Advertisements
Advertisements
प्रश्न
Solve problem:
Arjun purchased 250 g of glucose (C6H12O6) for Rs 40. Find the cost of glucose per mole.
Advertisements
उत्तर
Given: Mass of glucose = 250 g, cost for 250 g glucose = Rs 40, molecular formula of glucose = C6H12O6
To find: Cost per mole of glucose
Calculation: Molecular formula of glucose is (C6H12O6).
Molecular mass of glucose
= (6 × Average atomic mass of C) + (12 × Average atomic mass of H) + (6 × Average atomic mass of O)
= (6 × 12 u) + (12 × 1 u) + (6 × 16 u)
= 180 u
∴ Molar mass of glucose = 180 g mol−1
Number of moles = `"Mass of a substance"/"Molar mass of a substance"`
= `(250 "g")/(180"g mol"^-1)`
= `250/180` mol
Now,
`250/180` mol of glucose cost = Rs 40
1 mol glucose cost = x
∴ x = `(40xx180)/250`
= Rs 28.8/mol of glucose
The cost of glucose per mole is Rs 28.8.
APPEARS IN
संबंधित प्रश्न
Choose the correct option.
Which of the following has maximum number of molecules?
Calculate the molecular mass of the following in u.
NH3
Calculate the molecular mass of the following in u.
C2H5OH
What is the ratio of molecules in 1 mole of NH3 and 1 mole of HNO3?
Solve problem:
Calculate the number of an atom of the following (Given: Atomic mass of I = 127 u).
254 g of iodine (I)
24 g of carbon reacts with some oxygen to make 88 grams of carbon dioxide. Find out how much oxygen must have been used.
Solve problem:
Calculate the number of atoms of the following. (Average atomic mass : N = 14 u, S = 32 u)
0.4 mole of nitrogen
Solve problem:
Calculate the number of atoms of the following. (Average atomic mass : N = 14 u, S = 32 u)
1.6 g of sulfur
Calculate the number of atoms of hydrogen present in 5.6 g of urea, \[\ce{(NH2)2CO}\]. Also calculate the number of atoms of N, C, and O.
Explain formula mass with an example.
Which one of the following represents 180 g of water?
What is the mass of precipitate formed when 50 ml of 8.5% solution of AgNO3 is mixed with 100 ml of 1.865% potassium chloride solution?
Which of the following is/are true with respect to carbon-12.
Which one of the following is used as a standard for atomic mass.
Define relative atomic mass.
Calculate the average atomic mass of naturally occurring magnesium using the following data.
| Isotope | Isotopic atomic mass | Abundance (%) |
| Mg24 | 23.99 | 78.99 |
| Mg25 | 24.99 | 10.00 |
| Mg26 | 25.98 | 11.01 |
An element has a bee structure with cell edge of 288 pm. The density of element is 7.2 g cm-3. What is the atomic mass of an element?
Boron has two isotopes 10B and 11B with atomic masses 10 and 11, respectively. If its average atomic mass is 10.81, the abundance of 10B is ____________.
What is the average mass of an element if it has two isotopes, one of mass 6.015 u with 8.24 % and other of mass 7.016 u with 91.26% respectively?
One amu is equal to ________.
Calculate mass of 3.01 × 1024 atoms of an element having atomic mass 21.13.
A 100 g of sample of haemoglobin on analysis was found to contain 0.34% Fe by mass. If each haemoglobin molecule has four Fe2+ ions, the molecular mass of haemoglobin is: (Fe = 56 amu)
Which symbol replaces the unit of atomic mass, amu?
0.05 F electricity is passed through CuSO4 solution. Calculate the mass of Cu produced at cathode? (molar mass of Cu = 63.5 g mol-1)
