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irinina [24]
2 years ago
8

A blank cell has half the chromosomes of a blank cell

Chemistry
1 answer:
Vladimir [108]2 years ago
6 0
The answer to this is Haploid and Meiosis. I think
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At 25∘C, the decomposition of dinitrogen pentoxide, N2O5(g), into NO2(g) and O2(g) follows first-order kinetics with k=3.4×10−5
Annette [7]

Answer:

4600s

Explanation:

2N_{2}O_{5}(g) - - -> 4NO_{2}(g) +O_{2}

For a first order reaction the rate of reaction just depends on the concentration of one specie [B] and it’s expressed as:

-\frac{d[B]}{dt}=k[B] - - -  -\frac{d[B]}{[B]}=k*dt

If we have an ideal gas in an isothermal (T=constant) and isocoric (v=constant) process.

PV=nRT we can say that P = n so we can express the reaction order as a function of the Partial pressure of one component.  

-\frac{d[P(B)]}{P(B)}=k*dt  

-\frac{d[P(N_{2}O_{5})]}{P(N_{2}O_{5})}=k*dt

Integrating we get:

\int\limits^p \,-\frac{d[P(N_{2}O_{5})]}{P(N_{2}O_{5})}=\int\limits^ t k*dt

-(ln[P(N_{2}O_{5})]-ln[P(N_{2}O_{5})_{o})])=k(t_{2}-t_{1})

Clearing for t2:

\frac{-(ln[P(N_{2}O_{5})]-ln[P(N_{2}O_{5})_{o})])}{k}+t_{1}=t_{2}

ln[P(N_{2}O_{5})]=ln(650)=6.4769

ln[P(N_{2}O_{5})_{o}]=ln(760)=6.6333

t_{2}=\frac{-(6.4769-6.6333)}{3.4*10^{-5}}+0= 4598.414s

4 0
2 years ago
How many grams of oxygen is needed to completely react with 9.30 moles of aluminum
Orlov [11]
Balanced chemical equation:

* moles of oxygen

4 Al + 3 O2 = 2 Al2O3

4 moles Al -------------- 3 moles O2
9.30 moles Al ---------- moles O2

moles O2 = 9.30 * 3 / 4

moles O2 = 27.9 / 4 => 6.975 moles of O2

Therefore:

Molar mass O2 = 31.9988 g/mol

n = m / mm

6.975 = m / 31.9988

m = 6.975 * 31.9988

m = 223.19 of O2


5 0
2 years ago
High concentrations of ammonia (NH3), nitrite ion, and nitrate ion in water can kill fish. Lethal concentrations of these specie
kykrilka [37]

Explanation:

It is known that molality is the number of moles present in kg of solution.

Mathematically,  Molality = \frac{\text{no. of moles of solute}}{\text{mass of solvent in Kg}}

The given data is as follows.

Molar mass of ammonia = 17 g/mol

Concentration = 1.002 mg/L = \frac{0.001002 g/L}{17 g/mol}

                        = 5.89 \times 10^{-4} mol/L

Also,    density = \frac{1 g}{mL} = 1 kg/L

Therefore, molality will be calculated as follows.

        Molality = \frac{5.89 \times 10^{-4} mol/L}{1 kg/L}

                      = 5.89 \times 10^{-4} mol/kg

And,

Molar mass of nitrite = 46 g/mol

Concentration = 0.387 mg/L = \frac{0.000412 g/L}{46 g/mol}

                        = 8.956 \times 10^{-6} mol/L

And, density = \frac{1 g}{mL} = 1 kg/L

Hence, molality = \frac{8.956 \times 10^{-6} mol/L}{1 kg/L}

                          = 8.956 \times 10^{-6} mol/kg  

Now, Molar mass of nitarte = 62 g/mol

      Concentration = 1352.2 mg/L

                              = \frac{1.3522 g/L}{62 g/mol}

                              = 0.02181 mol/L

Also, density = \frac{1 g}{mL} = 1 kg/L

Hence, molality will be calculated as follows.

         Molality = \frac{0.02181 mol/L}{1 kg/L}

                       = 0.02181 mol/kg

Therefore, molality of given species is 5.89 \times 10^{-4} mol/kg  for ammonia, 8.956 \times 10^{-6} mol/kg  for nitrite, and 0.02181 mol/kg for nitrate ion.

7 0
3 years ago
Balance equation P2O5 + H20 - - - - &gt; H3PO4<br> Help me.....
Archy [21]

Answer:

Search by reactants (P 2O 5, H 2O) and by products (H 3PO 4)

H2O + P2O5 → H3PO4

H2O + HNO3 + P2O5 → H3PO4 + N2O5

8 0
3 years ago
Two masses exerting a force on each other is an example of What????
trasher [3.6K]

Newtons universal law of gravitation

hope this helps

8 0
2 years ago
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