An average person needs abut 10000 KJ energy per day. The amount of glucose (molar mass $=180.0\mathrm{~g}\mathrm{~mol}^{-1}$) needed to meet this energy requirement is ____ g, (Nearest integer) (Use: $\Delta_{\mathrm{c}}\mathrm{H}$ (glucose) $=-2700\mathrm{~kJ}\mathrm{~mol}^{-1}$)

JEE Main · 2021 · 20 Jul 2021 · Shift 1 · Chemical Thermodynamics

An average person needs abut 10000 KJ energy per day. The amount of glucose (molar mass

= 180.0 g mol^{- 1}

) needed to meet this energy requirement is ____ g,
(Nearest integer)
(Use:

Δ_{c} H

(glucose)

= - 2700 kJ mol^{- 1}

)

Answer: 667

Complete combustion of one mole of glucose releases

2700 kJ

, so the number of moles that supplies

10000 kJ

n = \frac{10000}{2700} = 3.704 mol

Multiplying by the molar mass gives the mass required,

m = 3.704 \times 180.0 = 666.7 g

To the nearest integer the glucose needed is

667 g

JEE Main · 2021 · 20 Jul 2021 · Shift 1 · Integer answer