How many grams of CO would be required to generate 635 g CO2
1 answer:
The amount of CO that would be required to generate 635 g of CO2 will be 404.14 g
<h3>Stoichiometric problem</h3>First, let us get the equation of the reaction:
From the equation, we can see that the mole ratio of CO to that of CO2 is 1:1.
635 g of CO2 is to be generated.
Mole of 635 g CO2 = mass/molar mass = 635/44.01 = 14.43 moles
Thus, the equivalent mole of CO required will also be 14.43 moles.
Mass of 14.43 moles CO = moles x molar mass = 14.43 x 28.01 = 404.14 g
Hence, 404.14 g of CO will be required to produce 635 g of CO2
More on stoichiometric problems can be found here: brainly.com/question/14465605
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Explanation:
Answer: 25.13 g of and 20.56 g of
will be produced from 45.70 g of
Explanation:
To calculate the moles :
The balanced chemical equation is:
According to stoichiometry :
1 mole of produce = 1 mole of
Thus 0.571 moles of will require=
of
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1 mole of produce = 2 moles of
Thus 0.571 moles of will require=
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Thus 25.13 g of and 20.56 g of
will be produced from 45.70 g of