Answer:
(a) 1:3
(b)
mmol of OH⁻ = 1.893 mmol
mmol of H₃C₆H₅O₇: 0.6310 mmol
mass of H₃C₆H₅O₇: 0.1212 g
mass % of H₃C₆H₅O₇ in orange juice: 1.37%
molarity of H₃C₆H₅O₇ in orange juice: 0.0726 M
Explanation:
Let's consider the following balanced chemical equation.
H₃C₆H₅O₇ + 3 OH⁻ → C₆H₅O₇³⁻ + 3 H₂O
<em>(a) What is the stoichiometry of H₃C₆H₅O₇ to OH⁻? </em>
The molar ratio of H₃C₆H₅O₇ to OH⁻ is 1:3
<em>(b)</em>
<em>mmol of OH⁻: ?</em>
<em>mmol of H₃C₆H₅O₇: ?</em>
<em>mass of H₃C₆H₅O₇: ?</em>
The molar mass of the citric acid is 192.1 g/mol.
<em>mass % of H₃C₆H₅O₇ in orange juice: ?</em>
<em>molarity of H₃C₆H₅O₇ in orange juice: ?</em>
Answer:
Explanation:
= Rydberg constant = 
= Initial shell = 3
= Final shell = 1
We have the relation
The energy of the photon emitted here is .
<span>(a) The balanced equation shows that 2 moles of water result from 5 moles of
oxygen that reacts, so that is 0.4 times as many moles of water as O2. So if we
have 2.50 moles of oxygen reacting, we produce 0.4 times that amount, or
1.0 mole of water.
(b) The molecular weight of acetylene is 26 and that of O2 is 32, so we can set
up the proportion: 2.25 gm. / 52 = x gm. / 160
Then x grams = (2.25)(160) / 52 = 6.923 grams of O2 are required.
(c) The balanced equation shows that twice as many moles of CO2 are produced
as we have acetylene reacting. If 78.0 grams of acetylene react, that is 3 moles
so we produce twice that, or 6 moles of CO2. The molecular weight of CO2 is 44,
so we have 44 times 6, or 264 grams of carbon dioxide produced.
(d) If we collect 186 grams of CO2, the percentage yield is:
186/264 = 0.7045, or 70.45 percent yield.
Whew! Hope this answers all parts of your question!</span><span>
</span>
The number of protons and neutrons in the nucleus : 92 and 146
<h3>Further explanation</h3>
Given
Mass number = 238
Atomic number = 92
Required
Protons and neutrons
Solution
Mass number=number of protons + neutrons
Atomic number=number of protons=number of electrons
Atomic number = 92⇒number of protons=92
Number of neutrons = mass number - atomic number
Number of neutrons = 238 - 92 = 146
Answer:
- 1273.02 kJ.
Explanation:
This problem can be solved using Hess's Law.
Hess's Law states that <em>regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes. This law is a manifestation that enthalpy is a state function.</em>
- We should modify the given 3 equations to obtain the proposed reaction:
<em>6C(s) + 6H₂(g) + 3O₂(g) → C₆H₁₂O₆(s),</em>
<em></em>
- We should multiply the first equation by (6) and also multiply its ΔH by (6):
6C(s) + 6O₂(g) → 6CO₂(g), ∆H₁ = (6)(–393.51 kJ) = - 2361.06 kJ,
- Also, we should multiply the second equation and its ΔH by (6):
6H₂(g) + 3O₂(g) → 6H₂O(l), ∆H₂ = (6)(–285.83 kJ) = - 1714.98 kJ.
- Finally, we should reverse the first equation and multiply its ΔH by (- 1):
6CO₂(g) + H₂O(l) → C₆H₁₂O₆(s) + 6O₂(g), ∆H₃ = (-1)(–2803.02 kJ) = 2803.02 kJ.
- By summing the three equations, we cam get the proposed reaction:
<em>6C(s) + 6H₂(g) + 3O₂(g) → C₆H₁₂O₆(s),</em>
<em></em>
- And to get the heat of reaction for the production of glucose, we can sum the values of the three ∆H:
<em>∆Hrxn = ∆H₁ + ∆H₂ + ∆H₃ =</em> (- 2361.06 kJ) + (- 1714.98 kJ) + (2803.02 kJ) = <em>- 1273.02 kJ.</em>
