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nika2105 [10]
1 year ago
12

Consider this reaction: 6 CO2 + 6 H2O + light equation C6H12O6 + 6 O2 If there were 2.38 x 102 g of H2O, 18.6 moles of CO2, and

plenty of light, which reactant would be the limiting reactant?
Chemistry
1 answer:
alisha [4.7K]1 year ago
7 0

H₂O would be the limiting reactant.

Balanced chemical equation:

6CO₂ + 6H₂O + light equation → C₆H₁₂O₆ + 6O₂

The amount of product that can be created is constrained by the reactant that is consumed first in a chemical reaction, commonly referred to as the limiting reactant (or limiting reagent).

Given

No. of moles of CO₂ = 18.6

Mass of H₂O = 2.38 × 10² g = 238g

No. of moles of H₂O = Given mass/ Molar mass

                                = 238 / 18 = 13.22 moles

Moles of H₂O = 13.22

According to the balanced chemical equation

6 moles of CO₂ react with 6 moles of H₂O

So the reactant that has less number of moles will be consumed first.

As the No. of moles of H₂O < No. of moles of CO₂

So, H₂O is the limiting reactant with 13.22 moles.

Hence, H₂O would be the limiting reactant.

Learn more about limiting reactant here brainly.com/question/14222359

#SPJ1

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Answer:

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Explanation:

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After you convert the volume from mL to L and the temperature from Celsius to Kelvin, you can use the equation to find the moles.

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The molar mass represents the mass (g) of the gas per every 1 mole. Since you have been given a mass and mole value, you can set up a proportion to determine the molar mass.

\frac{?grams}{1 mole} =\frac{0.896grams}{0.0104moles}                                      <----- Proportion

?grams(0.0104moles) = 0.896                       <----- Cross-multiply

?grams = 86.2                                               <----- Divide both sides by 0.0104

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