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

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