NTSE Stage 2 SAT 2014 Question Paper

Question : 19 of 100

Marks: +1, -0

The reaction of burning carbon in oxygen is represented by the equation

\C_(\s)+\O_{2(\g)}→\C\O_{2(g)}+\Heat+\Light

When 9.0 g of solid carbon is burnt in 16.0 g of oxygen gas, 22.0 g of carbon dioxide is produced. The mass of carbon dioxide gas formed on burning of 3.0 g of carbon in 32.0 g of oxygen would be (Note: Atomic mass of C = 12.0 u, O = 16.0 u)

6.60 g
7.33 g
8.25 g
11.00 g

Validate

Solution:

Reaction of burning carbon in oxygen→

\C_(\s)+\O_{2(\g)}→\C\O_{2(g)}+\Heat+\Light

12gms 32gm → 44gm
Here , moles of carbon

=1/4

(atomic mass of C = 12)
And, moles of oxygen = 1
(atomic mass of O = 16)
When

1/4

mole of

\O_2

react with

1/4

mole of carbon, then

\C\O_2

mass will be
⇒

3+1/4×32=11\gms

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