The equation for the combustion of glucose is- C6H12O6s - 6O2g- 6CO2g - 6H2Og- How many grams of H2O will be produced when 8-064 g of glucose is burned-

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Stoichiometric Calculations

The equation ...

Question

The equation for the combustion of glucose is: $C_{6} H_{12} O_{6} (s) + 6 O_{2} (g) \to 6 {CO}_{2} (g) + 6 H_{2} O (g)$ . How many grams of $H_{2} O$ will be produced when $8.064 g$ of glucose is burned?

Open in App

Solution

Step 1: Combustion reaction :
It refers to an exothermic chemical reaction that has a high temperature.
It happens between a fuel and an oxidant.
A combustion reaction in a fire produces a flame, and the heat emitting can thus make it self-sustaining.
A combustion reaction is often a complicated sequence of elementary radical reactions.
Step 2: Given information:
The amount of glucose is $8.064 g$ .
The molar mass of glucose is $180.15588 g {mol}^{- 1}$ .
The molar mass of water is $18.01528 g {mol}^{- 1}$ .
Step 3: Balanced chemical equation:
The equation for the combustion of glucose is given as:
$C_{6} H_{12} O_{6} (s) + 6 O_{2} (g) \to 6 {CO}_{2} (g) + 6 H_{2} O (g)$
Step 4: Calculation of the amount of water:
The following conversion will take place;
$\Rightarrow 8.064 g of C_{6} H_{12} O_{6} \times \frac{1 mol of C_{6} H_{12} O_{6}}{180.15588 g {mol}^{- 1} of C_{6} H_{12} O_{6}} \times \frac{6 mol of H_{2} O}{1 mol of C_{6} H_{12} O_{6}} \times \frac{18.01528 g {mol}^{- 1} of H_{2} O}{1 mol of H_{2} O} On cancelling, the amount of water is : = 4.838 g of H_{2} O$
Thus, approximately $0.8 g$ water will produce.

Suggest Corrections

Similar questions

A person requires $10000 k J$ energy per day and $∆ H$ combustion of glucose is $2700 k J m o l^{- 1}$ . How many grams of glucose are required by the body in a day?

Q. How many grams of glucose be dissolved to make one-litre solution of 10% glucose?

Q. When 180 grams of glucose is subjected to combustion, the volume of

C O_{2}

liberated at STP is

Q. The combustion of a sample of butane C4H10 produced 2.46 grams of water? 2C4H10 + 13O2 ====== 8CO2 + 10H2O
A-How many moles of water formed?
B-How many moles of butane burned?
C-How many grams of butane burned?
D-How many oxygen was used up in moles? in grams?

Q. How many moles of glucose is present in

100

gram of glucose

(C_{6} H_{12} O_{6})

Join BYJU'S Learning Program

The equation for the combustion of glucose is: C6H12O6(s)+6O2(g)→6CO2(g)+6H2O(g). How many grams of H2O will be produced when 8.064g of glucose is burned?

The equation for the combustion of glucose is: $C_{6} H_{12} O_{6} (s) + 6 O_{2} (g) \to 6 {CO}_{2} (g) + 6 H_{2} O (g)$ . How many grams of $H_{2} O$ will be produced when $8.064 g$ of glucose is burned?