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Lunna [17]
3 years ago
12

How many moles of oxygen are required to produce 37.15 g CO2?

Chemistry
2 answers:
denpristay [2]3 years ago
8 0
Carbon = 12.010. Oxygen = 15.999 x 2 15.999 x 2 = 31.998 + 12.010 = 44.008 \frac{37.15 grams * 1 mole CO2}{44.008 grams}
Nostrana [21]3 years ago
4 0
1.407.........................................................
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Example 1: urea, (nh2)2co, is used in the manufacture of resins and glues. when 5.00 g of urea is dissolved in 250.0 ml of water
katen-ka-za [31]
A) i believe the reaction is exothermic, because 27.6 kg of thermal energy is gained by the water solution, the dissolution of urea is exothermic. Exothermic reaction is a chemical reaction that releases energy by light or heat. It is the opposite of an endothermic reaction where heat is gained by the reaction.

b) The water gained the heat released when urea dissolve. That is the water gained 27.6 kJ, while dissolution of urea released 27.6 kJ. Therefore, the heat gained is equal to the heat lost.

c) From part B, since heat gained is equal to heal lost, then
250 g × (Tf -30) ×4.18 J/g = 27600 J
 = 1045 Tf - 31350J = 27600 J
Tf = 56.41°C.
Therefore the final temperature  of the solution is 56.41°C

d) The initial and final temperature in Fahrenheit
°F = °C × (9/5) +32,
Thus, 30°C will be equal to 86° F
while 56.41 will be equivalent to  133.54 ° F


7 0
2 years ago
Read 2 more answers
When the water level of a stream or river exceeds its natural banks, it has reached its
andre [41]
When the water level of a stream or river exceeds its natural banks, it has reached its D. FLOOD STAGE

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7 0
3 years ago
Can someone help me to answer these Chemistry questions?
Andreyy89
Which ones in specific
3 0
3 years ago
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Ray Of Light [21]
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Hope this helps! :)

3 0
2 years ago
How many grams of carbon monoxide are needed to react with an excess of iron (III) oxide to produce 198.5 grams of iron? Fe2O3(s
erastova [34]

Answer : The grams of carbon monoxide needed are 148.89 g

Solution : Given,

Mass of iron, Fe = 198.5 g

Molar mass of iron, Fe = 56 g/mole

Molar mass of carbon monoxide, CO = 28 g/mole

First we have to calculate the moles of iron, Fe.

\text{ Moles of Fe}=\frac{\text{ Mass of Fe}}{\text{ Molar mass of Fe}}=\frac{198.5g}{56g/mole}=3.545moles

The balanced chemical reaction is,

Fe_2O_3(s)+3CO(g)\rightarrow 3CO_2(g)+2Fe(s)

From the balanced reaction, we conclude that

2 moles of iron produces from the 3 moles of carbon monoxide

3.545 moles of iron produces from the \frac{3}{2}\times 3.545=5.3175 moles of carbon monoxide

Now we have to calculate the mass of carbon monoxide, CO.

\text{ Mass of CO}=\text{ Moles of CO}\times \text{ Molar mass of CO}

\text{ Mass of CO}=(5.3175moles)\times (28g/mole)=148.89g

Therefore, the grams of carbon monoxide needed are 148.89 g

7 0
2 years ago
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