17) What is the (Delta Hrxn) for the reaction?
a) -200.5 kJ
b) -2219 kJ
c) -3182.5 kJ
d) -2389.5 kJ
e) -2267.7 kJ<\/p>\n\n\n\n
18) Based on the (Delta Hrxn) for the reaction, we can argue that:
a) The reaction is exothermic
b) The reaction is endothermic
c) The system released a lot of energy and the surroundings did not absorb it
d) The surroundings gave a little energy to the system for the reaction to occur
e) None of the above<\/p>\n\n\n\n
19) Hess’s Law is interesting because it allows you to determine the (Delta Hxrn) for a reaction using the (Delta H) of others. This is possible because:
a) The (Delta Hxrn) is only dependent on the initial and final states.
b) The (Delta Hxrn) is a function of the step. So I can use the others (Delta H) of the other reactions
c) (Delta Hxrn) is a function of the state.
d) Statements a and c are correct.
e) Statements a and b are correct<\/p>\n\n\n\n
20) In the exercise you just did, to use Equation 3 in determining the (Delta Hxrn), I have to:
a) Leave it the same and multiply the (Delta H) they give me by 2
b) Invert it and multiply the (Delta H) they give me by 2
c) Invest it and also change the sign of the (Delta H) that they give me
d) I don’t have to do anything.
e) I just have to change the sign of the (Delta H) they give me.<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n Here are the correct answers:<\/p>\n\n\n\n 17) What is the (\u0394Hrxn) for the reaction?<\/strong> 18) Based on the (\u0394Hrxn) for the reaction, we can argue that:<\/strong> 19) Hess\u2019s Law is interesting because it allows you to determine the (\u0394Hrxn) for a reaction using the (\u0394H) of others. This is possible because:<\/strong> 20) In the exercise you just did, to use Equation 3 in determining the (\u0394Hrxn), I have to:<\/strong> To determine the enthalpy change (\u0394Hrxn) for the reaction, we need to apply Hess\u2019s Law, which states that the enthalpy change of a reaction depends only on the initial and final states, not the pathway taken. The correct answer is -2267.7 kJ<\/strong>, meaning the reaction releases this much energy.<\/p>\n\n\n\n Since \u0394Hrxn is negative, the reaction is exothermic<\/strong>. This means the system releases energy to the surroundings. The only correct answer is (a) The reaction is exothermic<\/strong>.<\/p>\n\n\n\n Hess\u2019s Law states that enthalpy is a state function<\/strong>, meaning that the overall enthalpy change only depends on the initial and final states, not the steps in between. This allows us to determine \u0394Hrxn using other reactions. The correct answer is d) Statements a and c are correct<\/strong>, since enthalpy depends only on the state<\/strong>, not the steps.<\/p>\n\n\n\n If we use Equation 3 to determine \u0394Hrxn, we may need to invert it, which means reversing the reaction and changing the sign of \u0394H<\/strong>. This follows the principle that if a reaction is flipped, the enthalpy sign must also flip. The correct answer is (c) Invert it and also change the sign of the (\u0394H) that they give me.<\/strong><\/p>\n","protected":false},"excerpt":{"rendered":" 17) What is the (Delta Hrxn) for the reaction?a) -200.5 kJb) -2219 kJc) -3182.5 kJd) -2389.5 kJe) -2267.7 kJ 18) Based on the (Delta Hrxn) for the reaction, we can argue that:a) The reaction is exothermicb) The reaction is endothermicc) The system released a lot of energy and the surroundings did not absorb itd) The […]<\/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-187376","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187376","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=187376"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187376\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187376"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187376"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187376"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Answer: e) -2267.7 kJ<\/strong><\/p>\n\n\n\n
Answer: a) The reaction is exothermic<\/strong><\/p>\n\n\n\n
Answer: d) Statements a and c are correct.<\/strong><\/p>\n\n\n\n
Answer: c) Invert it and also change the sign of the (\u0394H) that they give me.<\/strong><\/p>\n\n\n\n
\n\n\n\nExplanation:<\/h3>\n\n\n\n
Question 17:<\/h4>\n\n\n\n
Question 18:<\/h4>\n\n\n\n
Question 19:<\/h4>\n\n\n\n
Question 20:<\/h4>\n\n\n\n