if I have 25 mL of gas at a pressure of 2.1 atm and a temperature of 300 K, what will the pressure be if I increase the temperat
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The balanced molecular equation for the given reaction is:
To check that the equation is balanced count how many atoms are present for each element in the reactant and product side. If they are the same before and after reaction for all elements, then the reaction is deemed balanced.
The atom counting for the equation is shown below:
<u>Reactants </u> → <u>Products</u>
C: (2 x 2) =4 C: (2 x 2) = 4
H: (2 x 4) + (1 x 2) =10 H: (3 x 2) + (2 X 2) = 10
O: (2 x 2) + (1 x 2) = 6 O: (2 x 2) + (2 x 1) = 6
Ba: 1 Ba: 1
Since the number of atoms of each element are similar in the reactants and products, the equation is balanced.
To determine the state of the substances, consider their solubility.
The reactants are both aqueous (aq) as indicated in the problem.
The first product, is aqueous (aq) because based on the solubility rule, it will dissolve in water. Acetates are generally soluble.
The other product is water which will be liquid (l) since it is the solvent used to dissolve the substances.
<h3>LEARN MORE</h3>- Solubility Rules brainly.com/question/12984314
- Net Ionic Equation brainly.com/question/12980075
Keywords: acid-base, neutralization, balancing equations, molecular equation
Answer:
Explanation:
Hello,
In this case, the first step is to compute the molar mass of carbon dioxide as shown below, considering it has one carbon atom and two oxygen atoms:
It is important to notice it is the mass in one mole of such compound. Afterwards, we need to use the Avogadro's number to compute the how many moles are in the given molecules of carbon dioxide as shown below:
Finally, the mass by using the molar mass:
Best regards.
Answer:
1.373 mol H₂O
General Formulas and Concepts:
<u>Chemistry - Atomic Structure</u>
- Reading a Periodic Table
- Using Dimensional Analysis
Explanation:
<u>Step 1: Define</u>
24.75 g H₂O
<u>Step 2: Identify 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 /> = 1.37347 mol H₂O
<u>Step 4: Check</u>
<em>We are given 4 sig figs. Follow sig fig rules and round.</em>
1.37347 mol H₂O ≈ 1.373 mol H₂O