Home
Class 12
CHEMISTRY
A flask contains 2.0xx10^(13) molecules ...

A flask contains `2.0xx10^(13)` molecules of `CO_(2)`. To this `1.5xx10^(14)` molecules of `CO_(2)` are added.
The number of molecules in the flask now is

A

`3.5xx10^(13)`

B

`3.5xx10^(14)`

C

`1.7xx10^(14)`

D

None of these

Text Solution

AI Generated Solution

The correct Answer is:
To find the total number of molecules of CO₂ in the flask after adding more molecules, we can follow these steps: ### Step 1: Identify the initial number of molecules The initial number of CO₂ molecules in the flask is given as: \[ 2.0 \times 10^{13} \text{ molecules} \] ### Step 2: Identify the number of molecules added The number of CO₂ molecules added to the flask is: \[ 1.5 \times 10^{14} \text{ molecules} \] ### Step 3: Convert both numbers to the same power of ten To add the two quantities, we need to express them with the same exponent. The smaller exponent is \(10^{13}\). We can rewrite \(1.5 \times 10^{14}\) as: \[ 1.5 \times 10^{14} = 15.0 \times 10^{13} \] ### Step 4: Add the two quantities Now we can add the two quantities: \[ 2.0 \times 10^{13} + 15.0 \times 10^{13} = (2.0 + 15.0) \times 10^{13} = 17.0 \times 10^{13} \] ### Step 5: Convert the result to standard scientific notation The result \(17.0 \times 10^{13}\) can be expressed in standard scientific notation as: \[ 1.7 \times 10^{14} \] ### Final Answer Thus, the total number of CO₂ molecules in the flask now is: \[ \boxed{1.7 \times 10^{14}} \] ---

To find the total number of molecules of CO₂ in the flask after adding more molecules, we can follow these steps: ### Step 1: Identify the initial number of molecules The initial number of CO₂ molecules in the flask is given as: \[ 2.0 \times 10^{13} \text{ molecules} \] ...
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • SOME BASIC CONCEPTS OF CHEMISTRY

    DINESH PUBLICATION|Exercise REASON ASSERTION TYPE MCQs|11 Videos
  • SOLUTIONS

    DINESH PUBLICATION|Exercise ULTIMATE PREPARATORY PACKAGE|10 Videos
  • SURFACE CHEMISTRY

    DINESH PUBLICATION|Exercise BRAIN STORMING MULTIPLE CHOICE QUESTIONS (MCQs)|8 Videos

Similar Questions

Explore conceptually related problems

Calculate number of molecules in 1 ml of Co_(2) at NTP.

A candle is burnt in a beaker until extinguishers itseft. A sample of gaseous mixutre in the beaker contains 6.08 xx 10^(20) molecules of O_(2) , and 0.50 xx 10^(20) molecules of CO_(2) . The total pressure is 734 mm of Hg . The partial pressure of O_(2) would be

Knowledge Check

  • The weight of 2.01xx10^(23) molecules of CO is-

    A
    `9.3 g`
    B
    `7.2g`
    C
    `1.2g`
    D
    `3g`
  • A candle is burnt in a beaker until it extinguishes itself. A sample of gaseous mixture in the beaker contains 6.08 xx 10^(20) molecules of N_(2), 0.76 xx 10^(20) molecules of O_(2) , and 0.50 xx 10^(20) molecules of CO_(2) . The total pressure is 734 mm of Hg. The partial pressure of O_(2) would be

    A
    760.0 mm of Hg
    B
    76.0 mm of Hg
    C
    7.6 mm of Hg
    D
    0.76 mm of Hg
  • A flask contains 3.0xx10^(16) atoms of He. From This 6.6xx10^(15) atoms of He are removed. The flask now contains atoms of He

    A
    `3.6xx10^(16)`
    B
    `2.3xx10^(16)`
    C
    `+3.6xx10^(15)`
    D
    None of these
  • Similar Questions

    Explore conceptually related problems

    10^(21) molecules are removed from 200 mg of CO_(2) . The moles of CO_(2) left are:

    x L of N_(2) at STP contains 3xx10^(22) molecules. The number of molecules in x//2 L of ozone at STP will be

    x L of N_2 at STP contains 3 xx 10^(22) molecules. The number of molecules in x/2 L of ozone at STP will be

    If 10^(21) molecules are removed from 100mg CO_(2) . Then number of moles of CO_(2) left are:

    In CO_(2) molecule,