How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 30.6 moles of water vapor?
Express your answer with the appropriate units.
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How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 30.6 moles of water vapor? Express your answer with the appropriate units. View Available. Hint(s)

UpStudy AI · Accepted Answer

To solve this problem, we need to use the balanced chemical equation for the reaction between hydrogen gas (H2) and carbon dioxide (CO2) to produce water vapor (H2O).

The balanced chemical equation for this reaction is:
$$ 2H_2 + CO_2 \rightarrow 2H_2O $$

From the balanced chemical equation, we can see that 2 moles of hydrogen gas (H2) react with 1 mole of carbon dioxide (CO2) to produce 2 moles of water vapor (H2O).

Given that we need to produce 30.6 moles of water vapor, we can calculate the number of moles of hydrogen gas needed using the stoichiometry of the reaction.

Let's denote the number of moles of hydrogen gas needed as $$ x $$.

From the balanced chemical equation, we can set up the following proportion:
$$ \frac{2 \text{ moles of H}_2}{1 \text{ mole of CO}_2} = \frac{x \text{ moles of H}_2}{30.6 \text{ moles of H}_2O} $$

Solving for $$ x $$, we have:
$$ x = \frac{2 \times 30.6}{1} $$

Now, let's calculate the number of moles of hydrogen gas needed.
Calculate the value by following steps:
- step0: Calculate:
  $$2\times 30.6$$
- step1: Multiply the numbers:
  $$61.2$$
The number of moles of hydrogen gas needed to react with excess carbon dioxide to produce 30.6 moles of water vapor is 61.2 moles of hydrogen gas.
To produce 30.6 moles of water vapor, 61.2 moles of hydrogen gas are needed.

How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 30.6 moles of water vapor?
Express your answer with the appropriate units.
View Available. Hint(s)

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