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n200080 [17]
3 years ago
15

Assuming that the F−18 can be transported at 59.0 miles/hour, how close must the hospital be to the cyclotron if 68% of the F−18

produced is to make it to the hospital?
Chemistry
1 answer:
tekilochka [14]3 years ago
6 0

Answer:

60.12 miles

Explanation:

Using the calculation formula shown below:

t_{1/2} =\frac{t}{[tex]log_{2}\frac{N_{o} }{N_{t} } }[/tex]

where:

t_{1/2} is the half life, N_{o} is the original amount of F-18, and N_{t} is the remaining amount of F-18 at time t.

Generally, F-18 has an half life of 1.83 hours.

Therefore:

t = 1.83*[tex]log_{2}\frac{100}{68} = 1.02 hours[/tex]

Therefore using a speed of 59 miles/hour, the closeness of the hospital is:

distance = speed*time = 59*1.02 = 60.12 miles

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­­2K + 2HBr → 2 KBr + H2
Inessa [10]

Answer:

\large \boxed{\text{0.0503 g}}

Explanation:

The limiting reactant is the reactant that gives the smaller amount of product.

Assemble all the data in one place, with molar masses above the formulas and masses below them.

M_r:   39.10    80.41                2.016  

            2K  +  2HBr ⟶ 2KBr + H₂

m/g:     5.5      4.04

a) Limiting reactant

(i) Calculate the moles of each reactant  

\text{Moles of K} = \text{5.5 g} \times \dfrac{\text{1 mol}}{\text{31.10 g}} = \text{0.141 mol K}\\\\\text{Moles of HBr} = \text{4.04 g} \times \dfrac{\text{1 mol}}{\text{80.91 g}} = \text{0.049 93 mol HBr}

(ii) Calculate the moles of H₂ we can obtain from each reactant.

From K:  

The molar ratio of H₂:K is 1:2.

\text{Moles of H}_{2} = \text{0.141 mol K} \times \dfrac{\text{1 mol H}_{2}}{\text{1 mol K}} = \text{0.0703 mol H}_{2}

From HBr:  

The molar ratio of H₂:HBr is 3:2.  

\text{Moles of H}_{2} = \text{0.049.93 mol HBr } \times \dfrac{\text{1 mol H}_{2}}{\text{1 mol HBr}} = \text{0.024 97 mol H}_{2}

(iii) Identify the limiting reactant

HBr is the limiting reactant because it gives the smaller amount of NH₃.

b) Excess reactant

The excess reactant is K.

c) Mass of H₂

\text{Mass of H}_{2} = \text{0.024 97 mol H}_{2} \times \dfrac{\text{2.016 g H}_{2}}{\text{1 mol H}_{2}} = \textbf{0.0503 g H}_{2}\\ \text{The mass of hydrogen is $\large \boxed{\textbf{0.0503 g}}$ }

3 0
3 years ago
What is the numerical value of the equilibrium constant Kc?
Nezavi [6.7K]

ANSWER

EXPLANATION

Given that;

The number of moles of NH3 is 3 moles

The number of moles of H2 is 1 mole

The number of moles of N2 is 2 moles

At equilibrium, the concentration of ammonia is 1.4 moles/L

To find the value of Kc, follow the steps below

Step 1: Write the balanced equation of the reaction

\text{ N}_{2(g)}\text{ + 3H}_{2(g)}\text{ }\rightleftarrows\text{ 2NH}_{3(g)}

Step 2: Write the equation of the reaction in terms of Kc

\text{ K}_C\text{ = }\frac{[\text{ NH}_3]^2}{[N_2]\text{ \lbrack H}_2]^3}

Step 3: Find the concentration of each reactant at equilibrium using a stoichiometry ratio

From the reaction above, you will see that 1 mole of Nitrogen reacts with 3 moles of hydrogen to give 2 moles of ammonia.

Let x represents the concentration of nitrogen at equilibrium

Recall, that the concentration of ammonia at equilibrium is 1.4 moles/L

\begin{gathered} \text{ 2 mole NH}_3\text{ }\rightarrow\text{ 1 mole N}_2 \\ \text{ 1.04 mole/L NH}_3\text{ }\rightarrow\text{ x moles/L N}_2 \\ \text{ cross multiply} \\ \text{ 2 moles NH}_3\times\text{ x moles/L N}_2\text{ = 1 mole N}_2\times1.4\text{ mol/L} \\ \text{ Isolate x} \\ \text{ x mol/L N}_2\text{ = }\frac{1\text{ moles N}_2\times1.41\cancel{\frac{mol}{L}}}{2\cancel{moles}} \\ \text{ x mol/L = }\frac{1.04}{2} \\ \text{ x= 0.52 mole/L} \end{gathered}

Since the initial number of moles of nitrogen is 1 mole, hence, the concentration of nitrogen at equilibrium is calculated below as

Concentration at equilibrium = 1 -0.52

Concentration of nitrogen at equilibrium = 0.48 mole/L

The next step is to find the concentration of hydrogen at equilibrium

Let y represent the mole of hydrogen at equilibrium

\begin{gathered} \text{ 2 moles NH}_3\rightarrow\text{ 3 moles H}_2 \\ \text{ 1.04 moles/L NH}_3\text{ }\rightarrow\text{ y moles/L H}_2 \\ \text{ cross multiply} \\ \text{ 2 moles NH}_3\times\text{ y moles/L H}_2\text{ = 1.04 moles/L NH}_3\times3\text{ moles H}_2 \\ \text{  Isolate y} \\ \text{ y moles/L H}_2\text{ = }\frac{1.04\cancel{\frac{moles}{L}}NH_3\times3mole\text{ H}_2}{2\cancel{molsNH_3}} \\ y\text{ = }\frac{1.40\times3}{2} \\ \text{ y = }\frac{3.12}{2} \\ \text{ y = 1.56 moles} \end{gathered}

Since the initial concentration of hydrogen is 2 moles, hence the concentration of hydrogen at equilibrium can be calculated below as

Concentration at equilibrium = 2 - 1.56

Concentration at equilibrium = 0.44 mole/L

Step 4: Find the value of Kc using the equation in step 2

\text{ Kc = }\frac{[NH_3]^2}{[N_2]\text{ \lbrack H}_2]^3}\begin{gathered} \text{ Kc = }\frac{1.04^2}{0.48\times0.44^3} \\  \\ \text{ K}_c=\text{ }\frac{1.0816}{0.48\times\text{ 0.085184}} \\  \\ \text{ kc = }\frac{1.0816}{0.0408832} \\ \text{ kc = 26.4558547276} \end{gathered}

Hence, the value of Kc is 26

6 0
1 year ago
Adenosine triphosphate (ATP) is the main energy currency used in cells. ATP hydrolysis is coupled with unfavorable reactions, ma
kotegsom [21]

Answer:

<em>Thioesters- the Sulfur-Carbon bond is hydrolyzed, e.g. AcetylCoA</em>

<em>Reduced cofactor- These compounds accept electrons during the oxidation of substrates and energy is released when they are oxidized, e.g. Ubiquinol</em>

<em>Phosphorylated compounds- These compounds yield H₂P0₄⁻ upon hydrolysis, e.g. Phosphocreatine</em>

Explanation:

<em>Thioesters</em><em> are esters in which the linking oxygen atom is replaced by a sulphur atom. </em>They are the product of esterification between a carboxylic acid and a sulfhydryl group (thiol). They have the functional group R–S–CO–R'. Thioesters are common intermediates in many biosynthetic reactions. Examples include malonyl-CoA, acetyl-CoA, and propionyl-CoA. <em>In the hydrolysis of thioesters, the sulfur-carbon bond is hydrolyzed.</em>

<em>Cofactors</em><em> can be either organic or inorganic molecules that are required by enzymes to function. Cofactors can be oxidized or reduced for the enzymes to catalyze the reactions.</em>  Examples include, NAD, FAD, NADP, <em>Coenzyme Q₁₀.</em> Coenzyme Q₁₀ exists in three redox states, fully oxidized, partially reduced, and fully reduced. Ubiquinol is the reduced (electron-rich) form of coenzyme Q₁₀. Coenzyme Q₁₀ is vital for proper transfer of electrons within the mitochondrial oxidative respiratory chain, whose main function is to produce adenosine triphosphate (ATP). <em>These compounds accept electrons during the oxidation of substrates and energy is released when they are oxidized. </em>

Phosphorylated compounds are compounds with a phosphoryl group (PO₃²⁻) attached to its molecules. <em>These compounds yield an inorganic phosphate (H₂P0₄⁻) upon hydrolysis</em>. Phosphorylation is especially important for protein function as this modification activates or deactivates almost half of the enzymes, thereby regulating their function. Examples include, glucose-1-phosphate, phosphoserine, phosphocreatine, etc.

4 0
3 years ago
Calculate the mass of a liquid with a density of 3.2 g/ml and a volume of 25 ml
erma4kov [3.2K]
The equation is x/25=3.2
                         *25    *25
                         -------------
                          x=80g
4 0
3 years ago
How does the labrador current affect the climate of canada and greenland
max2010maxim [7]
The Labrador current affects the climate of Canada and Greenland because it creates one of the densest concentrations of fog in the world occurs.
3 0
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