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4. What mass of oxygen is consumed when 61.0 g of water is produced in the following equation? $2H_2 + O_2 \rightarrow 2H_2O$ 5. What mass of $H_2O$ is produced when 28.5 g of HCl react completely in the following equation? $6HCl + Fe_2O_3 \rightarrow 2FeCl_3 + 3H_2O$ 

          4. What mass of oxygen is consumed when 61.0 g of water is produced in the following equation?
$2H_2 + O_2 \rightarrow 2H_2O$

5. What mass of $H_2O$ is produced when 28.5 g of HCl react completely in the following equation?
$6HCl + Fe_2O_3 \rightarrow 2FeCl_3 + 3H_2O$
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4. What mass of oxygen is consumed when 61.0 g of water is produced in the following equation? 2H2 + O2 → 2H2O 5. What mass of H2O is produced when 28.5 g of HCl react completely in the following equation? 6HCl + Fe2O3 → 2FeCl3 + 3H2O

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Chemistry: Structure and Properties
Chemistry: Structure and Properties
Nivaldo Tro 2nd Edition
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When mass conservation is considered, 61.0 g of water is produced in the following equation: 2H2 + O2 -> 2H2O. What mass of H2O is produced when 28.5 g of HCl reacts completely in the following equation: 6HCl + FeO2 -> 2FeCl3 + 3H2O.
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Transcript

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00:01 So, in this question we are given the reaction where hcl is reacting with ferric oxide to give ferric chloride and 3 moles of water.
00:16 We need to determine mass of water produced.
00:19 Firstly, we will determine number of moles for hcl by dividing its given mass with its molar mass.
00:25 On dividing 12 grams with 36 .46 grams per mole we get 0 .32913 moles...
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