Answer:
0.19 mol H₂O
General Formulas and Concepts:
<u>Chem</u>
- Reading a Periodic Table
- Using Dimensional Analysis
Explanation:
<u>Step 1: Define</u>
Given: 3.5 g H₂O from RxN
<u>Step 2: Define conversions</u>
Molar Mass of H - 1.01 g/mol
Molar Mass of O - 16.00 g/mol
Molar Mass of H₂O - 2(1.01) + 16.00 = 18.02 g/mol
<u>Step 3: Convert</u>
<u /> = 0.194229 mol H₂O
<u>Step 4: Check</u>
<em>We are given 2 sig figs. Follow sig fig rules.</em>
0.194229 mol H₂O ≈ 0.19 mol H₂O
The position of equilibrium lies far to the right, with products being favoured. Hence, option A is correct.
<h3>What is equilibrium?</h3>
Chemical equilibrium is a condition in the course of a reversible chemical reaction in which no net change in the amounts of reactants and products occurs.
A very high value of K indicates that at equilibrium most of the reactants are converted into products.
The equilibrium constant K is the ratio of the concentrations of products to the concentrations of reactants raised to appropriate stoichiometric coefficients.
When the value of the equilibrium constant is very high, the concentration of products is much higher than the concentration of reactants.
This means that most of the reactants are converted into products and the position of equilibrium lies far to the right, with products being favoured.
Hence, option A is correct.
Learn more about the equilibrium here:
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Answer: Thus 24.0 g of would be needed.
Explanation:
To calculate the moles :
According to stoichiometry :
1 mole of require = 2 moles of
Thus 0.1875 moles of will require= of
Mass of
Thus 24.0 g of would be needed to completely react with 6.00 g of such that all reactants could be consumed.
The answer would be 6.022 × 10^18