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TEA [102]
3 years ago
6

Chicago uses 1.2x10^9 gallons of water/day.How many gallons per second must be pumped from the adjacent Lake Michigan every seco

nd to supply the city?
Chemistry
2 answers:
Rzqust [24]3 years ago
8 0

13888.8888889 i think?

ira [324]3 years ago
7 0

Answer:

13,888.88 gallons per second must be pumped from the adjacent Lake Michigan every second to supply the city.

Explanation:

Gallons of water used by Chicago city in 1 day = 1.2\times 10^9 gal

1 day = 24 hours

1 hour = 60 mins

1 min = 60 seconds

1 day=24\times 60\times 60 min = 86,400 seconds

Gallons of water used by Chicago city in 86,400 seconds :

= 1.2\times 10^9 gal

Gallons of water used by Chicago city in 1 second:

\frac{1.2\times 10^9 gal}{86,400}=13,888.88 gal

13,888.88 gallons per second must be pumped from the adjacent Lake Michigan every second to supply the city.

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Water molecules form hydrogen bonds to help in the process of water transport. Which property of water is described?
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7 0
3 years ago
Find the standard enthalpy of formation of ethylene, C2H4(g), given the following data: C2H4(g) + 3 O2(g) --&gt; 2CO2(g) + 2 H2O
Brums [2.3K]

Answer : The standard enthalpy of formation of ethylene is, 52.4 kJ

Explanation :

According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.

The formation reaction of C_2H_4 will be,

2C(s)+2H_2(g)\rightarrow C_2H_4(g)    \Delta H_{formation}=?

The intermediate balanced chemical reaction will be,

(1) C_2H_4(g)+3O_2(g)\rightarrow 2CO_2(g)+2H_2O(l)     \Delta H_1=-1411kJ

(2) C(s)+O_2(g)\rightarrow CO_2(g)    \Delta H_2=-393.5kJ

(3) H_2(g)+\frac{1}{2}O_2(g)\rightarrow H_2O(l)    \Delta H_3=-285.8kJ

Now we will reverse the reaction 1, multiply reaction 2 and 3 by 2 then adding all the equation, we get :

(1) 2CO_2(g)+2H_2O(l)\rightarrow C_2H_4(g)+3O_2(g)     \Delta H_1=+1411kJ

(2) 2C(s)+2O_2(g)\rightarrow 2CO_2(g)    \Delta H_2=2\times (-393.5kJ)=-787kJ

(3) 2H_2(g)+2O_2(g)\rightarrow 2H_2O(l)    \Delta H_3=2\times (-285.8kJ)=-571.6kJ

The expression for enthalpy of formation of C_2H_4 will be,

\Delta H_{formation}=\Delta H_1+\Delta H_2+\Delta H_3

\Delta H=(+1411kJ)+(-787kJ)+(-571.6kJ)

\Delta H=52.4kJ

Therefore, the standard enthalpy of formation of ethylene is, 52.4 kJ

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3 years ago
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3 years ago
Identify the type of reaction in the chemical reaction below:
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Complete question is;

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