The chemical reaction of hydrogen with oxygen produces water. 2 H 2 (g) + O 2 (g) → 2 H 2 O(g) c. How many moles of H 2 O form when 2.5 moles of O 2 reacts?

Hey, everyone, we're told that nitrogen combines with oxygen to yield nitric oxide. And they provided us the balanced chemical equation where we have N two plus 02 gets us to two of nitric oxide. We're asked to determine the number of moles of nitric oxide produced when 3.75 moles of nitrogen reacts with excess oxygen. First, let's go ahead and write out our pathway here for our dimensional analysis. So we were given mole of nitrogen and we're being asked to convert this to mole of nitric oxide in order to do. So, we're going to take a look at our multi mole ratios Starting off with 3.75 moles of nitrogen. We're going to look at our balanced chemical equation and we can see that one mole of nitrogen Is equivalent to two mole of nitric oxide due to that coefficient of two prior to our nitric oxide. Now, when we calculate this out and cancel out all of our units, we end up with a total of 7.50 mole of nitric oxide, which is going to be our final answer. Now, I hope this made sense and let us know if you have any questions.

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6. Chemical Reactions & Quantities

Stoichiometry

GOB Chemistry

6. Chemical Reactions & Quantities

Stoichiometry

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1:25 minutes

Problem 55c

Textbook Question

The chemical reaction of hydrogen with oxygen produces water.
2 H₂(g) + O₂(g) → 2 H₂O(g)
c. How many moles of H₂O form when 2.5 moles of O₂ reacts?

Verified step by step guidance

Identify the balanced chemical equation: 2H₂(g) + O₂(g) → 2H₂O(g). This equation shows the stoichiometric relationship between the reactants and products.

Determine the mole ratio between O₂ and H₂O from the balanced equation. For every 1 mole of O₂, 2 moles of H₂O are produced. This can be written as a ratio: \( \frac{2 \text{ moles of H₂O}}{1 \text{ mole of O₂}} \).

Start with the given amount of O₂, which is 2.5 moles. Use the mole ratio to convert moles of O₂ to moles of H₂O.

Set up the conversion: \( 2.5 \text{ moles of O₂} \times \frac{2 \text{ moles of H₂O}}{1 \text{ mole of O₂}} \).

Perform the multiplication to find the number of moles of H₂O formed. This will give you the final answer in moles of H₂O.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate how much of each substance is involved in the reaction based on the balanced chemical equation. In this case, it helps determine the amount of water produced from a given amount of oxygen.

Mole Ratio

The mole ratio is derived from the coefficients of a balanced chemical equation and indicates the proportion of moles of one substance to another. In the reaction 2H₂ + O₂ → 2H₂O, the mole ratio between O₂ and H₂O is 1:2. This means that for every mole of O₂ consumed, two moles of H₂O are produced, which is essential for calculating the amount of water formed.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. In this scenario, understanding which reactant limits the formation of water is crucial for accurately calculating the moles of H₂O produced when 2.5 moles of O₂ reacts.

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Textbook Question

The following diagram represents the reaction of A₂(red spheres) with B₂(blue spheres):

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b. How many moles of product can be made from 1.0 mol of A₂? From 1.0 mol of B₂?

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Textbook Question

Titanium metal is obtained from the mineral rutile, TiO2. The process requires multiple steps, as shown in the following reactions:

TiO₂(s) + 2 Cl₂(g) + 2 C(s) → TiCl₄(s) + 2 CO(g)

TiCl₄(s) + 2 Mg(s) → Ti(s) + 2 MgCl₂(s)

a. Write mole ratios to show the relationship between the reactants and products for each reaction.

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Textbook Question

Titanium metal is obtained from the mineral rutile, TiO2. The process requires multiple steps, as shown in the following reactions:

TiO₂(s) + 2 Cl₂(g) + 2 C(s) → TiCl₄(s) + 2 CO(g)

TiCl₄(s) + 2 Mg(s) → Ti(s) + 2 MgCl₂(s)

c. How many kilograms of rutile are needed to produce 95 kg of Ti?

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Textbook Question

Titanium metal is obtained from the mineral rutile, TiO2. The process requires multiple steps, as shown in the following reactions:

TiO₂(s) + 2 Cl₂(g) + 2 C(s) → TiCl₄(s) + 2 CO(g)

TiCl₄(s) + 2 Mg(s) → Ti(s) + 2 MgCl₂(s)

b. How many moles of TiO2 are needed to form one mole of titanium?

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Textbook Question

When table sugar (sucrose, C₁₂H₂₂O₁₁) is heated, it decomposes to form C and H₂O.

b. How many grams of carbon are formed by the breakdown of 60.0 g of sucrose?

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Textbook Question

Although Cu is not sufficiently active to react with acids, it can be dissolved by concentrated nitric acid, which functions as an oxidizing agent according to the following equation:

Cu(s) + 4 HNO₃(aq) → Cu(NO₃)₂(aq) + 2 NO₂(g) + 2 H₂O(l)

b. Is 35.0 g of HNO3 sufficient to dissolve 5.00 g of copper?

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Textbook Question

Ethyl alcohol is formed by enzyme action on sugars and starches during fermentation.

C₆H₁₂O₆ → 2 CO₂ + 2 C₂H₆O

If the density of ethyl alcohol is 0.789 g/mL, how many quarts can be produced by the fermentation of 100.0 lb of sugar?