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sergij07 [2.7K]

2 years ago

9

Please help I don’t know the answer

1 answer:

trapecia [35]2 years ago

4 0

Answer:

the answer is B, "summer, winter"

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What happens to the sugars that are made during photosynthesis?

KiRa [710]

The sugars (c6h12o6) or the glucose that is made during photosynthesis is turned into glucose cellulose or starch that the plant can use for energy and food for the plant. Hope this helps.

8 0

3 years ago

Why guys always coming at me for?

pav-90 [236]

You are beautiful just like me trust me i know<span />

5 0

2 years ago

C10H12O4S(s) + O2(g)  CO2(g) + SO2(g) + H2O(g)

ale4655 [162]

Answer: The coefficient for $O_2(g)$ is 12.

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

$C_{10}H_{12}O_4S(s)+12O_2(g)\rightarrow 10CO_2(g)+SO_2(g)+6H_2O$

Thus in the reactants, there are 12 molecules of oxygen in balanced chemical equation. Thus the coefficient for $O_2(g)$ is 12.

8 0

2 years ago

A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both sol

Reika [66]

Answer : The enthalpy change for the process is 52.5 kJ/mole.

Explanation :

Heat released by the reaction = Heat absorbed by the calorimeter + Heat absorbed by the solution

$q=[q_1+q_2]$

$q=[c_1\times \Delta T+m_2\times c_2\times \Delta T]$

where,

q = heat released by the reaction

$q_1$ = heat absorbed by the calorimeter

$q_2$ = heat absorbed by the solution

$c_1$ = specific heat of calorimeter = $12.1J/^oC$

$c_2$ = specific heat of water = $4.18J/g^oC$

$m_2$ = mass of water or solution = $Density\times Volume=1/mL\times 100.0mL=100.0g$

$\Delta T$ = change in temperature = $T_2-T_1=(26.3-20.2)^oC=6.1^oC$

Now put all the given values in the above formula, we get:

$q=[(12.1J/^oC\times 6.1^oC)+(100.0g\times 4.18J/g^oC\times 6.1^oC)]$

$q=2623.61J$

Now we have to calculate the enthalpy change for the process.

$\Delta H=\frac{q}{n}$

where,

$\Delta H$ = enthalpy change = ?

q = heat released = 2626.61 J

n = number of moles of copper sulfate used = $Concentration\times Volume=1M\times 0.050L=0.050mole$

$\Delta H=\frac{2623.61J}{0.050mole}=52472.2J/mole=52.5kJ/mole$

Therefore, the enthalpy change for the process is 52.5 kJ/mole.

8 0

3 years ago

5. Which material has the highest thermal conductivity? Which material has the highest electrical conductivity? Explain why ther

Afina-wow [57]

Answer:

Sliver

Explanation:

Silver has the highest electrical conductivity of all metals. :)

6 0

2 years ago