Answer:
The correct answer is 0.36 mol
Explanation:
First we have to calculate the molecular weight (Mw) of H₃BO₃ from the molar masses of the elements:
Mw(H₃BO₃)= 3 x Molar mass H + Molar mass B + (3 x Molar mass O)
= 3 x 1 g/mol + 10.8 g/mol + (3 x 16 g/mol)
= 61.8 g/mol
The molecular weight indicates that there are 61.6 grams per mol of substance. The scientist has 22.5 g, thus we can calculate the number of moles of H₃BO₃ by dividing the mass into the molecular weight as follows:
Number of moles of H₃BO₃ = mass/Mw= (22.5 g)/(61.8 g/mol) = 0.36 mol
There are 0.36 mol of H₃BO₃ in 750.0 mL of solution.
Answer:
Grade A is the best percentage that is developing, proficient, exceeding, and emerging
Answer:
(E) changing temperature
Explanation:
Consider the following reversible balanced reaction:
aA+bB⇋cC+dD
If we know the molar concentrations of each of the reaction species, we can find the value of Kc using the relationship:
Kc = ([C]^c * [D]^d) / ([A]^a * [B]^b)
where:
[C] and [D] are the concentrations of the products in the equilibrium; [A] and [B] reagent concentrations in equilibrium; already; b; c and d are the stoichiometric coefficients of the balanced equation. Concentrations are commonly expressed in molarity, which has units of moles / 1
There are some important things to remember when calculating Kc:
- <em>Kc is a constant for a specific reaction at a specific temperature</em>. If you change the reaction temperature, then Kc also changes
- Pure solids and liquids, including solvents, are not considered for equilibrium expression.
- The reaction must be balanced with the written coefficients as the minimum possible integer value in order to obtain the correct value of Kc
Answer:
Explanation:
Hello there!
In this case, according to the given information, it will be possible for us to solve this problem by using the Boyle's law as an inversely proportional relationship between pressure and volume:
In such a way, we solve for the final volume, V2, and plug in the initial volume and pressure and final pressure to obtain:
Regards!
