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olga_2 [115]
3 years ago
10

Highlight the claim.

Chemistry
1 answer:
Dahasolnce [82]3 years ago
8 0

Answer:

The claim is: Therefore Mitosis requires less energy than sexual reproduction does.

Explanation:

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In which of the following compounds is the mass ratio of chromium to oxygen closest to 1.62 to 1.00?
ohaa [14]

Answer:

The answer to your question is letter A

Explanation:

Data

Mass ratio 1.62 to 1.00

Atomic mass Cr = 52 g

Atomic mass O  = 16

Process

1.- Calculate the proportion Chromium to Oxygen to each possible solutions

a) CrO₃   =   \frac{52}{16 x 3} = \frac{52}{48} = 1.08

b) CrO₂   =   \frac{52}{16 x 2} = \frac{52}{32} = 1.63

c) CrO     = \frac{52}{16} = 3.25

d) Cr₂O   =  \frac{52 x 2}{16} = \frac{104}{16} = 6.5  

8 0
3 years ago
When backpacking in the wilderness, hikers often boil water to sterilize it for drinking. Suppose that you are planning a backpa
Pavlova-9 [17]

Answer:

2.104 L fuel

Explanation:

Given that:

Volume of water = 35 L = 35 × 10³ mL

initial temperature of water = 25.0 ° C

The amount of heat needed to boil water at this temperature can be calculated by using the formula:

q_{boiling} = mc \Delta T

where

specific heat   of water c= 4.18 J/g° C

q_{boiling} = 35 \times 10^{3} \times \dfrac{1.00 \ g}{1 \ mL} \times 4.18  \ J/g^0 C \times (100 - 25)^0 C

q_{boiling} = 10.9725 \times 10^6 \ J

Also; Assume that the fuel has an average formula of C7 H16 and 15% of the heat generated from combustion goes to heat the water;

thus the heat of combustion can be determined via the expression

q_{combustion} =-  \dfrac{q_{boiling}}{0.15}

q_{combustion} =-  \dfrac{10.9725 \times 10^6 J}{0.15}

q_{combustion} = -7.315 \times 10^{7} \ J

q_{combustion} = -7.315 \times 10^{4} \ kJ

For heptane; the equation for its combustion reaction can be written as:

C_7H_{16} + 11O_{2(g)} -----> 7CO_{2(g)}+ 8H_2O_{(g)}

The standard enthalpies of the  products and the reactants are:

\Delta H _f   \ CO_{2(g)} = -393.5 kJ/mol

\Delta H _f   \ H_2O_{(g)} = -242 kJ/mol

\Delta H _f   \ C_7H_{16 }_{(g)} = -224.4 kJ/mol

\Delta H _f   \ O_{2{(g)}} = 0 kJ/mol

Therefore; the standard enthalpy for this combustion reaction is:

\Delta H ^0= \sum n_p\Delta H^0_{f(products)}- \sum n_r\Delta H^0_{f(reactants)}

\Delta H^0 =( 7  \ mol ( -393.5 \ kJ/mol)  + 8 \ mol (-242 \ kJ/mol) -1 \ mol( -224.4 \ kJ/mol) - 11  \ mol  (0 \ kJ/mol))

\Delta H^0 = (-2754.5 \ \  kJ -  1936 \ \  kJ+224.4 \  \ kJ+0 \ \  kJ)

\Delta H^0 = -4466.1 \ kJ

This simply implies that the amount of heat released from 1 mol of C7H16 = 4466.1 kJ

However the number of moles of fuel required to burn 7.315 \times 10^{4} \ kJ heat released is:

n_{fuel} = \dfrac{q}{\Delta \ H^0}

n_{fuel} = \dfrac{-7.315 \times 10^{4} \ kJ}{-4466.1  \ kJ}

n_{fuel} = 16.38  \ mol \ of \ C_7 H_{16

Since number of moles = mass/molar mass

The  mass of the fuel is:

m_{fuel } = 16.38 mol \times 100.198 \ g/mol}

m_{fuel } = 1.641 \times 10^{3} \ g

Given that the density of the fuel is = 0.78 g/mL

and we know that :

density = mass/volume

therefore making volume the subject of the formula in order to determine the volume of the fuel ; we have

volume of the fuel = mass of the fuel / density of the fuel

volume of the fuel = \dfrac{1.641 \times 10^3 \ g }{0.78  g/mL} \times \dfrac{L}{10^3 \ mL}

volume of the fuel  = 2.104 L fuel

3 0
3 years ago
2 C4H10 + 13 O2--> 8 CO2 + 10 H2O
AleksAgata [21]

Answer:

4.14 x 10²⁴ molecules CO₂

Explanation:

2 C₄H₁₀ + 13 O₂ --> 8 CO₂ + 10 H₂O

To find the number of CO₂ molecules, you need to start with 100 grams of butane (C₄H₁₀), convert to moles (using the molar mass), convert to moles of CO₂ (using coefficients from equation), then convert to molecules (using Avagadro's number). The molar mass of C₄H₁₀ is calculated using the quantity of each element (subscript) multiplied by the number on the periodic table. The ratios should be arranged in a way that allows for units to be cancelled.

4(12.011g/mol) + 10(1.008 g/mol) = 58.124 g/mol C₄H₁₀

100 grams C₄H₁₀          1 mol C₄H₁₀             8 mol CO₂          
--------------------------  x  ----------------------  x  ---------------------  
                                        58.124 g              2 mol C₄H₁₀          

    6.022 x 10²³ molecules
x  ------------------------------------  =  4.14 x 10²⁴ molecules CO₂
              1 mol CO₂

7 0
2 years ago
Which greenhouse gas typically exists in both the stratosphere and the troposphere?
Arturiano [62]
The answer should be ozone
5 0
3 years ago
Read 2 more answers
After being thoroughly stirred at 10.°C, which mixture is heterogenous?(1) 25.0 g of KCl and 100. g of H2O
zheka24 [161]
The answer is (2) KNO3. This depends on the solubility of these four compounds at 10℃. For NaCl, it is 35.8 g, For NaNO3, 80.8 g. KCl, 31.2 g. KNO3, 21.9g. So only KNO3 is less than 25.0 g.
5 0
3 years ago
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