Chemistry: 2h2 +o2 → 2h2o what mass of water forms when 1.45 × 10-3 g o2 react completely? (molar mass of o2 = 32.00 g/mol; molar mass of h2o = 18.02 g/mol) 1.63 × 10-3 g 8.16 × 10-4 g 1.29 × 10-3 g

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2h2 +o2 → 2h2o what mass of water forms when 1.45

babbiegirl8035

11.03.2022

Answer : The correct option is, $1.63\times 10^{-3}g$

Explanation : Given,

Mass of oxygen gas = $1.45\times 10^{-3}g$

Molar mass of oxygen gas = 32 g/mole

Molar mass of water = 18.02 g/mole

First we have to calculate the moles of O_2 .

$\text{Moles of }O_2=\frac{\text{Mass of }O_2}{\text{Molar mass of }O_2}=\frac{1.45\times 10^{-3}g}{32g/mole}=4.53\times 10^{-5}moles$

Now we have to calculate the moles of H_2O .

The balanced chemical reaction is,

$2H_2+O_2\rightarrow 2H_2O$

From the balanced reaction we conclude that

As, 1 mole of O_2 react to give 2 mole of H_2O

So, $4.53\times 10^{-5}$ moles of O_2 react to give $4.53\times 10^{-5}\times 2=9.06\times 10^{-5}$ moles of H_2O

Now we have to calculate the mass of H_2O

$\text{Mass of }H_2O=\text{Moles of }H_2O\times \text{Molar mass of }H_2O$

$\text{Mass of }H_2O=(9.06\times 10^{-5}mole)\times (18.02g/mole)=1.63\times 10^{-3}g$

Therefore, the mass water produced is, $1.63\times 10^{-3}g$

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