Question

Which of the following statements is wrong about 4.4 g of Co2 

A) A = 0.1 mole of Co2 
B) A = 100 ml at STP
C) A occupies 6.023*10^-23 
D) 6 g C= 16 g of O2

Answer 1

B, C are incorrect. 

Let's see All options and determine whether which option is correct. 

A) We know that 

Gram molecular weight of Co2 =12+32 = 44g 

1 mole of Co2 ----> 44 g 

x moles ------> 4.4 g 

4.4 = 44x 

x = 44/440=1/10=0.1 moles. 

Hence, If A is 4.4 g of Co2, then A = 0.1 mole of Co2. 

Hence, Option A ✓. 

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B) We know that 1 mole of Co2 = 22,400 ml 

Here given 0.1 moles of Co2 [ as per calculations in Option A. 

so, 1 mole of Co2 = 22400 ml 

0.1 mole of Co2 = x ml 

x =0.1*22400 

x = 2240 ml. 

Hence, Option B is incorrect. 

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C) We know that 1 mole of Co2 = 6.023*10^23 particles. 

0.1 moles = 6.023*10^23/10 = 6.023*10^22 particles. 

Hence, A occupies 6.023 * 10^22 particles. 

Hence Option C is wrong. 

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D) In Co2

1 mole of C combines with 1 mole of Co2 

12 g of C combines with 32 g of Co2 

Given, Weight of C =6 g. 


6 g of C = x g of O2 

12x =32*6 

x =32*1/2 

x =16 g. 

Hence, 6 g of C combines with 16 g of O2. 

Option D is correct. 

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The wrong statements are Option B,C

Answer 2

hey,
i think option B is right
because in this qustion no condition was given.......