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The value of x in balanced equation is ...

The value of x in balanced equation is
`C_(6)H_(12)O_(6(aq))+6O_(2(g))to"x"CO_(2(g))+6H_(2)O_((l))+"energy"`

Text Solution

Verified by Experts

The correct Answer is:
6
`C_(6)H_(12)O_(6(aq))+6O_(2(g))to6CO_(2(g))+6H_(2)O_((l))+"energy"`
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The heat envoled in the combustion of glucose is given by the equation C_(6)H_(12)O_(6(s))+6O_(2(g))rarr6CO_(2(g))+6H_(2)O_((g)) DeltaH=-680K.cal, The weight of CO_(2(g)) produced when 170 Kcal of heat is envolved in the combusation of glucose is

The heat evolved in the combustion of glucose is shown in the equation : C_(6)H_(12)O_(6)(s) + 6O_(2)(g) rarr 6CO_(2)(g) + 6H_(2)O (g) , Delta_(c ) H = -2840 kJ mol^(-1) What is the energy requirement for production of 0.36g of glucose by the reverse reaction ?

Knowledge Check

  • According to the equation C_(6)H_(6(l))+7/2 O_(2(g)) rarr 6CO_(2(g))+3H_(2)O_((l)), DeltaH=-xkJ The energy evolved when 3.9 gm of benzene is burnt in air is - 163.2 kJ heat of combustion of benzene is

    A
    32.46 kJ
    B
    16.32 kJ
    C
    326.4 kJ
    D
    `-3264 kJ`

  • The heat evolved in the combustion of benzene is given by the equation: C_(6)H_(6)(g) + (15)/(2) O_(2)(g) to 6CO_(2)(g) + 3H_(2)O(l), DeltaH = - 3264.6 kJ "mol"^(-1) The heat energy changes when 39 g of C_(6)H_(6) are burnt im an open ontainer will be:

    A
    `+ 816.15 kJ "mol"^(-1)`
    B
    `+ 1632.3 kJ "mol"^(-1)`
    C
    `-1632.3 kJ "mol"^(-1)`
    D
    `-2448.45 kJ "mol"^(-1)`

  • The fat C_(57)H_(104)O_(6)(s) , is metabolised via the following reaction C_(57)H_(104)O_(6)(s)+80O_(2)(g)to57CO_(2)(g)+52H_(2)O(1) the energy (kJ) liberated when 1.0 g of this fat reacts will be Given the enthapies of formation Delta_(f)H^(@)(C_(57)H_(104)O_(6)s)=-70870 kJ/mol Delta_(f)H^(@)(H_(2)O,l)=-285.8 kJ/mol Delta_(f)H^(@)(CO_(2),g)=-393.5 kJ/mol

    A
    `-37.98`
    B
    `-40.4`
    C
    `-33.4`
    D
    `-30.2`

    • Similar Questions

    Explore conceptually related problems

    Calculate the standard Gibbs enegry change for the combustion of alpha-D glucose at 300K . C_(6)H_(12)O_(6)(s) +6O_(2)(g) rarr 6CO_(2)(g) +6H_(2)O(l) Given the standard enthalpies of formation (kJ mol^(-1)) C_(6)H_(12)O_(6) =- 1274.5, CO_(2) =- 393.5, H_(2)O =- 285.8 . Entropies (J K mol^(-1)) C_(6)H_(12)O_(6) = 212.1, O_(1) = 205.0, CO_(2) =213, H_(2)O = 69.9

    Calculate the Delta_(r)G^(@) for the reaction: C_(6)H_(12)O_(6)(s) + 6O_(2)(g) to 6CO_(2)(g) + 6H_(2)O(l) Delta_(f)G^(@) values (kJ mol^(-1) ) are : C_(12)H_(12)O_(6)(s) = -910.2, CO_(2)(g) = -394.4, H_(2)O(l) = -237.2

    Heat of reaction for C_(6)H_(12)O_(6(s))+6O_(2(g)) rarr 6CO_(2(g))+6H_(2)O_(v) at constant pressure is -651 kcal at 17^(@)C . Calculate the heat of reaction at constant volume at 17^(@)C .

    Heat of reaction for C_(6)H_(12)O_(6)(s) + 6O_(2)(g) to 6CO_(2)(g) + 6H_(2)O(v) at constant pressure is -651 kcal at 17^(@) C. Calculate the heat of reaction at constant volume at 17^(@) C.

    Consider the reaction, C_(6)H_(12)O_(6)(g)+6O_(2)(g) to 6CO_(2)(g) +6H_(2)O(l) , which of the following expressions is /are correct?

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