ul {
		margin: 0;
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	.main-navigation li a,
	.main-navigation li {
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		text-decoration: none;
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	.main-navigation li a {
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	.main-navigation li a:hover {
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	.main-navigation li {
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		margin: 0 2.857142857rem 0 0;
		position: relative;
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	.menu-toggle {
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}

/* Minimum width of 960 pixels. */
@media screen and (min-width: 960px) {
	body {
		background-color: #e6e6e6;
	}
	body .site {
		padding: 0 40px;
		padding: 0 2.857142857rem;
		margin-top: 48px;
		margin-top: 3.428571429rem;
		margin-bottom: 48px;
		margin-bottom: 3.428571429rem;
		box-shadow: 0 2px 6px rgba(100, 100, 100, 0.3);
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}


/* =Print
----------------------------------------------- */

@media print {
	body {
		background: none !important;
		color: #000;
		font-size: 10pt;
	}
	a {
		text-decoration: none;
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	.site {
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		max-width: 100%;
		position: relative !important;
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	.site-header {
		margin-bottom: 72px;
		margin-bottom: 5.142857143rem;
		text-align: left;
	}
	.site-header h1 {
		font-size: 21pt;
		line-height: 1;
		text-align: left;
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	.site-header h2 {
		color: #000;
		font-size: 10pt;
		text-align: left;
	}
	.site-header h1 a {
		color: #000;
	}
	#colophon,
	.main-navigation {
		display: none;
	}
	.wrapper {
		border-top: none;
		box-shadow: none;
	}
}
</style>


<style type="text/css">.recentcomments a{display:inline !important;padding:0 !important;margin:0 !important;}</style>
</head>
<body class="custom-font-enabled single-author">
<div class="hfeed site" id="page">
<header class="site-header" id="masthead" role="banner">
<hgroup>
<h1 class="site-title"><a href="#" rel="home" title="{{ keyword }}">{{ keyword }}</a></h1>
<h2 class="site-description">Just another WordPress site</h2>
</hgroup>
<nav class="main-navigation" id="site-navigation" role="navigation">
<h3 class="menu-toggle">Menu</h3>
<a class="assistive-text" href="#" title="Skip to content">Skip to content</a>
<div class="nav-menu"><ul><li><a href="#" title="Home">Home</a></li><li class="page_item page-item-2"><a href="#">Sample Page</a></li></ul></div>
</nav>
</header>
<div class="wrapper" id="main">
{{ text }}
	</div>
<footer id="colophon" role="contentinfo">
{{ links }}
<div class="site-info">
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</body>
</html>";s:4:"text";s:4495:"Calculate the approximate enthalpy change for the combustion of methane: CH4 + 2O2 --->2H2O + CO2 deltaH(CH4) = 1656 KJ/mol deltaH(O2) = ? 2H 2 (g) + O 2 (g)  2H 2 O(l)..... DH = -571.6 kJ. Use small soup tins that fit loosely into a jam jar. Using Bond Energies to calculate enthalpy (H) of a reaction . Calculate the approximate enthalpy change, Delta H(rxn) for the combustion of methane: CH4 + 2O2 ----> 2H2O + CO2 Use the values you calculated in Parts A, B, C, and D, keeping in mind the stoichiometric coefficients. The enthalpy of combustion per mole of methanol is calculated by summing the bond energies for all reactants (accounting for stoichiometric ratios), and subtracting from that sum the bond energies for all products (since the formation of a bond releases energy). 1.28 Simple calorimeter See diagram 22.1.8: Simple calorimeter 1. H = H products  H reactants.  Calculate the enthalpy change for the reaction: NH. Calculate the approximate enthalpy change , h, for the combustion of methane: ch4+2o22h2o+co2 use the values you calculated in parts a to d, keeping in - 7788108 4. It is usually expressed in units of kJ mol-1, measured at 298 K. The exact bond enthalpy of a particular chemical bond depends upon the molecular environment in which the bond exists. Bond energies and enthalpy can show if a reaction is endothermic or exothermic. Calculate Enthalpy Changes Using Hess's Law. The enthalpy change of a reaction depends upon the state of the reactants and products. The enthalpy change for a chemical reaction is the difference. Calculate the approximate enthalpy change for the combustion of methane: CH4 + 2O2 ---> 2H20 + CO2 2. Methane (CH4) is a major constituent of natural gas. calculate the enthalpy of combustion of ethane. Early experimental effort at providing home tuition in chemistry via YouTube. View Notes - Chemistry-Solution from CHEMISTRY AP Chemist at Bethlehem Catholic High School. Using the data supplied in the table below, calculate the enthalpy of combustion of methane in kJ (kmol of fuel)-1 at 105 Pa. Study Chemistry 166 Chemistry and Chemical Reactivity 8th Edition.pdf notes from Kristen T. Calculate the approximate enthalpy change for the combustion of methane: CH4 + 2O2 --->2H2O + CO2 deltaH(CH4) = 1656 KJ/mol deltaH(O2) = By definition, the heat of combustion (enthalpy of combustion, H c) is minus the enthalpy change for the combustion reaction, ie, -H. So, by convention, the molar heat of combustion (molar enthalpy of combustion) is 1. calculate the approximate enthalpy change, Hrxn, for the combustion of one mole of methane a shown in the balanced chemical equation: ch4+2o22h2o+co2 Use the values 1656kJ/mol, 498kJ/mol, -928kJ/mol, -1598kJ/mol , keeping in mind the stoichiometric coefficients. 2H 2 (g) + O 2 (g)  2H 2 O(g)..... DH = -483.6 kJ. ... Use bond energies to estimate the enthalpy change for the combustion of methane. ... 3 1/2 O 2. Relevant equations CH4 + 2O2 -- 4. An overview of rocket propulsion including basic thrust equation, engine design considerations, and example problems. 1. Question Part E Calculate the approximate enthalpy change , H, for the combustion of methane: CH4+2O22H2O+CO2 Therefore, bond enthalpy values given in chemical data books are averaged What Is Enthalpy? This example shows how to determine enthalpy change of a reaction. The reaction enthalpy calculator on the right will facilitate these calculations. C2H5OH + 3O2 >> CO2 + 3H2O. This implies that the enthalpy of 2 moles of water in the liquid state is 88 kJ lower than 2 moles of water in the gaseous state. Calculate the approximate enthalpy change, Hrxn, for the combustion of methane: CH4+2O22H2O+CO2 Hrxn from a given table: CH4 = 1656 kJ/mol The enthalpy change delta H for the combustion of methan is -891kJ/mol. The Bond Enthalpy is the energy required to break a chemical bond. The complete combustion of methane, ... calculate the standard change of enthalpy for the combustion of coal. Assume the initial temperature of the water is 21 C, and the methane is at 1 bar and 25 C. Assume that methane is an ideal gas, the specific heat capacity of water to be constant and ... chemistry Calculate enthalpy change of reaction for the combustion of gaseous ethanol. Enthalpy of combustion is the enthalpy change during combustion of a substance in the presence of oxygen. Calculate the enthalpy change for the combustion of methane gas, CH4, to form CO2(g) & H2O(l). Using standard molar enthalpies of formation. ";s:7:"keyword";s:71:"calculate the approximate enthalpy change for the combustion of methane";s:5:"links";s:4117:"<a href='http://reklama.disigma.lt/tmp/docs/0e040.php?e0b334=soda-ash-manufacturers-in-russia'>Soda Ash Manufacturers In Russia</a>,
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