{"id":48412,"date":"2019-11-10T10:38:13","date_gmt":"2019-11-10T09:38:13","guid":{"rendered":"https:\/\/www.thermal-engineering.org\/o-que-e-alteracao-de-entalpia-delta-h-definicao\/"},"modified":"2020-01-29T10:30:39","modified_gmt":"2020-01-29T09:30:39","slug":"o-que-e-alteracao-de-entalpia-delta-h-definicao","status":"publish","type":"post","link":"https:\/\/www.thermal-engineering.org\/pt-br\/o-que-e-alteracao-de-entalpia-delta-h-definicao\/","title":{"rendered":"O que \u00e9 altera\u00e7\u00e3o de entalpia – delta h – Defini\u00e7\u00e3o"},"content":{"rendered":"
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A entalpia \u00e9 representada pelo s\u00edmbolo H, e a altera\u00e7\u00e3o na entalpia em um processo (delta h) \u00e9 H2 – H1.\u00a0O delta h \u00e9 aqui calculado para v\u00e1rios exemplos.\u00a0Engenharia T\u00e9rmica<\/div>\n<\/div>\n
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Entalpia em unidades extensivas<\/h2>\n
\"Propriedades<\/a>
Propriedades extensivas e intensivas do meio no pressurizador.<\/figcaption><\/figure>\n

H = U + pV<\/strong><\/em><\/p>\n

A entalpia<\/strong><\/a>\u00a0\u00a0\u00e9 uma quantidade extensa, depende do tamanho do sistema ou da quantidade de subst\u00e2ncia que ele cont\u00e9m.\u00a0A unidade SI de entalpia \u00e9 o joule (J).\u00a0\u00c9 a energia contida no sistema, excluindo a energia cin\u00e9tica do movimento do sistema como um todo e a energia potencial do sistema como um todo devido a campos de for\u00e7a externos.\u00a0\u00c9 a quantidade termodin\u00e2mica equivalente ao\u00a0conte\u00fado total de calor<\/strong>\u00a0de um sistema.<\/p>\n

Por outro lado, a energia pode ser armazenada nas liga\u00e7\u00f5es qu\u00edmicas entre os \u00e1tomos que comp\u00f5em as mol\u00e9culas.\u00a0Esse armazenamento de energia no n\u00edvel at\u00f4mico inclui energia associada a estados orbitais de el\u00e9trons, rota\u00e7\u00e3o nuclear e for\u00e7as de liga\u00e7\u00e3o no n\u00facleo.<\/p>\n

A entalpia<\/strong>\u00a0\u00e9 representada pelo s\u00edmbolo\u00a0H<\/strong>\u00a0, e a altera\u00e7\u00e3o na entalpia (delta H) em um processo \u00e9\u00a0H\u00a02<\/sub>\u00a0– H\u00a01<\/sub><\/strong>\u00a0.<\/p>\n

Existem express\u00f5es em termos de vari\u00e1veis \u200b\u200bmais familiares, como\u00a0temperatura<\/a>\u00a0e\u00a0press\u00e3o<\/a>\u00a0:<\/p>\n

dH = C\u00a0p<\/sub>\u00a0dT + V (1-aT) dp<\/strong><\/em><\/p>\n

Onde\u00a0C\u00a0p<\/sub><\/strong>\u00a0\u00e9 a\u00a0capacidade calor\u00edfica a press\u00e3o constante<\/strong>\u00a0e\u00a0\u03b1<\/em><\/strong>\u00a0\u00e9 o coeficiente de expans\u00e3o t\u00e9rmica (c\u00fabico).\u00a0Para o g\u00e1s ideal \u03b1T = 1 e, portanto:<\/p>\n

dH = C\u00a0p<\/sub>\u00a0dT<\/em><\/strong><\/p>\n<\/div>\n<\/div>\n

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Exemplo: Pist\u00e3o sem atrito – Calor – Entalpia<\/span><\/h2>\n
\"Entalpia<\/a>
Calcule a temperatura final, se 3000 kJ de calor forem adicionados.<\/span><\/figcaption><\/figure>\n

Um pist\u00e3o sem atrito \u00e9 usado para proporcionar uma press\u00e3o constante de\u00a0<\/span>500 kPa<\/span><\/strong>\u00a0num cilindro contendo vapor (\u00a0<\/span>vapor sobreaquecido<\/span><\/a>\u00a0) de um volume de\u00a0<\/span>2 m\u00a0<\/span>3<\/span><\/sup><\/strong>\u00a0\u00a0a\u00a0<\/span>500 K<\/span><\/strong>\u00a0.\u00a0Calcule a temperatura final, se\u00a0<\/span>3000 kJ<\/span><\/strong>\u00a0de\u00a0<\/span>calor<\/span><\/strong>\u00a0forem adicionados.<\/span><\/p>\n

Solu\u00e7\u00e3o:<\/span><\/strong><\/p>\n

Usando\u00a0<\/span>tabelas de vapor<\/span><\/a>\u00a0, sabemos que a\u00a0<\/span>entalpia espec\u00edfica<\/span><\/strong>\u00a0desse vapor (500 kPa; 500 K) \u00e9 de cerca de\u00a0<\/span>2912 kJ \/ kg<\/span><\/strong>\u00a0.\u00a0Como nessa condi\u00e7\u00e3o o vapor possui densidade de 2,2 kg \/ m\u00a0<\/span>3<\/span><\/sup>\u00a0, sabemos que h\u00e1 cerca de\u00a0<\/span>4,4 kg de vapor<\/span><\/strong>\u00a0no pist\u00e3o na entalpia de 2912 kJ \/ kg x 4,4 kg =\u00a0<\/span>12812 kJ<\/span><\/strong>\u00a0.<\/span><\/p>\n

Quando usamos simplesmente\u00a0<\/span>Q = H\u00a0<\/span>2<\/span><\/sub>\u00a0– H\u00a0<\/span>1<\/span><\/sub><\/strong>\u00a0, a entalpia resultante do vapor ser\u00e1:<\/span><\/p>\n

H\u00a0<\/span>2<\/span><\/sub>\u00a0= H\u00a0<\/span>1<\/span><\/sub>\u00a0+ Q =\u00a0<\/span>15812 kJ<\/span><\/strong><\/p>\n

Nas\u00a0<\/span>tabelas de vapor<\/span><\/strong>\u00a0, esse vapor superaquecido (15812 \/ 4,4 = 3593 kJ \/ kg) ter\u00e1 uma temperatura de\u00a0<\/span>828 K (555 \u00b0 C)<\/span><\/strong>\u00a0.\u00a0Uma vez que nesta entalpia do vapor tem a densidade de 1,31 kg \/ m\u00a0<\/span>3<\/span><\/sup>\u00a0, \u00e9 \u00f3bvio que se expandiu em cerca de 2,2 \/ 1,31 = 1,67 (+ 67%).\u00a0Portanto, o volume resultante \u00e9 de 2 m\u00a0<\/span>3<\/span><\/sup>\u00a0x 1,67 = 3,34 m\u00a0<\/span>3<\/span><\/sup>\u00a0e \u2206V = 3,34 m\u00a0<\/span>3<\/span><\/sup>\u00a0– 2 m\u00a0<\/span>3<\/span><\/sup>\u00a0= 1,34 m\u00a0<\/span>3<\/span><\/sup>\u00a0.<\/span><\/p>\n

A\u00a0parte\u00a0<\/span>p\u2206V<\/span><\/strong>\u00a0da entalpia, ou seja, o trabalho realizado \u00e9:<\/span><\/p>\n

W = p\u2206V = 500 000 Pa x 1,34 m\u00a0<\/span>3<\/span><\/sup>\u00a0= 670 kJ<\/span><\/strong><\/p>\n<\/div>\n<\/div>\n

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Entalpia em unidades intensivas – Entalpia espec\u00edfica<\/span><\/h2>\n

A\u00a0<\/span>entalpia<\/span><\/strong>\u00a0pode ser transformada em uma\u00a0vari\u00e1vel\u00a0<\/span>intensiva<\/span><\/strong>\u00a0ou\u00a0<\/span>espec\u00edfica<\/span><\/strong>\u00a0dividindo-se pela\u00a0<\/span>massa<\/span><\/a>\u00a0.\u00a0<\/span>Os engenheiros usam mais a\u00a0<\/span><\/strong>entalpia espec\u00edfica<\/span><\/strong>\u00a0na an\u00e1lise termodin\u00e2mica do que a pr\u00f3pria entalpia.\u00a0A entalpia espec\u00edfica (h) de uma subst\u00e2ncia \u00e9 a sua entalpia por unidade de massa.\u00a0\u00c9 igual \u00e0 entalpia total (H) dividida pela massa total (m).<\/span><\/p>\n

h = H \/ m<\/span><\/em><\/strong><\/p>\n

Onde:<\/span><\/p>\n

h = entalpia espec\u00edfica (J \/ kg)<\/span><\/p>\n

H = entalpia (J)<\/span><\/p>\n

m = massa (kg)<\/span><\/p>\n

Observe que a entalpia \u00e9 a quantidade termodin\u00e2mica equivalente ao\u00a0<\/span>conte\u00fado total de calor<\/span><\/strong>\u00a0de um sistema.\u00a0A entalpia espec\u00edfica \u00e9 igual \u00e0\u00a0<\/span>energia interna espec\u00edfica<\/span><\/a>\u00a0do sistema mais o produto da\u00a0<\/span>press\u00e3o<\/span><\/a>\u00a0e\u00a0<\/span>volume espec\u00edfico<\/span><\/a>\u00a0.<\/span><\/p>\n

h = u + pv<\/span><\/strong><\/em><\/p>\n

Em geral, a entalpia \u00e9 uma\u00a0<\/span>propriedade de uma subst\u00e2ncia<\/span><\/strong>\u00a0, como press\u00e3o, temperatura e volume, mas n\u00e3o pode ser medida diretamente.\u00a0Normalmente, a entalpia de uma subst\u00e2ncia \u00e9 dada com rela\u00e7\u00e3o a algum valor de refer\u00eancia.\u00a0Por exemplo, a entalpia espec\u00edfica da \u00e1gua ou vapor \u00e9 dada usando a refer\u00eancia de que a entalpia espec\u00edfica da \u00e1gua \u00e9\u00a0<\/span>zero a 0,01 \u00b0 C<\/span><\/strong>\u00a0e\u00a0<\/span>press\u00e3o atmosf\u00e9rica normal<\/span><\/strong><\/a>\u00a0, em que\u00a0<\/span>h\u00a0<\/span>L<\/span><\/sub>\u00a0= 0,00 kJ \/ kg<\/span><\/strong>\u00a0.\u00a0O fato de o valor absoluto da entalpia espec\u00edfica ser desconhecido n\u00e3o \u00e9 um problema, no entanto, porque \u00e9 a\u00a0<\/span>altera\u00e7\u00e3o na entalpia espec\u00edfica (\u2206h)<\/span><\/strong>\u00a0e n\u00e3o o valor absoluto que \u00e9 importante nos problemas pr\u00e1ticos.<\/span><\/p>\n<\/div>\n<\/div>\n

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Altera\u00e7\u00f5es na entalpia nas rea\u00e7\u00f5es qu\u00edmicas<\/span><\/h2>\n
\"Combust\u00e3o<\/a>
Em uma chama de g\u00e1s hidrog\u00eanio puro, queimando no ar, o hidrog\u00eanio (H2) reage com o oxig\u00eanio (O2) para formar \u00e1gua (H2O) e libera energia.<\/span><\/figcaption><\/figure>\n

Considere a\u00a0<\/span>combust\u00e3o de hidrog\u00eanio<\/span><\/strong>\u00a0no ar.\u00a0Em uma chama de g\u00e1s hidrog\u00eanio puro, queimando no ar, o\u00a0<\/span>hidrog\u00eanio (H\u00a0<\/span>2<\/span><\/sub>\u00a0)<\/span><\/strong>\u00a0reage com o\u00a0\u00a0<\/span>oxig\u00eanio (O\u00a0<\/span>2<\/span><\/sub>\u00a0)<\/span><\/strong>\u00a0para formar\u00a0<\/span>\u00e1gua (H\u00a0<\/span>2<\/span><\/sub>\u00a0O)<\/span><\/strong>\u00a0e\u00a0<\/span>libera energia<\/span><\/strong>\u00a0.<\/span><\/p>\n

Energicamente, o processo pode ser considerado para exigir a energia para dissociar o\u00a0<\/span>H\u00a0<\/span>2<\/span><\/sub>\u00a0<\/strong>\u00a0e\u00a0<\/span>O\u00a0<\/span>2<\/span><\/sub><\/strong>\u00a0, mas, em seguida, a liga\u00e7\u00e3o do inibidor da H\u00a0<\/span>2<\/span><\/sub>\u00a0O retorna o sistema para um estado ligado com\u00a0<\/span>potencial negativo<\/span><\/strong>\u00a0.\u00a0Na verdade, \u00e9\u00a0<\/span>mais negativo do<\/span><\/strong>\u00a0que os estados ligados dos reagentes, e a forma\u00e7\u00e3o das duas mol\u00e9culas de \u00e1gua \u00e9, portanto, uma\u00a0<\/span>rea\u00e7\u00e3o exot\u00e9rmica<\/span><\/strong>\u00a0, que libera 5,7 eV de energia.\u00a0Em palavras de entalpia, a entalpia de combust\u00e3o \u00e9 \u2212286 kJ \/ mol:<\/span><\/p>\n

2H\u00a0<\/span>2<\/span><\/sub>\u00a0(g) + O\u00a0<\/span>2<\/span><\/sub>\u00a0(g) \u2192 2H\u00a0<\/span>2<\/span><\/sub>\u00a0O (g)<\/span><\/strong><\/p>\n

Em palavras de entalpia, a entalpia de combust\u00e3o \u00e9 \u2212286 kJ \/ mol (energia por mol de hidrog\u00eanio molecular):<\/span><\/p>\n

2H\u00a0<\/span>2<\/span><\/sub>\u00a0(g) + O\u00a0<\/span>2<\/span><\/sub>\u00a0(g) \u2192 2H\u00a0<\/span>2<\/span><\/sub>\u00a0O (l) +572 kJ<\/span><\/strong><\/p>\n

O balan\u00e7o de energia antes e depois da rea\u00e7\u00e3o pode ser ilustrado esquematicamente com o estado em que todos os \u00e1tomos s\u00e3o livres, tomados como refer\u00eancia de energia.<\/span><\/p>\n<\/div>\n<\/div>\n

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Entalpia de vaporiza\u00e7\u00e3o<\/span><\/h2>\n
\"Calor<\/a>
O calor da vaporiza\u00e7\u00e3o diminui com o aumento da press\u00e3o, enquanto o ponto de ebuli\u00e7\u00e3o aumenta.\u00a0Ele desaparece completamente em um determinado ponto chamado ponto cr\u00edtico.<\/span><\/figcaption><\/figure>\n

Em geral, quando um material\u00a0<\/span>muda de fase<\/span><\/strong>\u00a0de s\u00f3lido para l\u00edquido ou de l\u00edquido para g\u00e1s, uma certa quantidade de energia est\u00e1 envolvida nessa mudan\u00e7a de fase.\u00a0No caso de mudan\u00e7a de fase de l\u00edquido para g\u00e1s, essa quantidade de energia \u00e9 conhecida como\u00a0<\/span>entalpia de vaporiza\u00e7\u00e3o<\/span><\/strong>\u00a0(s\u00edmbolo \u2206H\u00a0<\/span>vap<\/span><\/sub>\u00a0; unidade: J), tamb\u00e9m conhecida como\u00a0<\/span>calor (latente) de vaporiza\u00e7\u00e3o<\/span><\/strong>\u00a0ou calor de evapora\u00e7\u00e3o.\u00a0Calor latente \u00e9 a quantidade de calor adicionada ou removida de uma subst\u00e2ncia para produzir uma mudan\u00e7a de fase.\u00a0Essa energia decomp\u00f5e as for\u00e7as atraentes intermoleculares e tamb\u00e9m deve fornecer a energia necess\u00e1ria para expandir o g\u00e1s (o\u00a0<\/span>trabalho p\u0394V<\/span><\/strong>)\u00a0Quando o calor latente \u00e9 adicionado, nenhuma mudan\u00e7a de temperatura ocorre.\u00a0A entalpia da vaporiza\u00e7\u00e3o \u00e9 uma fun\u00e7\u00e3o da press\u00e3o na qual essa transforma\u00e7\u00e3o ocorre.<\/span><\/p>\n

Calor latente de vaporiza\u00e7\u00e3o – \u00e1gua a 0,1 MPa (press\u00e3o atmosf\u00e9rica)<\/span><\/p>\n

h\u00a0<\/span>lg<\/span><\/sub>\u00a0= 2257 kJ \/ kg<\/span><\/strong><\/p>\n

Calor latente de vaporiza\u00e7\u00e3o – \u00e1gua a 3 MPa (press\u00e3o dentro de um gerador de vapor)<\/span><\/p>\n

h\u00a0<\/span>lg<\/span><\/sub>\u00a0= 1795 kJ \/ kg<\/span><\/strong><\/p>\n

Calor latente de vaporiza\u00e7\u00e3o – \u00e1gua a 16 MPa (press\u00e3o dentro de um\u00a0<\/span>pressurizador<\/span><\/a>\u00a0)<\/span><\/p>\n

h\u00a0<\/span>lg<\/span><\/sub>\u00a0= 931 kJ \/ kg<\/span><\/strong><\/p>\n

O\u00a0<\/span>calor da vaporiza\u00e7\u00e3o<\/span><\/strong>\u00a0diminui com o aumento da press\u00e3o, enquanto o\u00a0<\/span>ponto de ebuli\u00e7\u00e3o<\/span><\/a>\u00a0aumenta.\u00a0Ele desaparece completamente em um determinado ponto chamado\u00a0<\/span>ponto cr\u00edtico<\/span><\/a>\u00a0.\u00a0Acima do ponto cr\u00edtico, as fases l\u00edquida e de vapor s\u00e3o indistingu\u00edveis, e a subst\u00e2ncia \u00e9 chamada de\u00a0<\/span>fluido supercr\u00edtico<\/span><\/a>\u00a0.<\/span><\/p>\n

O calor da vaporiza\u00e7\u00e3o \u00e9 o calor necess\u00e1rio para vaporizar completamente uma unidade de\u00a0<\/span>l\u00edquido saturado<\/span><\/a>\u00a0(ou condensar uma unidade de massa de vapor saturado) e \u00e9 igual a\u00a0<\/span>h\u00a0<\/span>lg<\/span><\/sub>\u00a0= h\u00a0<\/span>g<\/span><\/sub>\u00a0– h\u00a0<\/span>l<\/span><\/sub><\/strong>\u00a0.<\/span><\/p>\n

O calor necess\u00e1rio para derreter (ou congelar) uma unidade de massa na subst\u00e2ncia a press\u00e3o constante \u00e9 o calor da fus\u00e3o e \u00e9 igual a\u00a0<\/span>h\u00a0<\/span>sl<\/span><\/sub>\u00a0= h\u00a0<\/span>l<\/span><\/sub>\u00a0– h\u00a0<\/span>s<\/span><\/sub><\/strong>\u00a0, onde h\u00a0<\/span>s<\/span><\/sub>\u00a0\u00e9 a entalpia do s\u00f3lido saturado e h\u00a0<\/span>l<\/span><\/sub>\u00a0\u00e9 a entalpia do l\u00edquido saturado.<\/span><\/p>\n

\"Mudan\u00e7as<\/a>
Calor latente de vaporiza\u00e7\u00e3o – \u00e1gua a 0,1 MPa.\u00a0Parte dominante do calor absorvido.<\/span><\/figcaption><\/figure>\n<\/div>\n<\/div>\n
……………………………………………………………………………………………………………………………….<\/p>\n

Este artigo \u00e9 baseado na tradu\u00e7\u00e3o autom\u00e1tica do artigo original em ingl\u00eas. Para mais informa\u00e7\u00f5es, consulte o artigo em ingl\u00eas. Voc\u00ea pode nos ajudar. Se voc\u00ea deseja corrigir a tradu\u00e7\u00e3o, envie-a para: translations@nuclear-power.com ou preencha o formul\u00e1rio de tradu\u00e7\u00e3o on-line. Agradecemos sua ajuda, atualizaremos a tradu\u00e7\u00e3o o mais r\u00e1pido poss\u00edvel. Obrigado.<\/p>\n<\/figcaption><\/figure>\n<\/div>\n<\/div>\n","protected":false},"excerpt":{"rendered":"

A entalpia \u00e9 representada pelo s\u00edmbolo H, e a altera\u00e7\u00e3o na entalpia em um processo (delta h) \u00e9 H2 – H1.\u00a0O delta h \u00e9 aqui calculado para v\u00e1rios exemplos.\u00a0Engenharia T\u00e9rmica Entalpia em unidades extensivas Propriedades extensivas e intensivas do meio no pressurizador. H = U + pV A entalpia\u00a0\u00a0\u00e9 uma quantidade extensa, depende do tamanho … Ler mais<\/a><\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":[],"categories":[14],"tags":[],"yoast_head":"\nO que \u00e9 altera\u00e7\u00e3o de entalpia - delta h - Defini\u00e7\u00e3o<\/title>\n<meta name=\"description\" content=\"A entalpia \u00e9 representada pelo s\u00edmbolo H, e a altera\u00e7\u00e3o na entalpia em um processo (delta h) \u00e9 H2 - H1. O delta h \u00e9 aqui calculado para v\u00e1rios exemplos. 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